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saul85 [17]
3 years ago
5

A 250 mL sample of saturated AgOH solution was titrated with HCl, and the endpoint was reached after 2.60 mL of 0.0136 M of HCl

was dispensed. Based on this titration, what is the Ksp of AgOH?
Chemistry
1 answer:
777dan777 [17]3 years ago
3 0

Answer:

Ksp=1.9×10⁻⁸

Explanation:

First write the balane chemical reaction

AgOH + HCl → AgCl+H2O

Titration reaction occur completely

N-factor of AgOH and HCl is one

normality=molarity

Noermality of HCl=0.0136

N₁ and N₂ are the normality of AgOH and HCl respectively

V₁ and V₂ are the volume of AgOH and HCl respectively

mili equvalent of AgOH-mili equivalent of HCl

N_1=?

V_1=250ml

N_2=0.0136

V_2=2.6ml

N_1V_1=N_2V_2

after puttting all the value we get,

N_1=0.000141 =normality of AgOH solution

molarity=0.000141M

<em>Calculation of Ksp</em>

AgOH⇄Ag⁺  +  OH⁻

Lets solubility=S

<em />[Ag^+]<em>=</em>S

[OH⁻]=S

and S is equal to the concentration of AgOH because that concentration is calculated when solution become satrated.

hence S=0.000141M

Ksp=[Ag+][OH-]

Ksp=S×S

Ksp=1.9×10⁻⁸

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