Acids, Bases and Salts

(a) What to you understand by the term acid?

(b) Name the positive ion formed when an acid is dissolved in water.

(c) Draw the structure of this ion.

Answer

(a) Acids are defined as compounds which contain one or more hydrogen atoms, and when dissolved in water, they produce hydronium ions (H₃O⁺) as the only positively charged ions.

(b) Hydronium ion (H₃O⁺)

(c) The structure of hydronium ion is shown below:

Write the ionisation of sulphuric acid showing the formation of hydronium ion.

Answer

H₂SO₄ + H₂O ⇌ H₃O⁺ + HSO₄^-

HSO₄^- + H₂O ⇌ H₃O⁺ + SO₄^2-

Water is never added to acid in order to dilute it. Why?

Answer

Water is not added to acid as it is an exothermic process and in this process so much heat is produced that splashing of acidic acid solution may occur, also the container may break which can be fatal to the person.

Define the term 'basicity' of an acid. Give the basicity of: nitric acid, sulphuric acid and phosphoric acid.

Answer

The basicity of an acid is defined as the number of hydronium ions (H₃O⁺) that can be produced by the ionization of one molecule of that acid in aqueous solution.

The basicity of following compounds are:

Basicity of Nitric acid = 1

Basicity of Sulphuric acid = 2

Basicity of Phosphoric acid = 3

Give two examples of each of the following :

(a) oxy-acid

(b) hydracid

(c) tribasic acid

(d) dibasic acid

Answer

(a) Oxyacids — Nitric acid [HNO₃] and Sulphuric acid [H₂SO₄]

(b) Hydracid — Hydrochloric acid [HCl] and Hydrobromic acid [HBr]

(c) Tribasic acid — Phosphoric acid [H₃PO₄] and Citric acid [C₆H₈O₇]

(d) Dibasic acid — Sulphuric acid [H₂SO₄] and Carbonic acid [H₂CO₃]

Name the :

(a) acidic anhydride of the following acids:

1. sulphurous acid
2. nitric acid
3. phosphoric acid
4. carbonic acid

(b) acid present in vinegar, grapes and lemons.

Answer

(a) Below are the acidic anhydride of the given acids:

1. Sulphurous acid — SO₂
2. Nitric acid — N₂O₅
3. Phosphoric acid — P₂O₅
4. Carbonic acid — CO₂

(b) Acids present in following are:

1. Vinegar — Acetic acid
2. Grapes — Tartaric acid
3. Lemon — Citric acid

What do you understand by the statement 'acetic acid is a monobasic acid'?

Answer

Acetic acid is a monobasic acid because it's molecule ionises by liberating only one hydronium ion.

CH₃COOH + H₂O ⇌ H₃O⁺ + CH₃COO^-

Give a balanced equation for :

(i) reaction of nitrogen dioxide with water

(ii) preparation of a non volatile acid from a volatile acid.

Answer

(i) 2NO₂ + H₂O ⟶ HNO₂ + HNO₃

(ii) S + 6HNO₃ ⟶ H₂SO₄ + 2H₂O + 6NO₂

What do you understand by the strength of an acid? On which factor does the strength of an acid depend.

Answer

The strength of an acid is the measure of concentration of hydronium ions [H₃O⁺] produced by that acid in aqueous solution.

Factors on which the strength of an acid depends are:

1. Degree of ionisation (α).
2. Concentration of hydronium ions [H₃O⁺] produced by that acid in aqueous solution.

Explain the following:

(a) Carbonic acid gives an acid salt but hydrochloric acid does not.

(b) Dil. HCl acid is stronger than highly concentrated acetic acid.

(c) H₃PO₃ is not a tribasic acid.

(d) Lead carbonate does not react with dil. HCl

(e) Nitrogen dioxide is a double acid anhydride.

Answer

(a) Carbonic acid is a dibasic acid i.e., it has two replaceable hydrogen ions. Hence, it forms one acid salt or one normal salt. On the other hand, hydrochloric acid is a monobasic acid with one replaceable hydrogen ion. Hence, it forms only one normal salt.

(b) Concentration of an acid means the amount of water present in the acid and not at all the strength of an acid. Strength of an acid is the measure of concentration of hydronium ions it produces in its aqueous solution. Thus, dil. HCl is stronger acid than highly concentrated acetic acid.

(c) H₃PO₃ is not a tribasic acid but dibasic because in oxyacids of phosphorus, hydrogen atoms which are attached to oxygen atoms are replaceable. Hydrogen atoms directly bonded to phosphorus atoms are not replaceable.

(d) Generally, acids liberate carbon dioxide on reaction with metallic carbonates and bicarbonates. But if the salt produced is insoluble, then the reaction does not proceed. So, we do not expect lead carbonate to react with hydrochloric acid.

(e) Nitrogen dioxide is called double acid anhydride because two acids – nitrous acid and nitric acid – are formed when it reacts with water.

    2NO₂ + H₂O ⟶ HNO₂ + HNO₃

How is an acid prepared from a (a) Non-metal (b) salt ? Give an equation for each.

Answer

(a) A non-metal, e.g., sulphur or phosphorous is oxidised by conc. nitric acid to form to form sulphuric acid or phosphoric acid respectively.

S + 6HNO₃ ⟶ H₂SO₄ + 2H₂O + 6NO₂

P + 5HNO₃ ⟶ H₃PO₄ + H₂O + 5NO₂

(b) Normal salts of more volatile acids are displaced by a less or non-volatile acid.

E.g., Both hydrochloric acid and nitric acid are formed by using sulphuric acid [H₂SO₄].

NaCl + H₂SO₄ $\xrightarrow{\space\Delta\space}$ NaHSO₄ + HCl

NaNO₃ + H₂SO₄ $\xrightarrow{\space\Delta\space}$ NaHSO₄ + HNO₃

Give equations to show how the following are made from their corresponding anhydrides.

(a) sulphurous acid

(b) phosphoric acid

(c) carbonic acid

(d) sulphuric acid

Answer

(a) SO₂ + H₂O ⟶ H₂SO₃

(b) P₂O₅ + 3H₂O ⟶ 2H₃PO₄

(c) CO₂ + H₂O ⟶ H₂CO₃

(d) SO₃ + H₂O ⟶ H₂SO₄

Name an acid used:

(a) to flavour and preserve food;

(b) in a drink

(c) to remove ink spots

(d) as an eyewash.

Answer

(a) Citric acid

(b) Carbonic acid

(c) Oxalic acid

(d) Boric acid

Give reaction of acids with

(a) chlorides

(b) nitrates

State the conditions under which they react.

Answer

(a) Chlorides do not react with dilute acids. They react with concentrated sulphuric acid on warming to liberate hydrogen chloride.

$\text{NaCl} + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\lt 200 \degree\text{C}}\text{NaHSO}_4 + \text{HCl}$

$2\text{NaCl} + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\gt 200 \degree\text{C}}\text{Na}_2\text{SO}_4 + 2\text{HCl}$

(b) Nitrates do not react with dilute acids. When heated with conc. sulphuric acid they produce more volatile nitric acid.

