The solubility of CuBr ( s ) at equilibrium to be calculated. Concept introduction: The constant K sp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

Question

Cu2+(aq) + H2O(l) ⇌ CuOH+(aq) + H+(aq) Keq = 1.2 x 10−8 A 1.00 M solution of copper(II) nitrate is created and the system shown above reaches equilibrium. What happens to the pH of the system if more CuOH+ is added after reaching equilibrium? The pH of the system will not change because of the small size of K. The pH of the system will increase because of the increased concentration of CuOH+. The pH of the system will increase as the reverse reaction proceeds at a faster rate to reestablish equilibrium. The pH of the system will decrease as the forward reaction proceeds at a faster rate to reestablish equilibrium.

Answer 1

Question

Chapter 16, Problem 99CP

(a)

Interpretation Introduction

Interpretation: The solubility of CuBr(s) at equilibrium to be calculated.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

(b)

Interpretation Introduction

Interpretation: The concentration of Br− at equilibrium to be calculated.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

(c)

Interpretation Introduction

Interpretation: The concentration of CN− at equilibrium to be calculated.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

Expert Solution & Answer

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

Cu2+(aq) + H2O(l) ⇌ CuOH+(aq) + H+(aq) Keq = 1.2 x 10−8 A 1.00 M solution of copper(II) nitrate is created and the system shown above reaches equilibrium. What happens to the pH of the system if more CuOH+ is added after reaching equilibrium? The pH of the system will not change because of the small size of K. The pH of the system will increase because of the increased concentration of CuOH+. The pH of the system will increase as the reverse reaction proceeds at a faster rate to reestablish equilibrium. The pH of the system will decrease as the forward reaction proceeds at a faster rate to reestablish equilibrium.

理 E The equilibrium concentration of hydroxide ion in a saturated cobalt(II) hydroxide solution is

Given the equation: Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq) ?f=2.00×10^7 determine the concentration of NH3(aq) that is required to dissolve 295 mg of AgCl(s) in 100.0 mL of solution. The ?sp of AgCl is 1.77×10^−10. I've worked this through several times, but I am just not coming up with the right answer! Thanks :)