Question

Calculate the solubility of
CuX(*K*sp=[Cu2+][X2?]=1.27

Answer #1

Let the solubility of CuX in NaCN = S mol / L

CuX
Cu^{2+} + X^{2-}

We know that NaCN
Na^{+} + CN^{-}

K_{sp} = [Cu^{2+}][X^{2-}]

But there is no common ion.so its solubility is calculated as follows:

Concentration of Cu^{2+} = S mol / L

Concentration of X^{2-} = S mol / L

Plug the values we get
K_{sp} = [Cu^{2+}][X^{2-}]

K_{sp} = S x S

= S^{2}

So S = (K_{sp} ) ^{1/2}

= ( 1.27

calculate the molar solubility of CuX (for which Ksp=
1.27•10^-36) in each of the following. A.) pure water B.) 0.28 M
CuCl2 C.) 0.18 M Na

Calculate the molar solubility of CuX(Ksp=1.27×10−36) in each of
the following.
a) 0.23 M CuCl2
b) 0.18 M Na2X

Calculate the molar solubility of CuX(Ksp=1.27×10?36)
in each of the following.
Part A
pure water
Express your answer using three significant figures.
Part B
0.25 M CuCl2
Express your answer using two significant figures.
Part C
0.23 M Na2X
Express your answer using two significant figures.

MX (Ksp = 5.67×10−36)
Use the Ksp values to calculate the molar solubility of
each of the following compounds in pure water.

Calculate the solubility of Mercury (I) carbonate, Hg2CO3 if its
solubility product constant, Ksp is 8.9 X 10^-17

Use the Ksp values to calculate the molar solubility of each of
the following compounds in pure water.
MX (Ksp = 1.47×10−38)
Ag2CrO4 (Ksp = 1.12×10−12)

Calculate the molar solubility of Ag2CrO4 (Ksp = 1.1 × 10-12) at
25 °C in various aqueous solutions.
Calculate the solubility in 0.249 M
AgNO3
Calculate the solubility in 0.134 M
Na2CrO4

A. Calculate the solubility of Au(OH)3 in water
(Ksp=5.5×10−46).
B. Calculate the solubility of Au(OH)3 in a solution maintained
at a nitric acid concentration of 1.2 M .

Calculate the molar solubility of Ag2CrO4
(Ksp = 1.1 × 10-12) at 25 °C in
various aqueous solutions.
A)Calculate the solubility in 0.200 M
AgNO3
B)Calculate the solubility in 0.200 M
Na2CrO4

Calculate the molar solubility of PbCl2 in 0.332M
CaCl2. Ksp=1.72 x10-5

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