Ch10 - Dembinski Winter 2016 PDF

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CHEM 6A – Chapter 10 Extra Practice Problems

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PRECIPITATION REACTIONS Show the ionic and net ionic equations for the following molecular equations. Also, identify the spectator ions and the precipitates 1. AgNO3 (aq) + KCl (aq)

2. Mg(NO3)2 (aq)

à฀

+ Na2CO3 (aq)

AgCl (s) + KNO3 (aq)

à฀ MgCO3 (s) +

3. strontium bromide (aq) + potassium sulfate (aq) à฀ potassium bromide (aq)

NaNO3 (aq)

strontium sulfate (s) +

4. manganese(II) chloride (aq) + ammonium carbonate (aq) à฀ manganese(II) carbonate (s) + ammonium chloride (aq)

5. chromium(III) nitrate (aq) (aq) + iron(II) nitrate (aq)

+ iron(II) sulfate (aq) à฀ chromium(III) sulfate

Please complete the following reactions, and show the total ionic and net ionic forms of the equation based on the solubility rules presented in class: 6. K3PO4 (aq) + Al(NO3)3 (aq) à฀

7. BeI2 (aq) + Cu2SO4 (aq) à฀

8. cobalt(III) bromide + potassium sulfide à฀

9. barium nitrate +

ammonium phosphate à฀

CHEM 6A – Chapter 10 Extra Practice Problems

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10. calcium hydroxide + iron(III) chloride à฀

11. For each of the following problems, a) determine whether a precipitate forms when solutions of reactants are mixed, b) write a net ionic equation for the formation of the precipitate 1.

KCl and Na3PO4

2.

Ca(NO3)2 and MgSO4

3.

FeCl3 and LiOH

4.

CuSO4 and (NH4)3PO4

5.

Sodium nitrate and calcium chloride

6.

Sodium sulfate and barium nitrate

7.

Zinc nitrate and potassium sulfate

8.

Lead(II) nitrate and sodium carbonate

9.

Potassium phosphate and cobalt(II) chloride

10.

Copper(I) nitrate and magnesium chloride

OXIDATION STATES 1. Determine the oxidation number of the elements in each of the following compounds: a. H2CO3

b. N2

CHEM 6A – Chapter 10 Extra Practice Problems

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c. Zn(OH)42d. NO2e. LiH

f. Fe3O4 2. Find the oxidation states of the metals in the following compounds: 1. FeBr3 2. CrO3

3. NaH

4. KMnO4

IDENTIFYING OXIDIZING OR REDUCING AGENTS Determine what molecule/atom is being oxidized and which is being reduced in each of the following reactions. Also, determine which substance is the oxidizing agent and which substance is the reducing agent. 1. K + H2O à฀ KOH + H2

2. FeO + O2 à฀ Fe2O3

3. Ca + F2 à฀ CaF2

4. 2 Cr+ + Sn4+

Cr3+ + Sn2+

CHEM 6A – Chapter 10 Extra Practice Problems

5. 3 Hg2+ + 2 Fe (s)

6. 2 As (s) + 3 Cl2 (g)

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3 Hg2 + 2 Fe3+

2 AsCl3

BALANCING REDOX EQUATIONS 1. Under acidic conditions the bromate ion is reduced to the bromide ion. Write the balanced half-reaction for this process. a) BrO3-1 + 6H+ + 6e-1 → Br-1 + 3H2O b) 2BrO3-1 + 6H+ → Br2 +6H2O + 3e-1 c) BrO3 -1 + 6H2O + 10e-1 → Br2 + 12H+ + 3O2 d) 2BrO3-1 + 6H2O → 2Br-1 + 12H+ + 6O2 + 8e-1 e) 2BrO3 -1 + 6H+ → Br2 + 3H2O + 3e-1

2. Balance the following redox equation which occurs in acidic solution. N2H4 (g) + BrO3-1 (aq) → Br-1 (aq) + N2(g) a) 3N2H4 + BrO3 -1 → 3N2 + Br- + 3H2O + 6H+ b) N2H4 + BrO3 -1 + 2H+ → 2Br-1 + N2 +3H2O c) 3N2H4 + 2BrO3-1 + 12H+ → 3N2 + 2Br-1 + 6H2O + 12H+ d) N2H4 + 2BrO3-1 + 8H+ → 2Br-1 + N2 + 6H2O e) 3N2H4 + 2BrO3-1 → 3N2 + 2Br-1 + 6H2O

3. Balance the following redox reactions: a) MnO4-1 (aq) + Br-1 (aq) → MnO2 (s) + BrO3-1 (aq) [in acidic solution]

b) I2 (s) + OCl-1 (aq) → IO3-1 (aq) + Cl-1 (aq) [in acidic solution]

CHEM 6A – Chapter 10 Extra Practice Problems

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c) Cr2O72- (aq) + C2O42- (aq) → Cr3+ (aq) + CO2 (g) [in acidic solution]

d) Mn (s) + HNO3 (aq) → Mn2+ (aq) + NO2 (g) [in acidic solution]

e) MnO4-1 (aq) + Fe2+ (aq) → Mn2+ (aq) + Fe3+ (aq) [in acidic solution]

f) Cr2O72- (aq) + H2S (g) → Cr3+ (aq) + S (s) [in basic solution]

g) MnO4-1 (aq) + H2S (g) → Mn2+ (aq) + S (s) [in basic solution]

h) Cu (s) + SO4 2- (aq) → Cu2+ (aq) + SO2 (g) [in basic solution]

i) Cr2O72- (aq) + NO2-1 (aq) → Cr3+ (aq) + NO3-1 (aq) [in basic solution]

j) I-1 (aq) + Br2 (l) → IO3-1 (aq) + Br-1 (aq) [in basic solution]...