Review the following concept if needed - Aqueous Reactions Study Guide
Practice Questions
Identify the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte.
1. sulfuric acid
2. glucose
3. cyanic acid
4. sodium cyanide
5. ammonia
Identify the following as being soluble or insoluble in water. If the substance is soluble, indicate the ions that would be formed upon dissolving in water.
6. chromium nitrate
7. lead (II) iodide
8. barium hydroxide
9. barium sulfate
10. potassium phosphate
Write the balanced molecular and net ionic equations when the following solutions are mixed together. If no precipitate forms, write "no reaction."
11. NH4Cl(aq) + AgNO3(aq) →
12. NaOH(aq) + MgCl2(aq) →
13. lead acetate(aq) + sodium sulfate(aq) →
14. potassium chloride(aq) + lithium carbonate (aq) →
15. K2S(aq) + Ni(NO3)2(aq) →
Identify the following substances as an acid or a base.
16. HCN
17. HNO3
18. strontium hydroxide
19. HClO4
20. LiOH
Write the net ionic equation for the following reactions.
21. cyanic acid(aq) + potassium hydroxide(aq) →
22. Al(OH)3(s) + HCl(aq) →
23. CH3CO2H(aq) + KOH(aq) →
24. sodium hydroxide(aq) + sulfuric acid(aq) →
25. HNO2(aq) + Mg(OH)2(s) →
Assign the oxidation state for each element in the following molecules.
26. I2
27. KNO3
28. H2CrO4
29. H2O2
30. PF3
Identify the species being oxidized, the species being reduced, the oxidizing agent, and the reducing agent in the following reactions.
31. Mg(s) + H2O(g) → Mg(OH)2(s) + H2(g)
32. 8H+(aq) + 6Cl–(aq) + Sn(s) + 4NO3–(aq) → SnCl62–(aq) + 4NO2(g) + 4H2O(l)
33. MnO4–(aq) + Fe2+(aq) → Fe3+(aq) + Mn2+(aq)
34. Na(s) + Cl2(g) → NaCl(s)
35. H2 + O2 → H2O
Answers
1. Strong electrolyte
2. Nonelectrolyte
3. Weak electrolyte
4. Strong electrolyte
5. Weak electrolyte
6. Soluble; Cr2+, NO3 –
7. Insoluble
8. Soluble; Ba2+, OH–
9. Insoluble
10. Soluble; K+, PO43–
11. NH4Cl(aq) + AgNO3(aq) → NH4NO3(aq) + AgCl(s); Cl–(aq) + Ag+(aq)→AgCl(s)
12. 2NaOH(aq) + MgCl2(aq) → 2NaCl(aq) + Mg(OH)2(s); 2OH –(aq) + Mg2+(aq) → Mg(OH)2(s)
13. Pb(C2H3O2)2(aq) + Na2SO4(aq) → PbSO4(s) + 2NaC2H3O2(aq); Pb2+ (aq) + SO42– (aq) → PbSO4(s)
14. KCl(aq) + Li2CO3(aq) → no reaction
15. K2S(aq) + Ni(NO3)2(aq) → 2KNO3(aq) + NiS(s); S2–(aq) + Ni2+(aq) → NiS(s)
16. Acid
17. Acid
18. Base
19. Acid
20. Base
21. HCN(aq) + OH–(aq) → CN–(aq) + H2O(l)
22. Al(OH)3(s) + 3H + (aq) → Al3+ (aq) + 3H2O(l)
23. CH3CO2H(aq) + OH–(aq) → CH3CO2–(aq) + H2O(l)
24. OH– (aq) + H + (aq) → H2O(l)
25. 2HNO2(aq) + Mg(OH)2(s) → Mg(NO2)2(s) + 2H2O(l)
26. 0
27. K = +1, N = +5, O = –2
28. H = +1, Cr = +6, O = –2
29. H = +1, O = –1
30. P = +3, F = –1
31. Species being oxidized = Mg, species being reduced = H, oxidizing agent = H2O, reducing agent = Mg
32. Species being oxidized = Sn, species being reduced = N, oxidizing agent = NO3–, reducing agent = Sn
33. Species being oxidized = Fe, species being reduced = Mn, oxidizing agent = MnO4–, reducing agent = Fe2+
34. Species being oxidized = Na, species being reduced = Cl, oxidizing agent = Cl2, reducing agent = Na
35. Species being oxidized = H, species being reduced = O, oxidizing agent = O2, reducing agent = H2
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