Write a balanced net ionic equation to show why the solubility of Co(OH)2 increa

Question

Write a balanced net ionic equation to show why the solubility of Co(OH)2 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 References to access important values if needed for this question. Write a balanced net ionic equation to show why the solubility of Co(OH)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) Submit Answer Retry Entire Group 1 more group attempt remaining

Explanation / Answer

Co(OH)2 ===== Co (aq) + 2 OH-

When you add an acid the H3O+ will react with OH ions in order to create water

Co(OH)2 ===== Co (aq) + 2 OH-

2 H3O+ + 2 OH- ======== H2O

------------------------------------------------------------

Co(OH)2 ===== Co (aq) + 2 OH-   Ksp = 3 x 10-16 ; from internet

2 H3O+ + 2 OH- ======== 2 H2O K1/w is the inverse of Kw so = (1 / 1 x 10-14 )2 ; 1 x 1028

_______________________________________

Co(OH)2 (s) + 2 H3O + (aq) ===== Co (aq) + 2 H2O (l)

K eq = Co / (H3O+)2; remember that liquids and solids are not considered in the equilibrium equation

For the combination of equations since we know the equilibriums from both, the equilibrium constant would be

Keq = K1/w * Ksp

K eq = 1 x 1028 *  3 x 10-16 = 3 x 10 12

*Rate this answer if you like it

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

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