The phosphate of a metal M has the formula M_ | vedclass

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(A) In the formula $M_3(PO_4)_2$,the phosphate ion $(PO_4)^{3-}$ has a valency of $3$. Since there are two phosphate ions,the total negative charge is

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$MSO_4$

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(A) In the formula $M_3(PO_4)_2$,the phosphate ion $(PO_4)^{3-}$ has a valency of $3$. Since there are two phosphate ions,the total negative charge is $2 	imes 3 = 6$. To maintain electrical neutrality,the three metal ions $M$ must provide a total positive charge of $6$. Therefore,each metal ion $M$ has a charge of $+2$,meaning $M$ is divalent $(M^{2+})$. The sulphate ion is $(SO_4)^{2-}$. Combining $M^{2+}$ and $(SO_4)^{2-}$ in a $1:1$ ratio gives the formula $MSO_4$.

Isotope	$\%$ Natural abundance	Molar mass
$^1H$	$99.985$	$1$
$^2H$	$0.015$	$2$

The phosphate of a metal $M$ has the formula $M_3(PO_4)_2$. What is the formula for its sulphate?

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