Question 1ACIDS — Ions present in acidsComplete and balance the equationsa. Definition — Dissolves in water yielding hydronium ions 1. Hydrochloric acidHCl ⇌ ............... + Cl-[H+ + H2O ⇌ ............... ]HCl + H2O ⇌ ............... + ...............2. Nitric acidHNO3 + H2O ⇌ ............... + ...............3. Sulphuric acidH2SO4 + H2O ⇌ ............... + ...............b. Classification 4. Monobasic acid [Basicity = 1 ]HCl [aq.] ⇌ ............... + ...............5. Dibasic acid [Basicity = 2]H2SO4 [aq.] ⇌ ............... + ...............6. Tribasic acid [Basicity = 3]H3PO4 [aq.] ⇌ ............... + ...............c. Preparation of acids 7. From non-metalsH2 + Cl2 ⟶ ...............8. From acidic oxidesCO2 + H2O ⟶ ............... SO3 + H2O ⟶ ............... P2O5 + H2O ⟶ ...............9. From normal saltsKNO3 + H2SO4 ⟶ ............... + ............... NaCl+ H2SO4 ⟶ ............... + ...............10. By oxidation of non-metalsS + HNO3 ⟶ ............... + H2O ............... [g]d. Properties of acids 11. Neutralizes basesCuO + H2SO4 ⟶ ............... + ............... NaOH + HCl ⟶ ............... + ...............Reaction with12. Chlorides and nitratesNaCl+H2SO4[conc.]→

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Question 1ACIDS — Ions present in acidsComplete and balance the equationsa. Definition — Dissolves in water yielding hydronium ions 1. Hydrochloric acidHCl ⇌ ............... + Cl-[H+ + H2O ⇌ ............... ]HCl + H2O ⇌ ............... + ...............2. Nitric acidHNO3 + H2O ⇌ ............... + ...............3. Sulphuric acidH2SO4 + H2O ⇌ ............... + ...............b. Classification     4. Monobasic acid [Basicity = 1 ]HCl [aq.] ⇌ ............... + ...............5. Dibasic acid [Basicity = 2]H2SO4 [aq.] ⇌ ............... + ...............6. Tribasic acid [Basicity = 3]H3PO4 [aq.] ⇌ ............... + ...............c. Preparation of acids     7. From non-metalsH2 + Cl2 ⟶ ...............8. From acidic oxidesCO2 + H2O ⟶ ...............   SO3 + H2O ⟶ ...............   P2O5 + H2O ⟶ ...............9. From normal saltsKNO3 + H2SO4 ⟶ ............... + ...............   NaCl+ H2SO4 ⟶ ............... + ...............10. By oxidation of non-metalsS + HNO3 ⟶ ............... + H2O ............... [g]d. Properties of acids     11. Neutralizes basesCuO + H2SO4 ⟶ ............... + ...............   NaOH + HCl ⟶ ............... + ...............Reaction with12. Chlorides and nitratesNaCl+H2SO4[conc.]→<200°C...............+...............	ext{NaCl} + 	ext{H}_2	ext{SO}_4 [	ext{conc.}] \xrightarrow{\lt 200 \degree	ext{C}} ............... + ...............NaCl+H2​SO4​[conc.]<200°C​...............+............... NaNO3+H2SO4[conc.]→<200°C...............+...............	ext{NaNO}_3 + 	ext{H}_2	ext{SO}_4 [	ext{conc.}] \xrightarrow{\lt 200 \degree	ext{C}} ............... + ...............NaNO3​+H2​SO4​[conc.]<200°C​...............+...............13. Carbonates and bicarbonatesNa2CO3 + H2SO4 ⟶ ............... + H2O + ............... [g]   NaHCO3 + H2SO4 ⟶ ............... + H2O + ............... [g]14. Sulphites and bisulphitesNa2SO3 + HCl ⟶ ............... + H2O + ............... [g]   NaHSO3 + HCl ⟶ ............... + H2O + ............... [g]15. Active metalsZn + HCl ⟶ ............... + ............... [g]

