Question

Write the balanced equations (all three types) for the reactions that occur when the following aqueous solutions are mixed. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) barium hydroxide (aqueous) and hydrochloric acid molecular equation: complete ionic equation: net ionic equation: (b) ammonia (aqueous) and nitric acid molecular equation: complete ionic equation: net ionic equation: (c) solid silver hydroxide and hydrochloric acid molecular equation: complete ionic equation: net ionic equation: (d) perchloric acid [HClO4(aq)] and iron(III) hydroxide molecular equation: complete ionic equation: net ionic equation:

Answer 1

Answer – We are given the reaction need to two write molecular equation, complete ionic equation and net ionic equation for each one as follow –

a) barium hydroxide (aqueous) and hydrochloric acid

Molecular equation –

Ba(OH)₂(aq) + 2 HCl(aq) -----> BaCl₂(aq) + 2 H₂O(l)

Complete ionic equation-

Ba²⁺(aq) + 2OH^-(aq) + 2H⁺(aq) + 2Cl^-(aq) -----> Ba²⁺(aq) + 2Cl^-(aq) + 2 H₂O(l)

Net ionic equation-

2OH^-(aq) + 2H⁺(aq) -----> 2 H₂O(l)

b) ammonia (aqueous) and nitric acid

Molecular equation –

NH₃(aq) + HNO₃(aq) ------> NH₄⁺(aq) + NO₃^-(aq)

Complete ionic equation-

NH₃(aq) + H⁺(aq) + NO₃^-(aq) -----> NH₄⁺(aq) + NO₃^-(aq)

Net ionic equation-

NH₃(aq) + H⁺(aq) -----> NH₄⁺(aq)

c) solid silver hydroxide and hydrochloric acid

Molecular equation –

AgOH(s) + HCl(aq) -----> AgCl(s) + H₂O(l)

Complete ionic equation-

AgOH(s) + H⁺(aq) + Cl(aq) -----> AgCl(s) + H₂O(l)

Net ionic equation –

AgOH(s) + H⁺(aq) + Cl(aq) -----> AgCl(s) + H₂O(l)

d) perchloric acid [HClO4(aq)] and iron(III) hydroxide

3 HClO₄(aq) + Fe(OH)₃(s) -----> Fe(ClO₄)₃(aq) + 3H₂O)(l)

Complete ionic equation-

3H⁺(aq) + 3 ClO₄^-(aq) + Fe(OH)₃(s) -----> Fe³⁺(aq) + 3 ClO₄^-(aq) + 3H₂O)(l)

Net ionic reaction –

3H⁺(aq) + + Fe(OH)₃(s) -----> Fe³⁺(aq) + 3H₂O)(l)