Equilibrium Ksp

Which one of the following is the solubility product constant for Mn(OH)₂?

• K_sp = [Mn²⁺][OH^-]²

• K_sp = [Mn²⁺][2 OH^-]²

• K_sp = [Mn²⁺]²[OH^-]²

• K_sp = [Mn²⁺]²[OH^-]

Tags

NGSS.HS-PS1-7

The solubility of HgS is 5.5 x 10^-27 mol/L. What is K_sp for HgS?

• 4.0 x 10^-3

• 8.2 x 10^-4

• 1.3 x 10^-13

• 3.0 x 10^-53

Which expression best describes the relationship between solubility product, K_sp, and the solubility, s, of MgF₂?

• K_sp = s²

• K_sp = 2s³

• K_sp = 4s²

• K_sp = 4s³

Calculate the molar solubility of Fe₂S₃.

K_sp = 1.4 x 10^-88

• 1.2 x 10^-44 M

• 1.1 x 10^-18 M

• 4.8 x 10^-24 M

• 5.5 x 10^-62 M

Calculate the equilibrium constant for the reaction:
CuCl (s) + I- (aq)  $\leftrightarrow$   CuI (s) + Cl- (aq)
CuCl;  Ksp = 1.9 x 10-7
CuI;  Ksp = 5.1 x 10-12

• 8.4 x 10^-2

• 2.3 x 10^-6

• 3.7 x 10⁴

• 4.4 x 10¹⁷

For BaSO₄, K_sp = 1.1 x 10^-10. If you mix 200. mL of 1.0 x 10^-4 M Ba(NO₃)₂ and 500. mL of 8.0 x 10^-2 M H₂SO₄, what will be observed?

• A precipitate forms because Q_sp > K_sp

• A precipitate forms because Q_sp < K_sp

• No precipitate forms because Q_sp < K_sp

• No precipitate forms because Q_sp > K_sp

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-5

A saturated solution of Ca(OH)₂, has a pH of 12.40. What is the K_sp for Ca(OH)₂?

• 2.5 x 10^-2

• 1.3 x 10^-2

• 8.0 x 10^-6

• 2.0 x 10^-6

Tags

NGSS.HS-PS1-7