Question

what’s the answer?

Question 3 A Solution pH 7.00 8.00 9.00 Ag... 1.41 x 10-4 1.41 x 10-4 1.37 x 10-4 1.00 x 10-4 1.96 x 100 2.00 x 10- 2.00 x 10-7 Submit 10.00 11.00 12.00 13.00 A student investigates the effects of pH on the solubility of AgOH(3), which dissolves in water according to the equation AgOH(3) Ag' (aq) + OH(aq). The value for Kp for AgOH is 2.0 x 10 at 298 K. The student places the same mass of AgOH(s) into 50.0 mL of different solutions with specific pH values and measures the concentration of Agions in each solution after equilibrium is reached. Based on the data in the table, what can be concluded about the solubility of AgOH? ( A ) The solubility of AgOH is unaffected by pH because Ksp is a constant value at 298 K The solubility of AgOH is unaffected by pH because it is the same value for pH 7.00 and pH 8.00 ) AGOH is more soluble at higher pH because lower concentrations of OH(aq) shift the solubility equilibrium toward Ag (aq) and OH (04). AgOH is less soluble at higher pH because higher concentrations of OH(aq) shift the solubility equilibrium toward solid AGOH.

Answer 1

The reaction for dissolution of AgOH is as follows :

AgOH (s) ⇌ Ag+ (aq)+ OH-(aq)

As pH increases, the concentration of   OH- already in the medium increases. This drives the above dissolution in the backward direction , i.e, AgOH will now dissociate less.This decreases the amount of Ag+  formed in the solution (as observed in the experiment). Thus, AgOH becomes less soluble as pH increases. So, option D is correct.