Back
Problem 6
Which of the following ions will always be a spectator ion in a precipitation reaction? (a) Cl- (b) NO3- (c) NH4+ (d) S2- (e) SO42-
Problem 8
Which of these statements is true?
a. If a compound is oxidized, it is gaining electrons.
b. If a base is neutralized, it is gaining protons.
c. Elements that are metals cannot be oxidized.
d. If hydrogen gas is generated in a reaction, it must be an acid–base reaction.
Problem 9
What kind of reaction is this? N2(g)+3H2(g)⟶2NH3(g)
a. an acid–base reaction
b. a metathesis reaction
c. a redox reaction
d. a precipitation reaction
Problem 10a
An aqueous solution contains 1.2 mM of total ions. (a) If the solution is NaCl(aq), what is the concentration of chloride ion?
Problem 10b
An aqueous solution contains 1.2 mM of total ions. (b) If the solution is FeCl3(aq), what is the concentration of chloride ion?
Problem 12
In a titration experiment, 50.0 mL of 0.075 M acetic acid, CH3COOH, is titrated with the 0.250 M KOH(aq) that is in the burette. The drawing shows the level of the KOH in the burette before the titration begins. What will be the burette reading at the equivalence point?
Problem 13a
State whether each of the following statements is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution.
Problem 13b
State whether each of the following statements is true or false. Justify your answer in each case. (b) If you add a nonelectrolyte to an aqueous solution that already contains an electrolyte, the electrical conductivity will not change.
- State whether each of the following statements is true or false. Justify your answer in each case. (b) When ammonium nitrate, NH4NO3, dissolves in water, the solution is weakly conducting and basic in nature.
Problem 14
Problem 15
We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.
Problem 16
Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?
Problem 17a
Specify what ions are present in solution upon dissolving each of the following substances in water: a. FeCl2
Problem 17c
Specify what ions are present in solution upon dissolving each of the following substances in water: c. (NH4)2SO4
Problem 18a
Specify what ions are present upon dissolving each of the following substances in water: (a) MgI2
Problem 18b
Specify what ions are present upon dissolving each of the following substances in water: (b) K2CO3
Problem 18c
Specify what ions are present upon dissolving each of the following substances in water: (c) HClO4
Problem 18d
Specify what ions are present upon dissolving each of the following substances in water: (d) NaCH3COO
Problem 19a
Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound?
Problem 19b
Formic acid, HCOOH, is a weak electrolyte. Write the chemical equation for the ionization of HCOOH.
Problem 20a1
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of CH3COCH3?
Problem 20a2
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of HClO?
Problem 20a3
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of NH4Cl?
Problem 20b
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (b) If 0.1 mol of each compound is dissolved in solution, which one contains 0.2 mol of solute particles, which contains 0.1 mol of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?
Problem 21
Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) MgBr2 (b) NH4OH (c) Ni(CH3COO)2 (d) AgNO3 (e) FeCO3.
Problem 22d
Predict whether each of the following compounds is soluble in water: d. Al(OH)3
Problem 23c
Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. c. FeSO4 and Pb(NO3)2
Problem 24b
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. b. KOH and Cu(NO3)2
Problem 25a
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate
Problem 25c
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (c) ammonium phosphate and calcium chloride
Problem 26a
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. a. Cr2(SO4)3(𝑎𝑞)+(NH4)2CO3(𝑎𝑞)⟶