The equivalent weight of MnSO4 is half its molecular weight when it is converted to Mn2+.

Explanation:

The concept of equivalent weight is used in stoichiometry to determine the amount of a substance that can react with or be replaced by one mole of another substance. It is often used in redox reactions and acid-base titrations.

Molecular Weight of MnSO4:
To understand the equivalent weight of MnSO4, we first need to determine its molecular weight. MnSO4 is composed of one manganese (Mn) atom, one sulfur (S) atom, and four oxygen (O) atoms. The atomic masses of these elements are as follows:

- Manganese (Mn): 54.938 g/mol
- Sulfur (S): 32.06 g/mol
- Oxygen (O): 16.00 g/mol

To calculate the molecular weight of MnSO4, we multiply the atomic masses by their respective subscripts and sum them up:

Molecular weight of MnSO4 = (1 * Mn) + (1 * S) + (4 * O) = 54.938 + 32.06 + (4 * 16.00) = 54.938 + 32.06 + 64.00 = 150.998 g/mol

Equivalent Weight of MnSO4:
The equivalent weight of a substance is defined as the molecular weight divided by the number of electrons transferred or exchanged in a reaction. In the case of MnSO4, it undergoes a redox reaction where the manganese ion (Mn2+) is formed.

Since the molecular weight of MnSO4 is 150.998 g/mol, we need to determine the number of electrons transferred in the reaction to calculate the equivalent weight.

In the redox reaction, MnSO4 loses two electrons to form Mn2+. Hence, the equivalent weight is calculated as follows:

Equivalent weight of MnSO4 = Molecular weight of MnSO4 / Number of electrons transferred = 150.998 g/mol / 2 = 75.499 g/equiv

Therefore, the equivalent weight of MnSO4 is half its molecular weight, which is 75.499 g/equiv, when it is converted to Mn2+.

MnO2..then it"s equivalent weight will be half of mnso4