Write a balanced net ionic equation to show why the solubility of BaF_2(s) incre

Question

Write a balanced net ionic equation to show why the solubility of BaF_2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s) Consider the insoluble compound zinc carbonate, ZnCO_3. The zinc ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of ZnCO_3(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH_3__4^2 +, K_f = 2.9 times 10^9. Use the pull-down boxes to specify states such as (aq) or (s).

Explanation / Answer

a) net ionic equation,

BaF2(s) + 2H+(aq) --> Ba2+(aq) + 2HF(aq)

Knet = 2.4 x 10^-5/(6.6 x 10^-4)^2

        = 55.1

b)

ZnCO3(s) + 4NH3(aq) --> Zn(NH3)4^2+(aq) + CO3^2-(aq)

Knet = 1.5 x 10^-10 x 1.9 x 10^9 = 0.285

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.