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Problem 40a
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide
Problem 40b
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (b) Solid chromium(III) hydroxide reacts with nitrous acid.
Problem 40c
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (c) Aqueous nitric acid and aqueous ammonia react.
Problem 41a,b
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.
Problem 42a,b
Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO(s) + 2 HClO4(aq) → Fe(ClO4)2(aq) + H2O(l) (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueous solution of nitric acid.
- Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?
Problem 43
- As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. (a) Write the molecular and net ionic equations for this reaction. (b) Based on the definitions of acid and base, what ion is the base in this reaction? (c) What is the acid in the reaction? (d) What is the spectator ion in the reaction?
Problem 44
- True or false: (a) If a substance is oxidized, there must be more oxygen in the substance.
Problem 45
- True or false: (a) Reduction occurs if the oxidation number of an element increases
Problem 46
Problem 47b
(a) Which region of the periodic table shown here contains elements that are easiest to oxidize? (b) Which region contains the least readily oxidized elements?
Problem 48a,b,c
Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, BaSO4 (b) sulfurous acid, H2SO3 (c) strontium sulfide, SrS
Problem 48d
Determine the oxidation number of sulfur in each of the following substances: (d) hydrogen sulfide, H2S
Problem 48e
Determine the oxidation number of sulfur in each of the following substances: (e) Locate sulfur in the periodic table in Exercise 4.47; what region is it in?
Problem 48f
Determine the oxidation number of sulfur in each of the following substances: (f) Which region(s) of the periodic table contains elements that can adopt both positive and negative oxidation numbers?
Problem 49a,b
Determine the oxidation number for the indicated element in each of the following substances: (a) S in SO3 (b) Ti in TiCl4
Problem 49c
Determine the oxidation number for the indicated element in each of the following substances: (c) P in AgPF6
Problem 49d
Determine the oxidation number for the indicated element in each of the following substances: (d) N in HNO3
Problem 50e,f
Determine the oxidation number for the indicated element in each of the following substances: (e) Pt in PtCl4 (f) O in OF2.
Problem 50f
Determine the oxidation number for the indicated element in each of the following substances: (f) Cl in NaClO4.
Problem 51a
Which element is oxidized, and which is reduced in the following reactions? (a) N2(g) + 3 H2(g) → 2 NH3(g)
Problem 51b
Which element is oxidized, and which is reduced in the following reactions? (b) 3 Fe(NO3)2(aq) + 2 Al(s) → 3 Fe(s) + 2 Al(NO3)3(aq)
Problem 51c,d
Which element is oxidized, and which is reduced in the following reactions? (c) Cl2(aq) + 2 NaI(aq) → I2(aq) + 2 NaCl(aq) (d) PbS(s) + 4 H2O2(aq) → PbSO4(s) + 4 H2O(l)
Problem 52
Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P4(s) + 10 HClO(aq) + 6 H2O(l) → 4 H3PO4(aq) + 10 HCl(aq) (b) Br2(l) + 2 K(s)→ 2 KBr(s) (c) CH3CH2OH(l) + 3 O2(g) → 3 H2O(l) + 2 CO2(g) (d) ZnCl2(aq) + 2 NaOH(aq) → Zn(OH)2(s) + 2 NaCl(aq)
Problem 53
Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid (b) chromium with hydrobromic acid (c) tin with hydrochloric acid (d) aluminum with formic acid, HCOOH.
Problem 54a,b
Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel (b) dilute sulfuric acid with iron
Problem 54c,d
Write balanced molecular and net ionic equations for the reactions of (c) hydrobromic acid with magnesium (d) acetic acid, CH3COOH, with zinc.
Problem 55a,b
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate (b) zinc metal is added to a solution of magnesium sulfate
Problem 55c
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal
Problem 55d
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride
Problem 55e
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) aluminum metal is added to a solution of cobalt(II) sulfate.