# Calculate the molar solubility of CuX Ksp = 1.27 x 10^-36 in each of the following.?

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Calculate the molar solubility of CuX Ksp = 1.27 x 10^-36 in each of the following.?

0.27M CuCl2

0.19M Na2X

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CuX = Cu2+ + X2-

Ksp = [Cu2+] * [X2-]

for each mole of CuX that dissolves we get x mol of each of the anions and cations

Ksp = x^2 = 1.27 x 10 ^-36

x= 1.13 x 10 ^-18 moles of CuX per liter of pure water

if the solution has [Cu2+]= 0.27 M

Ksp becomes x ( x + 0.27)

as we can see above x is extremely small so can be ignored inside the brackets

0.27 x = 1.27 x 10^-36

x = 1.27 x 10^-36 / 0.27 = 4.70 x 10 ^-36 moles per liter

In 0.19M X2- we have

Ksp = 0.19x = 1.27 x 10^-36

x = 1.27 x 10^-36 / 0.19 = 6.68 x 10 ^-36 moles per liter ..

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update

in 0.23M Na2X

S = 5.5x10^-36

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