Explanation:

The equivalent mass of a substance is the amount of that substance in grams that combines or replaces one mole of hydrogen ions (H+), hydroxide ions (OH-), or electrons (e-).

Formula: Equivalent mass (E) = Molecular weight (M) / n

where n is the number of H+ or OH- or electrons involved in the reaction.

In the case of metal M and its sulfate MSO4, we can assume that the reaction involves M reacting with SO4 (sulfate ion).

The equation for the reaction can be written as:

M + SO4 → MSO4

Here, one mole of M combines with one mole of SO4 to form one mole of MSO4.

So, n = 1

Therefore, the equivalent mass of metal M is equal to its atomic weight (since one mole of M reacts with one mole of SO4).

Formula: Equivalent mass (E) = Atomic weight (A)

Now, we need to find the molar mass of MSO4.

Formula: Molar mass of MSO4 = Molar mass of M + Molar mass of SO4

We know the molar mass of M and SO4 separately.

Formula: Molar mass of M = Atomic weight of M

Formula: Molar mass of SO4 = Atomic weight of S + (4 x Atomic weight of O)

Therefore, we can substitute these values in the above equation to get:

Molar mass of MSO4 = Atomic weight of M + Atomic weight of S + (4 x Atomic weight of O)

Final Answer:

Hence, the molar mass of MSO4 would be equal to the sum of the atomic weights of M, S, and O multiplied by their respective coefficients in the formula of MSO4.

Molar mass=Equivalent mass *" n" factor....
M. m=12*2=24 (Charge on SO4*2-= n factor =-2)
Mass of MSO4=24+32+(16*4)=24+32+64=122