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Chemistry

Give balanced equations for the conversions A and B.

  1. Metallic carbonateA →Ba(NO3)2White precipitateB →dil. HClprecipitate dissolves\text{Metallic carbonate} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{Ba(NO}3)2} \text{White precipitate} \quad \raisebox{0.35em}{B} \space \xrightarrow{\text{dil. HCl}} \text{precipitate dissolves}
  2. Metallic sulphideA →Pb(CH3COO)2 soln.black precipitate \text{Metallic sulphide} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{Pb(CH}3{\text{COO}})2 \text{ soln.}} \text{black precipitate }
  3. Metallic saltA →BaCl2 soln.Barium sulphiteB →dil. HClBarium chloride\text{Metallic salt} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{BaCl}_2 \text{ soln.}} \text{Barium sulphite} \quad \raisebox{0.35em}{B} \space \xrightarrow{\text{dil. HCl}} \text{Barium chloride}
  4. Metallic chlorideA →conc. H2SO4ΔGas evolvedB →AgNO3White precipitate\text{Metallic chloride} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{conc. H}2\text{SO}4\Delta} \text{Gas evolved} \quad \raisebox{0.35em}{B} \space \xrightarrow{\text{AgNO}_3} \text{White precipitate}
  5. Metallic saltA →BaCl2White precipitate insoluble in dil. HCl\text{Metallic salt} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{BaCl}_2} \text{White precipitate insoluble in dil. HCl}

Practical Chemistry

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Answer

  1. Na2CO3 + Ba(NO3)2 ⟶ BaCO3 ↓ [white ppt.] + 2NaNO3
    BaCO3 + 2HCl ⟶ BaCl2 [soluble] + H2O + CO2

  2. Pb(CH3COO)2 [colourless] + H2S ⟶ PbS ↓ [black] + 2CH3COOH

  3. Na2SO3 + BaCl2 ⟶ BaSO3 ↓ [white ppt.] + 2NaCl
    BaSO3 + 2HCl ⟶ BaCl2 [soluble] + H2O + SO2

  4. NaCl + H2SO4 [conc.] →<200°C\xrightarrow{\lt 200 \degree\text{C}} NaHSO4 + HCl
    HCl + AgNO3 ⟶ AgCl ↓ [white ppt.] + HNO3

  5. Na2SO4 + BaCl2 ⟶ BaSO4 ↓ [white ppt.] + 2NaCl

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