Calculate how many times more soluble Mg(OH)_2 is in pure water Based on the giv

Question

Calculate how many times more soluble Mg(OH)_2 is in pure water Based on the given value on of the K_sp Calculate the ratio of solubility of Mg (OH)_2 dissolved in pure H_2 O to Mg (OH)_2 dissolved is a 0.110 MNAOH solution A buffer is mixed solution of a weak acid or base Combined with its Note that this can be underload as a common ion problem The is a common ion added to an system of a weak acid or base. The of the What is the PH change of a 0.290 M solution of acid (pK_a = 4.77) if is added to a of 0.125 M with re change volume?

Explanation / Answer

C)

Find solubility difference in:

Ksp Mg(OH)2 5.61×10–12

pure water:

Ksp = [Mg+2][OH-]^2

5.61*10^-12 = s*(2s)^2

4s^3 = 5.61*10^-12

s =((5.61*10^-12)/4)^(1/3)

S = 0.00011193544 M

when we add

0.110 M of NaOH:

Ksp = [Mg+2][OH-]^2

5.61*10^-12 = (S)(0.11)^2

S = (5.61*10^-12) / ((0.11)^2)

S = 4.636*10^-10

Solubility difference

Swater / Sbase = 0.00011193544 / (4.636*10^-10 ) = 241448.3 times more soluble than water

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