Answer:
a. 3.8856x10⁻³M HCl
b. 1.23x10⁻⁴M OH⁻
c. 1.23x10⁻⁴M Ag⁺
d. Ksp = [Ag⁺] [OH⁻]
Explanation:
a. The reaction that you are studying is:
HCl(aq) + AgOH(aq) → H₂O(l) + AgCl(s)
The HCl solution is diluted from 10.00mL to 250.00mL, that is:
250.00mL / 10.00mL = <em>25 -The solution is diluted 25 times-</em>
As original concentration of HCl is 0.09714M, the concentration of the diluted solution is:
0.09714M / 25 =
<h3>3.8856x10⁻³M HCl</h3><h3 />
b. 1 mole of HCl reacts per mole of AgOH, moles of HCl that reacts are:
7.93mL = 7.93x10⁻³L × (3.8856x10⁻³mol HCl / L) = 3.0813x10⁻⁵ moles of HCl.
Based on the reaction, you have in solution
<em>3.0813x10⁻⁵ moles of AgOH = Ag⁺ = OH⁻</em>
The AgOH solution was 250.0mL = 0.2500L, its concentration is:
3.0813x10⁻⁵ moles OH⁻ / 0.2500L =
<h3>1.23x10⁻⁴M OH⁻</h3><h3 />
c. In solution, AgOH produce Ag⁺ and OH⁻ in equals proportions, that means:
1.23x10⁻⁴M OH⁻ =
<h3>1.23x10⁻⁴M Ag⁺</h3><h3 />
d. The solubility product reaction of AgOH(s) is:
AgOH(s) ⇄ Ag⁺(aq) + OH⁻(aq)
Where Ksp for this reaction is defined as:
<h3>Ksp = [Ag⁺] [OH⁻]</h3>
