Workshop CHE 166
Problem Set #5
 

1. Identify the ions present in an aqueous solution of

a)  LiOH
b)  NH₄NO₃
c)  Na₂CrO₄
d)  KCl
e)  Al₂(SO₄)₃

2. The distinguishing characteristic of all electrolyte solutions is that they:

3. Characterize the following compounds as soluble or insoluble in water

a)  Ca₃(PO₄)₂
b)  Mn(OH)₂
c)  AgClO₄
d)  K₂S
e)  CaCO₃
f)  ZnSO₄
g)  Hg(NO₃)₂
h)  HgSO₄
i)  NH₄ClO₃
j)  BaSO₃

4. Identify each of the following substances as a strong electrolyte, a weak electrolyte or a nonelectrolyte:

a)  H₂O
b)  KCl
c)  HNO₃
d)  HC₂H₃O₂
e)  C₁₂H₂₂O₁₁
f)  Ba(NO₃)₂
g)  Ne
h)  NH₃
i)  NaOH

5. Identify the following compounds as a weak or strong acid or base:

a)  NH₃
b)  H₃PO₄
c)  LiOH
d)  HCHO₂ (formic acid)
e)  H₂SO₄
f)  HF
g)  Ba(OH)₂

6. What is the chemical formula of the salt produced by neutralization of nitric acid with Ca(OH)₂?

7. What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid and calcium hydroxide?

8. In accordance with the solubility rules, what will happen when solutions of ZnSO_{4 (aq)} and MgCl_{2 (aq)} are mixed?

9. In accordance with the solubility rules, what will happen when solutions of Pb(NO₃)_{2 (aq)} and KI _(aq) are mixed?

10. What is the coefficient of H₂SO₄ when the following equation is properly balanced with the smallest set of whole numbers?

___ Ca₃(PO₄)_{2 (s)} + ___ H₂SO_{4 (aq)} ® ___ CaSO_{4 (aq)} + ___ H₃PO_{4 (aq)}

11. Write balanced molecular, total ionic and net ionic equations for the listed reactions. Show the state of each reactant and each product in each equation.

a) AgNO_{3 (aq)} + Na₂CO_{3 (aq)} ®

b) BaCl_{2 (aq)} + Na₂CO_{3 (aq)} ®

c) (NH₄)₂SO_{4 (aq)} + NaCl _(aq) ®

d) ZnS _(s) + HCl _(aq) ®

e) K₃PO_{4 (aq)} + Al(NO₃)_{3 (aq)} ®

f) NH₄C₂H₃O_{2 (aq)} + Pb(NO₃)₂ ®

12. The oxidation number of Cl in HClO₄ is:

13. The oxidation number of N in N₂H₄ is:
14. The oxidation number of Cr in Cr₂O₇^{2 -} is:

15. The highest possible oxidation number of carbon is:

16. Complete and balance the following half-reaction using whole numbers as coefficients:

Cr₂O₇^{2 -} _(aq) ® Cr³⁺_(aq) [acidic solution]

17. Complete and balance the following redox equation using whole numbers as coefficients. Identify the oxidizing agent, the reducing agent, the substance oxidized and the substance reduced.

MnO₄^- _(aq) + H⁺ _(aq) + Br^- _(aq) ® Mn²⁺ _(aq) + Br_{2 (aq)} + H₂O _(l) [acidic solution]

18. Complete and balance the following redox equation using whole numbers as coefficients. Identify the oxidizing agent, the reducing agent, the substance oxidized and the substance reduced.

As _(s) + ClO₃^- _(aq) ® HClO _(aq) + H₃AsO_{3 (aq)} [acidic solution]

19. Complete and balance the following redox equation using whole numbers as coefficients. Identify the oxidizing agent, the reducing agent, the substance oxidized and the substance reduced.

Ag⁺ _(aq) + H₂O_{2 (aq)} ® Ag _(s) [acidic solution]

20. Complete and balance the following half-reaction using whole numbers as coefficients:

ClO^- _(aq) ® Cl^- _(aq) [basic solution]

21. Complete and balance the following redox equation using whole numbers as coefficients. Identify the oxidizing agent, the reducing agent, the substance oxidized and the substance reduced.

Bi(OH)_{3 (s)} + SnO₂^2- _(aq) ® Bi _(s) + SnO₃^2- _(aq) [basic solution]

22. Complete and balance the following redox equation using whole numbers as coefficients. Identify the oxidizing agent, the reducing agent, the substance oxidized and the substance reduced.

MnO₄^- _(aq) + I ^- _(aq) ® MnO_{2 (s)} + IO₃^- _(aq) [basic solution]

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