$\text{KNO}_3 + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\lt 200 \degree\text{C}}\text{KHSO}_4 + \text{HNO}_3$

$2\text{KNO}_3 + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\gt 200 \degree\text{C}}\text{K}_2\text{SO}_4 + 2\text{HNO}_3$

What do you understand by an alkali? Give two examples of :

(a) strong alkalis

(b) weak alkalis

Answer

An alkali is a base soluble in water. All alkalis form hydroxyl (OH^-) ions in aqueous solution as the only negative ions. They turn red litmus blue.

(a) Strong alkalis — Sodium hydroxide [NaOH], Potassium hydroxide [KOH]

(b) Weak alkalis — Calcium hydroxide [Ca(OH)₂], Ammonium hydroxide [NH₄OH]

What is the difference between :

(a) an alkali and a base,

(b) the chemical nature of an aqueous solution of HCl and an aqueous solution of NH₃

Answer

(a) Difference between an alkali and a base:

(b) Difference between chemical nature of an aq. soln. of HCl and NH₃:

Name the ions furnished by:

(a) bases in solution

(b) an acid

Answer

(a) bases in solution — Hydroxyl ion [OH^-]

(b) an acid — H₃O[⁺] . At first the the hydrogen molecule furnishes hydrogen ion, but this hydrogen ion cannot exist independently. Therefore it combines with water molecule to form hydronium ion H₃O[⁺].

Give one example in case:

(a) A basic oxide which is soluble in water,

(b) A hydroxide which is highly soluble in water,

(c) A basic oxide which is insoluble in water,

(d) A hydroxide which is insoluble in water,

(e) A weak mineral acid

(f) A base which is not an alkali

(g) An oxide which is a base,

(h) A hydrogen containing compound which is not an acid

(i) A base which does not contain a metal ion.

Answer

(a) Sodium oxide [Na₂O]

(b) Sodium hydroxide [NaOH]

(c) Copper (II) oxide [CuO]

(d) Aluminium hydroxide [Al(OH)₃]

(e) Carbonic acid [H₂CO₃]

(f) Ferric hydroxide [Fe(OH)₃]

(g) Copper (II) oxide [CuO]

(h) Ammonia [NH₃]

(i) Ammonium hydroxide [NH₄OH]

You have been provided with three test tubes. One of them contains distilled water and the other two have an acidic solution and a basic solution respectively. If you are given only red litmus paper, how will you identify the contents of each test tube?

Answer

We take three pieces of red litmus paper. The solution which turns red litmus paper to blue is basic solution. Distilled water (neutral) and acidic solution will not effect red litmus paper.

Now we divide the so formed blue litmus paper into two pieces. The test tube containing distilled water does not change the colour of the blue litmus paper.

The test tube containing acidic solution changes the colour of the blue litmus paper to red. Hence, we can identify the three solutions.

HCl, HNO₃, C₂H₅OH, C₆H₁₂O₆ all contain H atoms but only HCl and HNO₃ show acidic character. Why?

Answer

HCl and HNO₃ show acidic character because they ionise in aqueous solution.

Ionisation of HCl in water:

HCl ⟶ H⁺ + Cl^-

H⁺ + H₂O ⟶ H₃O⁺

Ionisation of HNO₃ in water:

HNO₃ ⟶ H⁺ + NO₃^-

H⁺ + H₂O ⟶ H₃O⁺

C₂H₅OH (Ethanol) and C₆H₁₂O₆ (Glucose) are covalent compounds. Their H atoms do not ionise in water to form hydronium ions [H₃O⁺]. Hence, they don't show acidic character.

(a) Dry HCl gas does not change the colour of dry litmus paper. Why?

(b) Is PbO₂ a base or not? Comment.

(c) Do basic solutions also have H⁺(aq.) ? Explain why are they basic by taking an example?

Answer

(a) The colour of litmus paper changes only in presence of ions like hydrogen [H⁺] or hydronium ions [H₃O⁺]. HCl can produce these ions only in the form of aqueous solution. Hence, dry HCl gas does not change the colour of dry litmus paper.

(b) A base reacts with an acid to form salt and water ONLY. The word ONLY is of importance in the definition of a base. Lead oxide reacts with hydrochloric acid to produce lead (II) chloride (a salt) and water, but the word "only" excludes it from the class of bases because chlorine is also produced.

PbO₂(s) + 4HCl(aq.) ⟶ PbCl₂(aq.) + Cl₂(g) + 2H₂O

Thus, PbO₂ is not a base.

(c) Yes, basic solutions have H⁺ ions, but the concentration of OH^- ions is more than the H⁺ ions which makes the solution basic in nature.

Example — Sodium hydroxide (NaOH). It has more OH^- ions than H⁺ ions, so it is basic in nature.

How would you obtain:

(a) a base from another base,

(b) an alkali from a base,

(c) salt from another salt?

Answer

(a) A base from another base can obtained by double decomposition. The aqueous solution of salts with base (alkali) precipitates the respective metallic hydroxide.
For example,

FeCl₃ + 3NaOH ⟶ 3NaCl + Fe(OH)₃ ↓ [red brown ppt.]

(b) An alkali from a base can be obtained by the action of water on soluble metallic oxides like oxides of sodium, potassium and calcium:

CaO + H₂O ⟶ Ca(OH)₂

(c) A salt from another salt can be obtained by adding an alkali to the solutions of the salts of the heavy metals like copper, iron, zinc, etc.
For example,

FeSO₄ [aq.] + 2NaOH [aq.] ⟶ Na₂SO₄ [aq.] + Fe(OH)₂ ↓ [dirty green]

Write balanced equation to satisfy each statement.

(a) Acid + Active metal ⟶ Salt + Hydrogen

(b) Acid + Base ⟶ Salt + Water

(c) Acid + carbonate or bicarbonate ⟶ Salt + water + carbon dioxide

(d) Acid + sulphite or bisulphite ⟶ Salt + water + sulphur dioxide

(e) Acid + sulphide ⟶ Salt + hydrogen sulphide

Answer

(a) Mg + 2HCl ⟶ MgCl₂ + H₂

(b) HCl + NaOH ⟶ NaCl + H₂O

(c) CaCO₃ + 2HCl ⟶ CaCl₂ + H₂O + CO₂

(d) CaSO₃ + 2HCl ⟶ CaCl₂ + H₂O + SO₂

(e) ZnS + 2HCl ⟶ ZnCl₂ + H₂S

The skin has and needs natural oils. Why it is advisable to wear gloves while working with strong alkalis?

Answer

Alkalis react with oil to form soap. Since, our skin contains oil hence when we touch strong alkalis, a reaction takes place and soapy solutions are formed. This reaction can be corrosive for skin. Hence we should wear gloves while working with strong alkalis.

Complete the table:

Answer

Completed table is shown below:

What do you understand by pH value? Two solution X and Y have pH values of 4 and 10 respectively. Which one of these two will give a pink colour with phenolphthalein indicator.

Answer

pH of a solution is the negative logarithm to the base 10 of the hydrogen ion concentration expressed in moles per litre.

The solution with pH value 10 [i.e., Y] will give pink colour with phenolphthalein indicator.

You are supplied with five solutions : A, B, C, D and E with pH values as follows:

A = 1.8, B = 7, C = 8.5, D = 13, and E = 5

Classify these solutions as neutral, slightly or strongly acidic and slightly or strongly alkaline.

