Considering a solution that is made from mixing 35ml of 0.22M AgNO3 and 83ml of

Question

Considering a solution that is made from mixing 35ml of 0.22M AgNO3 and 83ml of 0.22M Na2SO4? a) how much silver sulfate forms? b) what is the concentration of silver ions and sulfate ions at equilibrium Considering a solution that is made from mixing 35ml of 0.22M AgNO3 and 83ml of 0.22M Na2SO4? a) how much silver sulfate forms? b) what is the concentration of silver ions and sulfate ions at equilibrium a) how much silver sulfate forms? b) what is the concentration of silver ions and sulfate ions at equilibrium

Explanation / Answer

a)

[Ag+] = 35 x 0.22 / (35+83) = 0.0652 M

[SO4-2] = 0.22 x 83 / 35+83 = 0.155 M

2Ag+    + SO4-2 ---------------------> Ag2SO4

2                 1                                   1

0.0652      0.155                                 ?

2 M ------------------> 1 M Ag2SO4

0.0652 M ---------------------> x M Ag2SO4

Ag2SO4 molarity = 1 x 0.0652 / 2 = 0.0326 M

total volume = 35 + 83 = 118 mL = 0.118 L

moles of Ag2SO4 = 0.0326 x 0.118 = 3.85 x 10^-3

mass of Ag2SO4 = 3.85 x 10^-3 x 311.8 = 1.2 g

mass of Ag2SO4 formed = 1.20g

2 M Ag+----------------> 1 M SO4-2

0.0652 M Ag+ -------------> 0.0326 M SO4-2

remaining SO4-2 = 0.155 - 0.0326 = 0.1224 M

equilibrium concentration of SO4-2 = 0.1124 M

Ag2SO4 -------------------> 2Ag+ SO4-2

Ksp = [Ag+]^2 x 0.1124

1.20 x 10^-5 = [Ag+]^2 x 0.1124

[Ag+] = 0.01 M

equilibrium concentration of Ag+   = 0.01 M

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