(D) In the compound $MPO_4$,the phosphate ion is $PO_4^{3-}$.Since the compound is neutral,the metal $M$ must have an oxidation state of $+3$ to balan

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(D) In the compound $MPO_4$,the phosphate ion is $PO_4^{3-}$.Since the compound is neutral,the metal $M$ must have an oxidation state of $+3$ to balance the $-3$ charge of the phosphate ion.Therefore,the metal ion is $M^{3+}$.The nitrate ion is $NO_3^-$.Combining $M^{3+}$ and $NO_3^-$ to form a neutral compound,we get $M(NO_3)_3$.

Class 11 Chemistry Some Basic Concepts of Chemistry Atomic, Molecular and Equivalent masses

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The phosphate of a metal has the formula $MPO_4$. The formula of its nitrate will be

A
$MNO_3$
B
$M_2(NO_3)_2$
C
$M(NO_3)_2$
D
$M(NO_3)_3$

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Some Basic Concepts of Chemistry

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Atomic, Molecular and Equivalent masses

Naturally occurring boron has $20\%$ $_5B^{10}$ and $80\%$ $_5B^{11}$. The average atomic weight of boron is

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What should be the equivalent weight of phosphorous acid,if $P=31, O=16, H=1$?

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If $1.2 \, g$ of a metal displaces $1.12 \, L$ of hydrogen at $STP$,the equivalent weight of the metal would be:

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The equivalent weight of $FeS_2$ in the reaction $FeS_2 \to Fe_2O_3 + SO_2$ is (where $M$ is the molecular weight of $FeS_2$):

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The equivalent weight of an acid is equal to

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The phosphate of a metal has the formula $MPO_4$. The formula of its nitrate will be

Similar Questions

Naturally occurring boron has $20\%$ $_5B^{10}$ and $80\%$ $_5B^{11}$. The average atomic weight of boron is

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