Which solution would be most likely to liberate hydrogen with:

(a) magnesium powder

(b) powdered zinc metal. Give a word equation for each reaction.

Answer

A = Strongly acidic

B = neutral

C = slightly alkaline

D = Strongly alkaline

E = slightly acidic

(a) Solution A (acidic solution)

Solution A (acidic solution) + magnesium powder ⟶ Hydrogen + Mg salt

(b) Solution A (acidic solution)

Solution A (acidic solution) + powdered zinc metal ⟶ Hydrogen + Zn salt

Distinguish between :

(a) a common acid base indicator and a universal indicator.

(b) acidity of bases and basicity of acids,

(c) acid and alkali (other than indicator)

Answer

(a) Difference between a common acid base indicator and a universal indicator:

(b) Difference between acidity of bases and basicity of acids:

(c) Difference between acid and alkali (other than indicator):

What should be added to

(a) increase the pH value

(b) decrease the pH value of a neutral solution

Answer

(a) Alkali

(b) Acid

How does tooth enamel get damaged? What should be done to prevent it?

Answer

Substances like chocolates and sweets are degraded by bacteria present in our mouth. When the pH falls to 5.5 tooth decay starts. Tooth enamel is the hardest substance in our body and it gets corroded. The saliva produced by salivary glands is slightly alkaline, it helps to increase the pH, to some extent, but toothpaste which contains basic substance is used to neutralize excess acid in the mouth.

When you use a universal indicator, you see that solutions of different acids produce different colours. Indeed, solutions of the same acid with different concentrations will also give different colours. Why?

Answer

Universal indicators give different colours at different concentrations of hydrogen ions in a solution. The hydrogen ion concentration differs for the same acid with different concentrations. Hence, the universal indicator gives different colours for the same acid with different concentrations.

(a) A solution has a pH of 7. Explain how you would: (i) increase it's pH (ii) decrease it's pH.

(b) If a solution changes the colour of litmus from red to blue, what you can say about it's pH.

(c) What you can say about the pH of a solution, that liberates carbon dioxide from sodium carbonate?

Answer

(a) A solution with pH of 7 is neutral. (i) Increasing it's pH means increasing its basic nature. Hence, we will add alkali to increase it's pH. (ii) Similarly, to decrease it's pH, we will add an acid to the solution.

(b) When a solution changes the colour of litmus from red to blue, it shows it is basic in nature and the pH value will be more than 7.

(c) Acids liberate carbon dioxide on reaction with metallic carbonates and bicarbonates. Hence, the pH of this solution will be less than 7.

Solution P has a pH of 13, solution Q has a pH of 6 and solution R has a pH of 2.

Which solution:

(a) Will liberate ammonia from ammonium sulphate on heating.

(b) is a strong acid?

(c) contains molecules as well as ions?

Answer

(a) Solution P
Reason — When alkalis are warmed with an ammonia salt, ammonia gas is given out.

(b) Solution R
Reason — Number 2 on pH scale represents a strong acid.

(c) Solution Q
Reason — As Q with pH 6 is a weak acid and will not be able to completely dissociate into ions. Hence, will have molecules and ions both.

M is an element in the form of powder. M burns in oxygen and the product obtained is soluble in water. The solution is tested with litmus. Write down only the word which will correctly complete each of the following sentences.

(a) If M is a metal, then the litmus will turn ...............

(b) If M is a non-metal, then the litmus will turn ...............

(c) If M is a reactive metal, then ............... will be evolved when M reacts with dilute sulphuric acid.

(d) If M is a metal, it will form ............... oxide, which will form ............... solution with water.

(e) If M is a non-metal, it will not conduct electricity unless it is in the form of ...............

Answer

(a) If M is a metal, then the litmus will turn blue

(b) If M is a non-metal, then the litmus will turn red

(c) If M is a reactive metal, then hydrogen gas will be evolved when M reacts with dilute sulphuric acid.

(d) If M is a metal, it will form basic oxide, which will form alkaline solution with water.

(e) If M is a non-metal, it will not conduct electricity unless it is in the form of graphite.

Explanation:

(a) Metal, M burns in oxygen to form an oxide. Metallic oxide forms an alkaline solution in water. Hence, turns red litmus blue.

(b) A non-metal on reacting with oxygen produces an acidic oxide. This acidic oxide will turn blue litmus paper blue.

(c) In Simple Displacement reaction, reactive metal and acid react to produce salt and hydrogen gas is evolved.

(d) Metals react with oxygen to form basic oxide which dissolve in water to give alkaline solution.

(e) In Graphite, each carbon atom is bonded to three other carbon atoms. Thus, one electron of carbon remains free. Due to this free valence electron, graphite is a good conductor of electricity. All other non-metals are poor conductors of electricity.

Define the following and give two examples in each case : (a) a normal salt, (b) an acid salt, (c) a basic salt.

Answer

(a) A normal salt — Normal salts are the salts formed by the complete replacement of the ionisable hydrogen atoms of an acid by a metallic or an ammonium ion.
Examples — Sodium Sulphate [Na₂SO₄], Sodium Chloride [NaCl]

(b) An acidic salt — Acid salts are formed by the partial replacement of the ionisable hydrogen atoms of a polybasic acid by a metal or an ammonium ion.
Examples — Sodium Hydrogen Sulphate [NaHSO₄], Disodium Hydrogen Phosphate [Na₂HPO₄]

(c) A basic salt — Basic salts are formed by the partial replacement of the hydroxyl group of a di- or a tri-acidic base by an acid radical.
Examples — Basic lead chloride [Pb(OH)Cl], Basic magnesium chloride [Mg(OH)Cl].

Answer the following questions related to salts and their preparations:

(a) What is a 'salt' ?

(b) What kind of salt is prepared by precipitation?

(c) Name a salt prepared by direct combination. Write an equation for the reaction that takes place in preparing the salt you have named.

(d) Name the procedure used to prepare a sodium salt such as sodium sulphate.

Answer

(a) Salt is a compound formed by the partial or total replacement of the ionisable hydrogen atoms of an acid by a metallic ion or an ammonium ion.

(b) An insoluble salt can be prepared by precipitation.

(c) A salt prepared by direct combination is Lead(II) Sulphide.
Pb + S $\xrightarrow{\space\Delta\space}$ PbS

(d) By neutralisation of alkali (caustic soda) with acid (dilute sulphuric acid):
2NaOH + H₂SO₄ ⟶ Na₂SO₄ + 2H₂O

Explain the following methods with examples:

(a) Direct combination

(b) Displacement

(c) Double decomposition (precipitation)

(d) Neutralization of insoluble base

(e) Neutralization of an alkali (titration)

Answer

(a) In direct combination, a metal and a non-metal are heated together to obtain the corresponding salt.

i.e., Metal + Non-Metal ⟶ Salt

Example:

Pb + S $\xrightarrow{\space\Delta\space}$ PbS

(b) The displacement method involves action of a dilute acid on active metal producing the corresponding salt with the liberation of Hydrogen gas.

i.e., Active metal + Acid ⟶ Salt + Hydrogen

Example :

Zn + H₂SO₄ ⟶ ZnSO₄ + H₂

(c) Double decomposition (precipitation) — A chemical change, in which two compounds in solution react to form two other compounds by the mutual exchange of radicals. A solid precipitate is formed as a result of the reaction.

