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Wittaler [7]
3 years ago
7

1.24 grams of magnesium phosphate tribasic dissolved in 1 L of lemon juice. What is the Ksp of the magnesium phosphate tribasic

in lemon juice at room temperature?
a. 2.52e^-10
b. 7.56e^-9
c. 1.26e^-11
d. 6.42e^-10
Chemistry
1 answer:
vivado [14]3 years ago
4 0

<u>Answer:</u> The solubility product of magnesium phosphate tribasic is 2.52\times 10^{-10}

<u>Explanation:</u>

To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}

Given mass of magnesium phosphate = 1.24 g

Molar mass of magnesium phosphate = 262.85 g/mol

Volume of solution = 1 L

Putting values in above equation, we get:

\text{Molarity of solution}=\frac{1.24g}{262.85g/mol\times 1}\\\\\text{Molarity of solution}=4.72\times 10^{-3}M

The equation for the ionization of the magnesium phosphate is given as:

Mg_3(PO_4)_2\leftrightharpoons 3Mg^{2+}+2PO_4^{3-}

Expression for the solubility product of Mg_3(PO_4)_2 will be:

K_{sp}=[Mg^{2+}]^3[PO_4^{3-}]^2

We are given:

[Mg^{2+}]=(3\times 4.72\times 10^{-3})=1.416\times 10^{-2}M

[PO_4^{3-}]=(2\times 4.72\times 10^{-3})=9.44\times 10^{-3}M

Putting values in above expression, we get:

K_{sp}=(1.416\times 10^{-2})^3\times (9.44\times 10^{-3})^2=2.52\times 10^{-10}

Hence, the solubility product of magnesium phosphate tribasic is 2.52\times 10^{-10}

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