0.24 Bis2a 06.appendix a review of red/ox reactions  (Page 6/31)

Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(a) H ₂ SO ₄

(b) Ca(OH) ₂

(c) BrOH

(d) ClNO ₂

(e) TiCl ₄

(f) NaH

Classify the following as acid-base reactions or oxidation-reduction reactions:

(a) ${\text{Na}}_2\text{S(}aq\text{)}+2\text{HCl(}aq\text{)}⟶2\text{NaCl(}aq\text{)}+{\text{H}}_2\text{S(}g\text{)}$

(b) $2\text{Na(}s\text{)}+2\text{HCl(}aq\text{)}⟶2\text{NaCl(}aq\text{)}+{\text{H}}_2\text{(}g\text{)}$

(c) $\text{Mg(}s\text{)}+{\text{Cl}}_2\text{(}g\text{)}⟶{\text{MgCl}}_2\text{(}s\text{)}$

(d) $\text{MgO(}s\text{)}+2\text{HCl(}aq\text{)}⟶{\text{MgCl}}_2\text{(}aq\text{)}+{\text{H}}_2\text{O(}l\text{)}$

(e) ${\text{K}}_3\text{P(}s\text{)}+2{\text{O}}_2\text{(}g\text{)}⟶{\text{K}}_3{\text{PO}}_4\text{(}s\text{)}$

(f) $3\text{KOH(}aq\text{)}+{\text{H}}_3{\text{PO}}_4\text{(}aq\text{)}⟶{\text{K}}_3{\text{PO}}_4\text{(}aq\text{)}+3{\text{H}}_2\text{O(}l\text{)}$

Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations:

(a) $\text{Mg(}s\text{)}+{\text{NiCl}}_2\text{(}aq\text{)}⟶{\text{MgCl}}_2\text{(}aq\text{)}+\text{Ni(}s\text{)}$

(b) ${\text{PCl}}_3\text{(}l\text{)}+{\text{Cl}}_2\text{(}g\text{)}⟶{\text{PCl}}_5\text{(}s\text{)}$

(c) ${\text{C}}_2{\text{H}}_4\text{(}g\text{)}+3{\text{O}}_2\text{(}g\text{)}⟶2{\text{CO}}_2\text{(}g\text{)}+2{\text{H}}_2\text{O(}g\text{)}$

(d) $\text{Zn(}s\text{)}+{\text{H}}_2{\text{SO}}_4\text{(}aq\text{)}⟶{\text{ZnSO}}_4\text{(}aq\text{)}+{\text{H}}_2\text{(}g\text{)}$

(e) $2{\text{K}}_2{\text{S}}_2{\text{O}}_3\text{(}s\text{)}+{\text{I}}_2\text{(}s\text{)}⟶{\text{K}}_2{\text{S}}_4{\text{O}}_6\text{(}s\text{)}+2\text{KI(}s\text{)}$

(f) $3\text{Cu(}s\text{)}+8{\text{HNO}}_3\text{(}aq\text{)}⟶3\text{Cu}{\text{(}{\text{NO}}_3\text{)}}_2\text{(}aq\text{)}+2\text{NO(}g\text{)}+4{\text{H}}_2\text{O(}l\text{)}$

Complete and balance the following acid-base equations:

(a) HCl gas reacts with solid Ca(OH) ₂ ( s ).

(b) A solution of Sr(OH) ₂ is added to a solution of HNO ₃ .

Complete and balance the following acid-base equations:

(a) A solution of HClO ₄ is added to a solution of LiOH.

(b) Aqueous H ₂ SO ₄ reacts with NaOH.

(c) Ba(OH) ₂ reacts with HF gas.

Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.

(a) $\text{Al(}s\text{)}+{\text{F}}_2\text{(}g\text{)}⟶$

(b) $\text{Al(}s\text{)}+{\text{CuBr}}_2\text{(}aq\text{)}⟶$ (single displacement)

(c) ${\text{P}}_4\text{(}s\text{)}+{\text{O}}_2\text{(}g\text{)}⟶$

(d) $\text{Ca(}s\text{)}+{\text{H}}_2\text{O(}l\text{)}⟶$ (products are a strong base and a diatomic gas)

Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.

(a) $\text{K(}s\text{)}+{\text{H}}_2\text{O(}l\text{)}⟶$

(b) $\text{Ba(}s\text{)}+\text{HBr(}aq\text{)}⟶$

(c) $\text{Sn(}s\text{)}+{\text{I}}_2\text{(}s\text{)}⟶$

Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used.

(a) $\text{Mg}{\text{(OH)}}_2\text{(}s\text{)}+{\text{HClO}}_4\text{(}aq\text{)}⟶$

(b) ${\text{SO}}_3\text{(}g\text{)}+{\text{H}}_2\text{O(}l\text{)}⟶\text{(assume an excess of water and that the product dissolves)}$

(c) $\text{SrO(}s\text{)}+{\text{H}}_2{\text{SO}}_4\text{(}l\text{)}⟶$