Example:

Na₂SO₄ + BaCl₂ ⟶ BaSO₄↓ + 2NaCl

(d) Neutralization of insoluble base — By the action of dilute acid on an insoluble base.

Example:

CuO + H₂SO₄ ⟶ CuSO₄ + H₂O

(e) Neutralization of an alkali (titration) — By the action of dilute acid on an alkali (i.e., soluble base):

Example:

2NaOH + H₂SO₄ ⟶ Na₂SO₄ + H₂O

How would you prepare :

(a) copper sulphate crystals from a mixture of charcoal and black copper oxide.

(b) zinc sulphate crystals from zinc dust (powdered zinc and zinc oxide),

(c) sodium hydrogen carbonate crystals.

(d) calcium sulphate from calcium carbonate.

Answer

(a) Copper sulphate crystals from a mixture of charcoal and black copper oxide

Method of preparation: Neutralisation of insoluble base

Reaction:
CuO + H₂SO₄ ⟶ CuSO₄ + H₂O
CuSO₄ + 5H₂O ⟶ CuSO₄.5H₂O (blue vitriol)

Procedure:

1. Take dilute sulphuric acid in a beaker and heat it on wire gauze.
2. Add black cupric oxide in small quantities at a time, with stirring till no more of it dissolves and the excess compound settles to the bottom.
3. Filter it hot and collect the filtrate in a china dish. Evaporate the filtrate by heating to the point of crystallization and then allow it to cool and
4. Collect the bright blue crystals of copper (II) sulphate pentahydrate CuSO₄.5H₂O (blue vitriol) and dry the crystals.

(b) Zinc sulphate crystals from Zinc dust

Method of preparation: Displacement — By the action of dilute acid (dil. H₂SO₄) on an active metal (Zinc, Iron).

Reaction:
Zn(s) + H₂SO₄(aq) ⟶ ZnSO₄ + H₂↑
ZnSO₄ + 7H₂O ⟶ ZnSO₄.7H₂O (white vitriol)

Procedure:

1. Take dilute sulphuric acid in a beaker and heat it on a wire gauze. Add some granulated zinc pieces with constant stirring.
2. Effervescence take place because of the liberation of hydrogen gas.
   Add zinc till the Zinc settles at the base of the beaker.
   When effervescence stops, it indicates that all the acid has been used up.
3. The excess of zinc is filtered off.
4. Collect the solution in a china dish and evaporate the solution to get crystals. Filter, wash them with water and dry them between the folds of a filter paper. The white, needle-shaped crystals are of hydrated Zinc sulphate.

(c) Sodium hydrogen carbonate crystals:

Method of preparation: By passing carbon dioxide gas into a cold solution of sodium carbonate.

Reaction:
Na₂CO₃ + CO₂ + H₂O ⟶ 2NaHCO₃

Procedure:

1. Dissolve 5 grams of anhydrous sodium carbonate in about 25 cm³ of distilled water in a flask.
2. Cool the solution by keeping the flask in a freezing mixture.
3. Pass carbon dioxide gas in the solution.
4. Crystals of sodium bicarbonate will precipitate out after some time.
5. Filter the crystals and dry it in the folds of filter paper.

(d) calcium sulphate from calcium carbonate.

Method of preparation: By Double Decomposition (precipitation)

Reaction:
CaCO₃ + 2HNO₃ ⟶ Ca(NO₃)₂ + H₂O + CO₂↑
Ca(NO₃)₂ + Na₂SO₄ ⟶ CaSO₄↓ + 2NaNO₃

Procedure:

1. First insoluble Calcium Carbonate [CaCO₃] is converted to soluble Calcium Nitrate [Ca(NO₃)₂] with the help of dilute nitric acid.
2. The resulting solution is then treated with Sodium Sulphate [Na₂SO₄] and a precipitate of Calcium Sulphate is obtained.

The following is a list of methods for the preparation of salts:

A — direct combination of two elements

B — reaction of a dilute acid with a metal

C — reaction of a dilute acid with an insoluble base

D — titration of a dilute acid with a solution of soluble base.

E — reaction of two solutions of salts to form a precipitate.

Choose from the list A to E, the best method of preparing the following salts by giving a suitable equation in each case:

1. Anhydrous ferric chloride
2. Lead chloride
3. Sodium sulphate
4. Copper sulphate

Answer

1. Anhydrous ferric chloride — A. (Direct combination of two elements)
   2Fe + 3Cl₂ ⟶ 2FeCl₃
2. Lead chloride — E. (Reaction of two solutions of salts to form a precipitate)
   Pb(NO₃)₂ + 2NaCl ⟶ PbCl₂ + 2NaNO₃
3. Sodium sulphate — D. (Titration of dilute acid with a solution of soluble base)
   2NaOH + H₂SO₄ ⟶ Na₂SO₄ + 2H₂O
4. Copper sulphate — C. (reaction of a dilute acid with an insoluble base)
   Cu(OH)₂ + H₂SO₄ ⟶ CuSO₄ + 2H₂O

Name:

(a) a chloride which is insoluble in cold water but dissolves in hot water,

(b) a chloride which is insoluble

(c) two sulphates which are insoluble

(d) a basic salt,

(e) an acidic salt,

(f) a mixed salt,

(g) a complex salt,

(h) a double salt.

Answer

(a) a chloride which is insoluble in cold water but dissolves in hot water - Lead Chloride [PbCl₂]

(b) a chloride which is insoluble - Silver chloride [AgCl]

(c) two sulphates which are insoluble - Barium sulphate [BaSO₄] and Lead Sulphate [PbSO₄]

(d) a basic salt - Basic lead chloride [Pb(OH)Cl]

(e) an acidic salt - Sodium hydrogen sulphate [NaHSO₄]

(f) a mixed salt - Sodium potassium carbonate [NaKCO₃]

(g) a complex salt - Sodium zincate [Na₂ZnO₂]

(h) a double salt - Dolomite [CaCO₃.MgCO₃]

Fill in the blanks with suitable words :

An acid is a compound which when dissolved in water forms hydronium ions as the only ............... ions. A base is a compound which is soluble in water contains ............... ions. A base reacts with an acid to form a ............... and water only. This type of reaction is known as ................

Answer

An acid is a compound which when dissolved in water forms hydronium ions as the only positively charged ions. A base is a compound which is soluble in water and contains O₂^- ions. A base reacts with an acid to form a salt and water only. This type of reaction is known as neutralisation.

What would you observe when:

(a) blue litmus is introduced into a solution of hydrogen chloride gas.

(b) red litmus paper is introduced into a solution of ammonia in water,

(c) red litmus paper is introduced in caustic soda solution?

Answer

(a) Blue litmus will turn into red showing acidic nature of solution.

(b) Red litmus will turn into blue showing alkaline nature of ammonia.

(c) Red litmus will turn into blue showing basic nature of solution.

Explain why :

(a) it is necessary to find out the ratio of reactants required in the preparation of sodium sulphate,

(b) fused calcium chloride is used in the preparation of FeCl₃

(c) Anhydrous FeCl₃ cannot be prepared by heating hydrated Iron (III) chloride.

