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3 years ago

Write the balanced equation for the formation of the Grignard reagent from bromobenzene.

Chemistry

1 answer:

alexgriva [62]3 years ago

7 0

Answer:

hello your question is incomplete attached below is the complete question

Write the balanced equation for the formation of the Grignard reagent from bromobenzene. Include all reagents and products BUT NOT SOLVENTS.

answer : attached below

Explanation:

I mol mg + 1 mol bromobenzene = 1 mol Grignard

attached below is the balanced equation for the formation of the Grignard reagent from bromobenzene

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<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

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Putting values in above equation, we get:

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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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