Accepted Answer

ACIDS — Ions present in acidsComplete and balance the equationsa. Definition — Dissolves in water yielding hydronium ions1. Hydrochloric acidHCl ⇌ H+ + Cl-[H+ + H2O ⇌ H3O+]HCl + H2O ⇌ H3O+ + Cl-2. Nitric acidHNO3 + H2O ⇌ H3O+ + NO3-3. Sulphuric acidH2SO4 + 2H2O ⇌ 2H3O+ + SO42-b. Classification     4. Monobasic acid [Basicity = 1 ]HCl [aq.] ⇌ H3O+ + Cl-5. Dibasic acid [Basicity = 2]H2SO4 [aq.] ⇌ 2H3O+ + SO42-6. Tribasic acid [Basicity = 3]H2PO4 [aq.] ⇌ 3H3O+ + PO43-c. Preparation of acids     7. From non-metalsH2 + Cl2 ⟶ 2HCl8. From acidic oxidesCO2 + H2O ⟶ H2CO3   SO3 + H2O ⟶H2SO4   P2O5 + 3H2O ⟶2H3PO49. From normal saltsKNO3 + H2SO4 ⟶KHSO4 + HNO3   NaCl+ H2SO4 ⟶NaHSO4 + HCl10. By oxidation of non-metalsS + 6HNO3 ⟶H2SO4 + 2H2O + 6NO2 [g]d. Properties of acids     11. Neutralizes baseCuO + H2SO4 ⟶ CuSO4 + H2O   NaOH + HCl ⟶ NaCl + H2OReaction with12. Chlorides and nitratesNaCl+H2SO4[conc.]→<200°CNaHSO4+HCl	ext{NaCl} + 	ext{H}_2	ext{SO}_4 [	ext{conc.}] \xrightarrow{\lt 200 \degree	ext{C}} \boldsymbol{NaHSO}_\bold{4} + \boldsymbol{HCl}NaCl+H2​SO4​[conc.]<200°C​NaHSO4​+HCl NaNO3+H2SO4[conc.]→<200°CNaHSO4+HNO3	ext{NaNO}_3 + 	ext{H}_2	ext{SO}_4 [	ext{conc.}] \xrightarrow{\lt 200 \degree	ext{C}} \boldsymbol{NaHSO}_\bold{4} + \boldsymbol{HNO}_\bold{3}NaNO3​+H2​SO4​[conc.]<200°C​NaHSO4​+HNO3​13. Carbonates and bicarbonatesNa2CO3 + H2SO4 ⟶ Na2SO4 + H2O + CO2 [g]   2NaHCO3 + H2SO4 ⟶ Na2SO4 + 2H2O + 2CO2 [g]14. Sulphites and bisulphitesNa2SO3 + 2HCl ⟶ 2NaCl + H2O + SO2 [g]   NaHSO3 + HCl ⟶ NaCl + H2O + SO2 [g]15. Active metalsZn + 2HCl ⟶ ZnCl2 + H2 [g]

ACIDS — Ions present in acids	Complete and balance the equations
a. Definition — Dissolves in water yielding hydronium ions
1. Hydrochloric acid	HCl ⇌ ............... + Cl^- [H⁺ + H₂O ⇌ ............... ] HCl + H₂O ⇌ ............... + ...............
2. Nitric acid	HNO₃ + H₂O ⇌ ............... + ...............
3. Sulphuric acid	H₂SO₄ + H₂O ⇌ ............... + ...............
b. Classification
4. Monobasic acid [Basicity = 1 ]	HCl [aq.] ⇌ ............... + ...............
5. Dibasic acid [Basicity = 2]	H₂SO₄ [aq.] ⇌ ............... + ...............
6. Tribasic acid [Basicity = 3]	H₃PO₄ [aq.] ⇌ ............... + ...............
c. Preparation of acids
7. From non-metals	H₂ + Cl₂ ⟶ *...............*
8. From acidic oxides	CO₂ + H₂O ⟶ *...............*
	SO₃ + H₂O ⟶ ...............
	P₂O₅ + H₂O ⟶ ...............
9. From normal salts	KNO₃ + H₂SO₄ ⟶ ............... + ...............
	NaCl+ H₂SO₄ ⟶ ............... + ...............
10. By oxidation of non-metals	S + HNO₃ ⟶ ............... + H₂O ............... [g]
d. Properties of acids
11. Neutralizes bases	CuO + H₂SO₄ ⟶ ............... + ...............
	NaOH + HCl ⟶ ............... + ...............
Reaction with
12. Chlorides and nitrates	$\text{NaCl} + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\lt 200 \degree\text{C}} ............... + ...............$
	$\text{NaNO}_3 + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\lt 200 \degree\text{C}} ............... + ...............$
13. Carbonates and bicarbonates	Na₂CO₃ + H₂SO₄ ⟶ ............... + H₂O + ............... [g]
	NaHCO₃ + H₂SO₄ ⟶ ............... + H₂O + ............... [g]
14. Sulphites and bisulphites	Na₂SO₃ + HCl ⟶ ............... + H₂O + ............... [g]
	NaHSO₃ + HCl ⟶ ............... + H₂O + ............... [g]
15. Active metals	Zn + HCl ⟶ ............... + ............... [g]