Answer

(a) Since sodium hydroxide and sulphuric acid both are soluble, an excess of either of them cannot be removed by filtration. Therefore, it is necessary to find out on a small scale, the ratio of the solutions of the two reactants required for complete neutralisation before preparation.

(b) Iron (III) Chloride (FeCl₃) is highly deliquescent. So, to keep it dry fused calcium chloride is used which is a drying agent.

(c) Anhydrous FeCl₃ cannot be prepared by heating the hydrated Iron (III) chloride (FeCl₃.6H₂O) because on heating, FeCl₃.6H₂O produces Fe₂O₃, H₂O, HCl.

2[FeCl₃.6H₂O] $\xrightarrow{\space\Delta\space}$ Fe₂O₃ + 9H₂O + 6HCl

Give the preparation of the salt shown in the left column by matching with the methods given in the right column. Write a balanced equation for each preparation.

Answer

Zinc Sulphate — Displacement
Zn + H₂SO₄ ⟶ ZnSO₄ + H₂

Ferrous sulphide — Synthesis
Fe + S ⟶ FeS

Barium sulphate — Precipitation
Na₂SO₄ + BaCl₂ ⟶ BaSO₄ ↓ + 2NaCl

Ferric Sulphate — Displacement
Fe + H₂SO₄ ⟶ FeSO₄ + H₂

Sodium sulphate — Neutralisation
2NaOH + H₂SO₄ ⟶ Na₂SO₄ + 2H₂O

Give the pH value of pure water. Does it change if common salt is added to it.

Answer

pH of pure water is 7. No, it does not change when common salt is added.

Common salt is sodium chloride (NaCl). It is a salt derived from a strong acid (HCl) and strong base (NaOH) hence it gives a neutral solution with water.

Classify the following solutions as acids, bases or salts.

Ammonium hydroxide, barium chloride, sodium chloride, sodium hydroxide, H₂SO₄ and HNO₃

Answer

Acids — H₂SO₄ and HNO₃

Bases — Ammonium hydroxide and sodium hydroxide.

Salts — Barium chloride and sodium chloride.

Define the term neutralisation :

(a) Give a reaction, mentioning clearly acid and base used in the reaction,

(b) If one mole of a strong acid reacts with one mole of a strong base, the heat produced is always the same. Why?

Answer

Neutralisation is the process by which [H⁺] ions of an acid react completely with the [OH^- ] ions of a base to give salt and water only.

(a) Base + Acid ⟶ Salt + water
NaOH + HCl ⟶ NaCl + H₂O
In the above neutralisation reaction Sodium Hydroxide (NaOH) is the base and Hydrochloric acid (HCl) is the acid.

(b) When one mole of a strong acid reacts with one mole of a strong base, the number of [H⁺] and [OH^-] ions produced is always same. Hence the heat of neutralization of a strong acid with strong base is always same.

Write the balanced equations for the preparation of the following salts in the laboratory.

(a) A soluble sulphate by the action of an acid on an insoluble base,

(b) An insoluble salt by the action of an acid on another salt,

(c) An insoluble base by the action of a soluble base on a soluble salt,

(d) A soluble sulphate by the action of an acid on a metal.

Answer

(a) CuO + H₂SO₄ ⟶ CuSO₄ + H₂O

(b) AgNO₃ + HCl ⟶ AgCl ↓ + HNO₃

(c) FeCl₃ + 3NaOH [base] ⟶ 3NaCl + Fe(OH)₃ ↓

(d) Zn + H₂SO₄ ⟶ ZnSO₄ + H₂↑

You are provided with the following chemicals:

NaOH, Na₂CO₃, H₂O, Zn(OH)₂, CO₂, HCl, Fe, H₂SO₄, Cl₂, Zn.

Using the suitable chemicals from the given list only, state briefly how you would prepare :

(a) iron (III) chloride

(b) sodium sulphate

(c) sodium zincate

(d) iron (II) sulphate

(e) sodium chloride

Answer

(a) Iron (III) Chloride: By synthesis i.e., direct combination of elements.
2Fe + 3Cl₂ ⟶ 2FeCl₂

(b) Sodium sulphate: By neutralisation of an alkali (caustic soda) with acid (dilute sulphuric acid)
2NaOH + H₂SO₄ ⟶ Na₂SO₄ + 2H₂O

(c) Sodium zincate: By the action of metals with alkalis
Zn + 2NaOH ⟶ Na₂ZnO₂ + H₂

(d) Iron (II) sulphate: Method of Simple Displacement by the action of dilute acid (H₂SO₄) on an active metal (iron).
Fe + H₂SO₄ (dil.) ⟶ FeSO₄ + H₂

(e) Sodium chloride: By the neutralisation reaction of strong acid (HCl) with strong base (NaOH) also known as titration NaOH + HCl ⟶ NaCl + H₂O

For each of the salt : A, B, C and D, suggest a suitable method of it's preparation.

(a) A is a sodium salt,

(b) B is an insoluble salt,

(c) C is a soluble salt of copper

(d) D is a soluble salt of zinc.

Answer

(a) By neutralisation:
NaOH + HCl ⟶ NaCl + H₂O

(b) By precipitation:
AgNO₃ + HCl ⟶ AgCl + HNO₃

(c) By Neutralisation :
Cu(OH)₂ + H₂SO₄⟶ CuSO₄ + 2H₂O

(d) Simple displacement:
Zn + H₂SO₄ ⟶ ZnSO₄ + H₂↑

Choosing only substances from the list given in the box below, write equations for the reactions which you would use in the laboratory to obtain:

(a) Sodium sulphate

(b) Copper sulphate

(c) Iron (II) sulphate

(d) Zinc carbonate

Answer

a. Na₂CO₃ + H₂SO₄ (dil.) ⟶ Na₂SO₄ + H₂O + CO₂↑

b. CuCO₃ + H₂SO₄ (dil.) ⟶ CuSO₄ + H₂O + CO₂↑

c. Fe + H₂SO₄ (dil.) ⟶ FeSO₄ + H₂↑

d. Zn + H₂SO₄ (dil.) ⟶ ZnSO₄ + H₂↑
    ZnSO₄ + Na₂CO₃ ⟶ ZnCO₃ + Na₂SO₄

From the formula listed below, choose one, in each case, corresponding to the salt having the given description :

AgCl, CuCO₃, CuSO₄.5H₂O, KNO₃, NaCl, NaHSO₄, Pb(NO₃)₂, ZnCO₃, ZnSO₄.7H₂O

(a) an acid salt.

(b) an insoluble chloride.

(c) on treating with concentrated sulphuric acid, this salt changes from blue to white.

(d) on heating, this salt changes from green to black.

(e) this salt gives nitrogen dioxide on heating.

Answer

(a) NaHSO₄

(b) AgCl

(c) CuSO₄.5H₂O

(d) CuCO₃

(e) Pb(NO₃)₂

(a) Ca(H₂PO₄)₂ is an example of compound called ............... (acid salt / basic salt / normal salt).

(b) Write the balanced equation for the reaction of :
A named acid and a named alkali.

Answer

(a) Ca(H₂PO₄)₂ is an example of compound called acid salt

(b) NaOH + HCl ⟶ NaCl + H₂O

State the terms defined by the following sentences:

(a) A soluble base

(b) The insoluble solid formed when two solution are mixed together.

