Question

What would be the concentration of Ag⁺ if AgCH₃CO₂ was dissolved in 0.01 M HNO₃? AgCH₃CO₂ Ksp = 1.94 x 10^-3; CH₃CO₂H Ka = 1.8 x 10^-5

Answer 1

AgCH₃CO₂(s) + HNO₃(aq) <====>AgNO₃(aq) + CH₃COOH(aq)

Net-ionic equation

AgCH₃CO₂(s) + H⁺(aq) <===> Ag⁺(aq) + CH₃COOH(aq)

But We are given with Ksp of CH₃COOAg

and

To get Keq we have divide Ka fro Ksp

Now we can find Keq

K_eq = 107.8

Using this Keq =107.8 we can find [Ag+]

[H⁺] = 0.01 M

we need [CH₃COO^-] and [CH₃COOAg]

Use ICE able

	CH3COOAg	H+ <===>	CH3COOH	Ag+
Initial	-	0.01	0	0
Change	-	-x	+x	+x
equilibrium	-	0.01-x	x	x

by solving above equation

we get x= 0.01 M

Therefore, molarity of [Ag⁺] = 0.01 M