Question

3.)

a.) For each of the following pairs of formulas, predict whether the substances they represent would react in a precipitation reaction. If there is no reaction, write, "NONE". If there is a reaction, write the complete equation for the reaction. (Use the lowest possible whole number coefficients. Include states-of-matter in your answer.)

(a1) NH₄Cl(aq) + CaSO₃(aq)

(a2) NaCl(aq) + Pb(NO₃)₂(aq)

(a3) NaOH(aq) + Zn(NO₃)₂(aq)

b.) When the following solutions are mixed together, what precipitate (if any) will form? (If no precipitate forms, enter 'NONE'.)

(b1) FeSO₄ (aq) + KCl (aq)

(b2) Al(NO₃)₃ (aq) + Ba(OH)₂ (aq)

(b3) CaCl₂ (aq) + Na₂SO₄ (aq)

(b4) K₂S (aq) + Ni(NO₃)₂ (aq)

c.) Write a balanced equation describing each of the following chemical reactions. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)

(c1) Solid potassium chlorate, KClO₃, decomposes to form solid potassium chloride and diatomic oxygen gas.

(c2) Solid indium metal reacts with solid diatomic iodine to form solid In₂I₆.

(c3) When solid lithium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous lithium sulfate are produced.

(c4) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

d.) Indicate what type, or types, of reaction each of the following represents. (Select all that apply.)

(d1) Pb(NO₃)₂(aq) + H₂SO₄(aq) → PbSO₄(s) + 2 HNO₃(aq)

acid-base, combustion, double displacement, neutralization, oxidation-reduction, precipitation, single-displacement

(d2) KClO₄(s) → KCl(s) + 2 O₂(g)

acid-base, combustion, double displacement, neutralization, oxidation-reduction, precipitation, single-displacement