(c) An acidic solution in which there is only partial ionization of the solute molecules.

Answer

(a) Alkali

(b) Precipitate

(c) Weak acid

Which of the following methods A, B, C, D or E is generally used for preparing the chlorides listed below from (i) to (v). Answer by writing down the chloride and the letter pertaining to the corresponding method. Each letter is to be used only once.

Answer

The methods for preparation of the given chlorides are listed below:

Choose the most appropriate answer from

[SO₂, SiO₂, Al₂O₃, CO, MgO, Na₂O]

(a) A covalent oxide of a metalloid

(b) An oxide which when dissolved in water form acid.

(c) A basic oxide

(d) An amphoteric oxide

Answer

(a) SiO₂

(b) SO₂

(c) Na₂O

(d) Al₂O₃

Complete the following table and write one equation for each to justify the statement:

Answer

Completed table along with the equations is given below:

What do you understand by the water of crystallisation?

Give four substances which contain water of crystallisation and write their common names.

Answer

It is the amount of water molecules which enter into loose chemical combination with the salts and can be driven out by heating the crystals above 100°C.

(a) Define efflorescence. Give examples.

(b) Define deliquescence. Give examples.

Answer

(a) Efflorescence is the property of some salts to loose wholly or partly their water of crystallisation when their crytals are exposed to dry air even for a short time.

Examples: MgSO₄.7H₂O (Epsom salt) , Na₂SO₄.10H₂O (Glauber's salt).

(b) Certain water-soluble substances, when exposed to the atmosphere at ordinary temperature, absorb moisture from the atmospheric air to become moist and ultimately dissolve in the absorbed water, forming a saturated solution. The phenomenon is called deliquescence and the salts are called deliquescent.

Examples: Caustic soda (NaoH), Caustic potash (KOH)

Answer the questions below, relating your answers only to salts in the following list: Sodium chloride, anhydrous calcium chloride, copper sulphate-5-water?

(a) What name is given to the water in the compound copper sulphate-5-water?

(b) If copper sulphate-5-water is heated, anhydrous copper sulphate is formed. What is it's colour?

(c) By what means, other than heating, could you dehydrate copper sulphate-5-water and obtain anhydrous copper sulphate?

(d) Which one of the salts in the given list is deliquescent?

Answer

(a) Water of crystallization

(b) White

(c) By adding concentrated sulphuric acid which acts as a dehydrating agent.

(d) Anhydrous calcium chloride.

State your observation when the following are exposed to the atmosphere:

(a) Washing soda crystals

(b) Iron (III) chloride salts.

Answer

(a) When washing soda (Na₂CO₃.10H₂O) is exposed to air, it loses 9 molecules of water to form a monohydrate.

Na₂CO₃.10H₂O $\xrightarrow{\space\text{dry air}\space}$ Na₂CO₃.H₂O + 9H₂O

(b) When Iron (III) chloride (FeCl₃) is exposed to the atmosphere at ordinary temperature, it absorbs moisture from the atmospheric air to become moist and ultimately dissolve in the absorbed water, forming a saturated solution.

Give reasons for the following:

(a) Sodium hydrogen sulphate is not an acid, but it dissolves in water to give hydrogen ions according to the equation

NaHSO₄ ⇌ H⁺ + Na⁺ + SO₄^2-

(b) Anhydrous calcium chloride is used in a desiccator.

Answer

(a) Sodium hydrogen sulphate [NaHSO₄] is not an acid but due to the partial replacement of the replaceable hydrogen ion in a dibasic acid [H₂SO₄] releases a [H⁺] ion. Thus, we get the above equation.

Therefore, on dissolving in water, it gives hydrogen ions.

(b) Desiccating agents are used to absorb moisture. Anhydrous calcium chloride (CaCl₂) has the capacity to absorb moisture as it is hygroscopic hence used as a desiccating agent.

Explain clearly how conc. H₂SO₄ is used as a dehydrating as well as a drying agent.

Answer

Conc. sulphuric acid is hygroscopic in nature and can remove moisture from other substances; therefore, it is used as a drying agent.

Conc. sulphuric acid can remove water molecules from blue vitriol (CuSO₄.5H₂O), so it is a dehydrating agent as well.

Distinguish between drying and dehydrating agent.

Answer

State whether a sample of each of the following would increase or decrease in mass if exposed to air.

(a) Solid NaOH

(b) Solid CaCl₂

(c) Solid Na₂CO₃.10H₂O

(d) Conc. Sulphuric acid

(e) Iron (III) Chloride

Answer

(a) Increase

(b) Increase

(c) Decrease

(d) Increase

(e) Increase

Explanation — Efflorescent substances lose their weight while hygroscopic and deliquescent substances gain weight when exposed to atmosphere. Solid NaOH, Solid CaCl₂ and Iron (III) Chloride (FeCl₃) are deliquescent substances while Conc. Sulphuric acid is hygroscopic hence they gain weight when exposed to air. Solid Na₂CO₃.10H₂O is an efflorescent substance hence it loses weight.

(a) Why does common salt get wet during the rainy season?

(b) How can this impurity be removed?

(c) Name a substance which changes the blue colour of copper sulphate crystals to white.

(d) Name two crystalline substances which do not contain water of crystallisation.

Answer

(a) Common salt gets wet during the rainy season, as it is deliquescent and absorbs moisture from the atmosphere. Though pure sodium chloride is not deliquescent, the commercial version of the salt contains impurities like, magnesium chloride and calcium chloride which are deliquescent substances.

(b) The impurity can be removed by passing a current of dry hydrogen chloride gas through a saturated solution of the affected salt. Pure sodium chloride is produced as a precipitate which can be recovered by filtering and washing first with a little water and finally with alcohol.

(c) Conc. sulphuric acid

(d) Common salt and sugar

Name the salt which on hydrolysis forms

(a) Acidic

(b) Basic and

(c) Neutral solution.

Give a balanced equation for each reaction.

Answer

(a) Iron chloride(FeCl₃)

FeCl₃ + 3H₂O ⟶ 3HCl + Fe(OH)₃

(b) Ammonium acetate (CH₃COONH₄)

CH₃COONH₄ + H₂O ⟶ CH₃COOH + NH₄OH

(c) Sodium chloride

NaCl + H₂O ⟶ NaOH + HCl

State the change noticed when blue litmus and red litmus are introduced in the following solutions:

(a) Na₂CO₃ solution

(b) NaCl solution

(c) NH₄NO₃

(d) MgCl₂ Solution

Answer

(a) Na₂CO₃ solution — Red litmus changes to blue as Na₂CO₃ gives alkaline solution.

(b) NaCl solution — No change in the colour of the litmus paper as NaCl solution is neutral.

(c) NH₄NO₃ — Acidic so blue litmus changes to red.

(d) MgCl₂ — Blue litmus changes to red showing acidic nature.

