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bogdanovich [222]
3 years ago
7

A mysterious compoud with the chemical formula MX (Ksp 1.27x10-36) is present in two different solutions. What is its molar solu

bility in 0.25 M M2SO4?
Chemistry
1 answer:
qwelly [4]3 years ago
4 0

<u>Answer:</u> The molar solubility of MX is 2.54\times 10^{-36}M

<u>Explanation:</u>

We are given:

K_{sp}(MX)=1.27\times 10^{-36}

The chemical equation for the ionization of MX follows:

MX\rightleftharpoons M^+(aq.)+X^-(aq.)

                  S         S

The expression of K_{sp} for above equation is:

K_{sp}=S\times S      ......(1)

The chemical equation for the ionization of M_2SO_4 follows:

M_2SO_4\rightleftharpoons 2M^+(aq.)+SO_4^{2-}(aq.)

 0.25M           0.5M      0.25M

Total concentration of cation from both the equation is:

[M^+]=0.5+S

As, K_{sp}(MX), so S is also very very less than 1 and can be easily neglected.

So, [M^+]=0.5M

Putting values in equation 1, we get:

1.27\times 10^{-36}=0.5\times S\\\\S=2.54\times 10^{-36}M

Hence, the molar solubility of MX is 2.54\times 10^{-36}M

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