Chemistry
| 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 | NaCl + H2SO4[conc.] ⟶ …………… + …………… |
| NaNO3 + H2SO4[conc.] ⟶ …………… + …………… | |
| 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] |
Answer
| 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+ + 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-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 | NaCl + H2SO4[conc.] ⟶ NaHSO4 + HCl |
| NaNO3 + H2SO4[conc.] ⟶ NaHSO4 + HNO3 | |
| 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] |
Related Questions
BASES — Ions present in bases a. Alkali — dissociates yielding hydroxyl ions 16. Sodium hydroxide NaOH [aq.] ⇌ …………… + …………… 17. Ammonium hydroxide NH4OH [aq.] ⇌ …………… + …………… b. Classification 18. Monoacidic base [Acidity = 1 ] KOH [aq.] ⇌ …………… + …………… 19. Diacidic base [Acidity = 2] Cu(OH)2 [aq.] ⇌ …………… + …………… c. Preparation of bases 20. From metals Na + O2 ⟶ …………… 21. From metallic oxides and metals K2O + H2O ⟶ …………… K + H2O ⟶ …………… + …………… 22.From salts AlCl3 + NaOH ⟶ …………… + …………… ↓ FeSO4 + NaOH ⟶ …………… + …………… ↓ 23. By thermal decomposition ZnCO3 ⟶ …………… + …………… [g] Pb(NO3)2 ⟶ …………… + ……………[g] + ………….. [g] c. Properties of bases 24. Neutralizes acids PbO + HNO3 ⟶ …………… + …………… Fe(OH)2 + HCl ⟶ …………… + …………… Reaction with 25. Metallic salt solution CuCl2 + NaOH ⟶ …………… + …………… ↓ FeCl3 + NaOH ⟶ …………… + …………… ↓ 26. Ammonium salts NH4Cl + NaOH ⟶ …………… + …………… + …………… [g] NH4Cl + Ca(OH)2 ⟶ …………… + …………… + …………… [g] SALTS — Ions present in salts 27a. Normal salt [formation] NaOH [excess] + H2SO4 ⟶ …………… + H2O 27b. Acid salt [formation] NaOH [insufficient] + H2SO4 ⟶ …………… + H2O Preparation of salts — General methods Direct combination — Synthesis 28. Iron and Chloride — salt iron [III] Chloride Fe + Cl2 ⟶ …………… 29. Zinc and sulphur — salt zinc sulphide Zn + S ⟶ …………… Displacement — Action of dilute acid on active metals 30. Iron — salt iron [II] sulphate Fe + H2SO4 ⟶ …………… + …………… [g] 31. Zinc — salt zinc sulphate Zn + H2SO4 ⟶ …………… + …………… [g] 32. Magnesium — salt magnesium chloride Mg + HCl ⟶ …………… + …………… [g] Precipitation — by double decomposition of two salt solutions 33. Lead nitrate and sodium chloride Pb(NO3)2 + NaCl ⟶ …………… + …………… ↓ 34. Calcium chloride and sodium carbonate CaCl2 + Na2CO3 ⟶ …………… + …………… ↓ Neutralization — Action of dilute acid on insoluble base 35. Oxide — salt copper sulphate CuO + H2SO4 ⟶ …………… + …………… 36. Hydroxide — salt copper sulphate Cu(OH)2 + H2SO4 ⟶ …………… + …………… Neutralization — [Titration] Action of dilute acid on an alkali 37. Hydroxide — salt sodium chloride NaOH + HCl ⟶ …………… + …………… 38. Hydroxide — salt ammonium chloride NH4OH + HCl ⟶ …………… + …………… Action of dilute acid on carbonate & bicarbonate 39. Carbonate — salt lead nitrate PbCO3 + HNO3 ⟶ …………… + …………… + …………… [g] 40. Carbonate — salt copper chloride CuCO3 + HCl ⟶ …………… + …………… + …………… [g] 41. Bicarbonate — salt potassium sulphate KHCO3 + H2SO4 ⟶ …………… + …………… + …………… [g] Mention the colour changes observed when the following indicators are added to acids:
(i) Alkaline phenolphthalein solution.
(ii) Methyl orange solution
(iii) Neutral litmus solution
Which of the following hydroxides is not an alkali — [Choose from the choices A, B, C and D]
(A) ammonium hydroxide
(B) calcium hydroxide
(C) copper hydroxide
(D) sodium hydroxide