Write the balanced equations for the preparation of the following compounds (as the major product) starting from iron and using only one other substance :

(a) Iron (II) chloride

(b) Iron (III) chloride

(c) Iron (II) sulphate

(d) Iron (II) sulphide

Answer

(a) Fe + 2HCl (dil) ⟶ FeCl₂ + H₂↑

(b) 2Fe (heated) + 3Cl₂ (dry) ⟶ 2FeCl₃

(c) Fe + H₂SO₄ (dil) ⟶ FeSO₄ + H₂↑

(d) Fe + S $\xrightarrow{\space\Delta\space}$ FeS

Write balanced reactions for the following conversions (A,B,C,D)

$\text{Fe} \xrightarrow{\text{A}} \text{FeCl}_2 \xrightarrow{\text{B}} \text{FeCO}_3 \xrightarrow{\text{C}} \text{Fe}(\text{NO}_3)_2 \xrightarrow{\text{D}} \text{Fe(OH)}_2$

Answer

A = HCl

B = Na₂CO₃

C = HNO₃

D = NaOH

A: Fe + 2HCl ⟶ FeCl₂ + H₂ ↑

B: FeCl₂ + Na₂CO₃ ⟶ FeCO₃ + 2NaCl

C: FeCO₃ + 2HNO₃ ⟶ Fe(NO₃)₂ + H₂O + CO₂

D: Fe(NO₃)₂ + 2NaOH ⟶ Fe(OH)₂ + 2NaNO₃

The preparation of lead sulphate from lead carbonate is a two step process. (lead sulphate cannot be prepared by adding dilute sulphuric acid to lead carbonate.)

(a) What is the first step that is required to prepare lead sulphate from lead carbonate?

(b) Write the equation for the reaction that will take place when this first step is carried out.

(c) Why is the direct addition of dilute sulphuric acid to lead carbonate an impractical method of preparing lead sulphate?

Answer

(a) The first step is to convert insoluble lead carbonate into soluble lead nitrate by treating lead carbonate with dilute nitric acid.

(b) PbCO₃ (s) + 2HNO₃(dil) ⟶ Pb(NO₃)₂ (aq) + H₂O (l) + CO₂

(c) Adding dilute sulphuric acid (H₂SO₄) to lead carbonate (PbCO₃) in order to prepare lead sulphate (PbSO₄) is an impractical method because an insoluble crust of lead sulphate is formed on lead carbonate which prevents further reaction.

What are the terms defined by the following:

(i) A salt containing a metal ion surrounded by other ions or molecules,

(ii) A base which is soluble in water.

Answer

(i) Complex salts

(ii) Alkali

Making use only of substances chosen from those given below:

Give the equations for the reactions by which you could obtain:

(i) hydrogen

(ii) sulphur dioxide

(iii) carbon dioxide

(iv) zinc carbonate (two steps required)

Answer

Equations for the reactions are :

(i) Zn + H₂SO₄ ⟶ ZnSO₄ + H₂↑

(ii) Na₂SO₃ + 2HCl ⟶ 2NaCl + H₂O + SO₂↑

(iii) Na₂CO₃ + H₂SO₄ $\xrightarrow{\space\Delta\space}$ Na₂SO₄ + H₂O + CO₂↑

(iv) Zn + H₂SO₄ ⟶ ZnSO₄ + H₂↑

ZnSO₄ + Na₂CO₃ ⟶ Na₂SO₄ + ZnCO₃

The acid which contains four hydrogen atoms —

1. Formic acid
2. Sulphuric acid
3. Nitric acid
4. Acetic acid

Answer

Acetic acid contains four hydrogen atoms.

A black coloured solid which on reaction with dilute sulphuric acid forms a blue coloured solution is:

1. Carbon
2. Manganese [IV] oxide
3. Lead [II] oxide
4. Copper [II] oxide

Answer

Copper [II] oxide
Reason — Copper [II] oxide is black in colour and the following reaction takes place when it is treated with dilute sulphuric acid —

CuO + H₂SO₄ ⟶ CuSO₄ + H₂O

CuSO₄ is a blue coloured soln.

Solution A is a strong acid
Solution B is a weak acid
Solution C is a strong alkali

(i) Which solution contains solute molecules in addition to water molecules?

(ii) Which solution will give a gelatinous white precipitate with zinc sulphate, the precipitate disappears in excess.

(iii) Give example of a soln. of a weak alkali.

Answer

(i) Solution B — weak acid
Reason — Weak Acid is an acid which dissociates only partially in aqueous solution thereby producing a low concentration of hydrogen [H⁺] ions [or H₃O⁺ ions]. For example — CH₃COOH ⇌ CH₃COO^- + H⁺ [contains molecules and ions]

(ii) Solution C — strong alkali
Reason — Alkalis react with certain salt solutions to precipitate insoluble hydroxide. Hence,
ZnSO₄ + 2NaOH ⟶ Na₂SO₄ + Zn(OH)₂ [gelatinous white precipitate]

(iii) Ammonium hydroxide (NH₄OH)

Write the equation[s] for the reaction[s] to prepare lead sulphate from lead carbonate.

Answer

PbCO₃ + 2HNO₃ ⟶ Pb(NO₃)₂ + H₂O + CO₂

Pb(NO₃)₂ + Na₂SO₄ ⟶ PbSO₄ + 2NaNO₃

Define the following terms — Neutralization

Answer

Neutralization — It is the process due to which [H⁺] ions of an acid react completely or combine with [OH^-] ions of a base to give salt and water only.

Acid + Base ⟶ Salt + Water

HCl + NaOH ⟶ NaCl + H₂O

H⁺Cl^- + Na⁺OH^- ⟶ Na⁺Cl^- + H₂O

[H⁺ (aq) + OH^- (aq) ⇌ H₂O (l)]

The diagram given below is to prepare Iron [III] chloride in the laboratory.

(i) What is substance B.

(ii) What is the purpose of B.

(iii) Why is iron[III] chloride to be stored in a closed container.

(iv) Write the equation for the reaction between iron and chlorine.

Answer

(i) Substance B is fused calcium chloride.

(ii) Iron (III) chloride is highly deliquescent so it is kept dry with the help of B [fused calcium chloride (drying agent)]

(iii) Iron[III] chloride is to be stored in a closed container because iron (III) chloride is highly deliquescent and it absorbs moisture from the surrounding air to form a saturated solution.

(iv) 2Fe (heated) + 3Cl₂ (dry) ⟶ 2FeCl₃

Select the correct answer from A, B, C, D and E —

A: Nitroso Iron [II] sulphate

B: Iron [III] chloride

C: Chromium sulphate

D: Lead [II] chloride

E: Sodium chloride.

(i) A deliquescent compound

(ii) A compound soluble in hot water but insoluble in cold water.

(iii) A compound which in the aqueous solution state, is neutral in nature.

Answer

(i) B: Iron [III] chloride

(ii) D: Lead [II] chloride

(iii) E: Sodium chloride

Select the correct answer from A, B, C and D –

(i) A weak organic acid is:

1. Formic acid
2. Sulphuric acid
3. Nitric acid
4. Hydrochloric acid

(ii) A complex salt is :

1. Zinc sulphate
2. Sodium hydrogen sulphate
3. Iron (II) ammonium sulphate
4. Tetrammine copper (II) sulphate

Answer

(i) Formic acid

(ii) Tetrammine copper (II) sulphate

Give an equation for the conversions A to E —

Answer

(i) ZnSO₄ + Na₂CO₃ ⟶ Na₂SO₄ + ZnCO₃ ↓

(ii) ZnCO₃ + 2HNO₃ ⟶ Zn(NO₃)₂ + H₂O + CO₂ ↑

(iii) Zn(NO₃)₂ + 2NaOH ⟶ Zn(OH)₂ + 2NaNO₃

(iv) Zn(OH)₂ $\xrightarrow{\space\Delta\space}$ ZnO + H₂O

(v) ZnO + H₂SO₄ ⟶ ZnSO₄ + H₂O

For the preparation of the following salts - give a balanced equation in each case:

1. Copper [II] sulphate from Copper [II] oxide.
2. Iron [III] chloride from the metal iron.
3. Potassium sulphate from KOH soln.
4. Lead [II] chloride from lead carbonate [give two equations].