ACIDS — Ions present in acids	Complete and balance the equations
a. Definition — Dissolves in water yielding hydronium ions
1. Hydrochloric acid	HCl ⇌ H⁺ + Cl^- [H⁺ + H₂O ⇌ *H₃O⁺] HCl + H₂O ⇌ H₃O⁺* + *Cl^-*
2. Nitric acid	HNO₃ + H₂O ⇌ *H₃O⁺* + *NO₃^-*
3. Sulphuric acid	H₂SO₄ + 2H₂O ⇌ *2H₃O⁺* + *SO₄^2-*
b. Classification
4. Monobasic acid [Basicity = 1 ]	HCl [aq.] ⇌ *H₃O⁺* + *Cl^-*
5. Dibasic acid [Basicity = 2]	H₂SO₄ [aq.] ⇌ *2H₃O⁺* + *SO₄^2-*
6. Tribasic acid [Basicity = 3]	H₂PO₄ [aq.] ⇌ *3H₃O⁺* + *PO₄^3-*
c. Preparation of acids
7. From non-metals	H₂ + Cl₂ ⟶ *2HCl*
8. From acidic oxides	CO₂ + H₂O ⟶ *H₂CO₃*
	SO₃ + H₂O ⟶*H₂SO₄*
	P₂O₅ + 3H₂O ⟶*2H₃PO₄*
9. From normal salts	KNO₃ + H₂SO₄ ⟶*KHSO₄* + *HNO₃*
	NaCl+ H₂SO₄ ⟶*NaHSO₄* + *HCl*
10. By oxidation of non-metals	S + 6HNO₃ ⟶*H₂SO₄* + 2H₂O + *6NO₂* [g]
d. Properties of acids
11. Neutralizes base	CuO + H₂SO₄ ⟶ *CuSO₄* + *H₂O*
	NaOH + HCl ⟶ *NaCl* + *H₂O*
Reaction with
12. Chlorides and nitrates	$\text{NaCl} + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\lt 200 \degree\text{C}} \boldsymbol{NaHSO}_\bold{4} + \boldsymbol{HCl}$
	$\text{NaNO}_3 + \text{H}_2\text{SO}_4 [\text{conc.}] \xrightarrow{\lt 200 \degree\text{C}} \boldsymbol{NaHSO}_\bold{4} + \boldsymbol{HNO}_\bold{3}$
13. Carbonates and bicarbonates	Na₂CO₃ + H₂SO₄ ⟶ *Na₂SO₄* + H₂O + *CO₂ [g]*
	2NaHCO₃ + H₂SO₄ ⟶ *Na₂SO₄* + 2H₂O + *2CO₂ [g]*
14. Sulphites and bisulphites	Na₂SO₃ + 2HCl ⟶ *2NaCl* + H₂O + *SO₂ [g]*
	NaHSO₃ + HCl ⟶ *NaCl* + H₂O + *SO₂ [g]*
15. Active metals	Zn + 2HCl ⟶ *ZnCl₂* + H₂ [g]

Acids, Bases and Salts — Question 1

Question 1