Answer

1. CuO + H₂SO₄ ⟶ CuSO₄ + H₂O

2. 2Fe + 3Cl₂ ⟶ 2FeCl₃

3. 2KOH + H₂SO₄ [dil.] ⟶ K₂SO₄ + 2H₂O

4. PbCO₃ + 2HNO₃ ⟶ Pb(NO₃)₂ + H₂O + CO₂ ↑
   Pb(NO₃)₂ + 2NaCl ⟶ 2NaNO₃ + PbCl₂

Write the balanced chemical equation — Lead nitrate solution is added to sodium chloride solution

Answer

Pb(NO₃)₂ + 2NaCl ⟶ PbCl₂ ↓ + 2NaNO₃

State what happens to the crystals of washing soda when exposed to air. Name the phenomenon exhibited.

Answer

When crystals of washing soda are exposed to air, it loses its water of crystallisation and the phenomenon is known as Efflorescence.

Name the method used for the preparation of the following salts from the list given below –

(i) Sodium nitrate

(ii) Iron (III) chloride

(iii) Lead chloride

(iv) Zinc sulphate

(v) Sodium hydrogen sulphate.

List:

A : Simple displacement
B : Neutralization
C : Decomposition by acid
D : Double decomposition
E : Direct synthesis

Answer

(i) Sodium nitrate — B : Neutralization

(ii) Iron (III) chloride — E : Direct synthesis

(iii) Lead chloride — D : Double decomposition

(iv) Zinc sulphate — A : Simple displacement

(v) Sodium hydrogen sulphate — C : Decomposition by acid

Match the following:

Answer

State your observation : zinc granule is added to copper sulphate solution.

Answer

Zinc displaces copper to form zinc sulphate and thus copper gets deposited and the blue coloured solution becomes colourless.

Zn + CuSO₄ ⟶ Cu + ZnSO₄

Give a balanced equation for the reaction: Silver nitrate solution and sodium chloride solution.

Answer

AgNO₃ + NaCl ⟶ NaNO₃ + AgCl ↓

Select the word/s given below which are required to correctly complete the blanks — [ammonia, ammonium carbonate, carbon dioxide, hydrogen, hydronium, hydroxide, precipitate, salt water] :

(i) A solution M turns blue litmus red, so it must contain (i) ............... ions ; another solution O turns red litmus blue and hence, must contain, (ii) ............... ions.

(ii) When solution M and O are mixed together, the prod­ucts will be (iii) ............... and (iv) ............... .

(iii) If a piece of magnesium was put into a solution M, (v) ............... gas would be evolved.

Answer

(i) A solultion M turns blue litmus red, so it must contain (i) hydronium ions ; another solution O turns red litmus blue and hence, must contain, (ii) hydroxide ions.

(ii) When solution M and O are mixed together, the prod­ucts will be (iii) salt and (iv) water.

(iii) If a piece of magnesium was put into a solution M, (v) hydrogen gas would be evolved.

Give a suitable chemical term for:

(i) A salt formed by incomplete neutralisation of an acid by a base.

(ii) A definite number of water molecules bound to some salts.

(iii) The process in which a substance absorbs moisture from the atmospheric air to become moist and ultimately dissolves in the absorbed water.

Answer

(i) Acid salt

(ii) Water of crystallization

(iii) Deliquescence

Choosing the substances from the list given:

dil. Sulphuric acid, Copper, Iron, Sodium, Copper (II) carbonate, Sodium carbonate, Sodium chloride, Zinc nitrate

Write balanced equations for the reactions which would be used in the laboratory to obtain the following salts:

1. Sodium sulphate
2. Zinc carbonate
3. Copper (II) sulphate
4. Iron (II) sulphate.

Answer

1. Sodium sulphate
   Na₂CO₃ + H₂SO₄ (dil.) ⟶ Na₂SO₄ + H₂O + CO₂

2. Zinc carbonate
   Zn(NO₃)₂ + Na₂CO₃⟶ 2NaNO₃ + ZnCO₃

3. Copper (II) sulphate
   CuCO₃ + H₂SO₄ (dil.) ⟶ CuSO₄ + H₂O + CO₂

4. Iron (II) sulphate
   Fe + H₂SO₄ (dil.) ⟶ FeSO₄ + H₂

Which one of the following will not produce acid with water

(i) CO

(ii) CO₂

(iii) NO₂

(iv) SO₃

Answer

CO

Reason
Carbon monoxide reacts with water to form carbon dioxide and releases hydrogen gas. Hence, acid is not formed.

CO + H₂O ⟶ CO₂ + H₂

Fill in the blank from the choices given:

The basicity of acetic acid is ............... [3, 1, 4].

Answer

The basicity of acetic acid is 1.

Draw the structure of the stable positive ion formed when an acid dissolves in water.

Answer

Hydronium ion is the stable positive ion formed when an acid dissolves in water. Its structure is shown below:

State the inference drawn from the observation:

Salt S is prepared by reacting dilute sulphuric acid with copper oxide. Identify S.

Answer

Salt S is Copper sulphate CuSO₄

CuO + H₂SO₄ (dil.) ⟶ CuSO₄ + H₂O

Give balanced chemical equations for the preparation of the following salts:

1. Lead sulphate — from lead carbonate.
2. Sodium sulphate — using dilute sulphuric acid.
3. Copper chloride — using copper carbonate.

Answer

1. Lead sulphate from lead carbonate.
   PbCO₃ + 2HNO₃ ⟶ Pb(NO₃)₂ + H₂O + CO₂
   Pb(NO₃)₂ + Na₂SO₄ ⟶ 2NaNO₃ + PbSO₄

2. Sodium sulphate using dilute sulphuric acid.
   Na₂CO₃ + H₂SO₄(dil.) ⟶ Na₂SO₄ + H₂O+ CO₂

3. Copper chloride using copper carbonate.
   CuCO₃ + 2HCl (dil) ⟶ CuCl₂ + H₂O + CO₂

From the list of salts — AgCl, MgCl₂, NaHSO₄, PbCO₃, ZnCO₃, KNO₃, Ca(NO₃)₂

Choose the salt that most appropriately fits the description given below :

(i) a deliquescent salt

(ii) an insoluble chloride.

Answer

(i) MgCl₂

(ii) AgCl

From — Na₂O, SO₂, SiO₂, Al₂O₃, MgO, CO — Select an oxide which dissolves in water forming an acid.

Answer

SO₂

The following reaction takes place.

SO₂ + H₂O ⟶ H₂SO₃

Match the salts given in column I with their method of preparation given in column II.

Answer