**Calculation of Equivalent Weight of Metal Oxide**

To calculate the equivalent weight of a metal oxide with 32% oxygen, we need to determine the molar mass of the metal and the molecular formula of the oxide. The equivalent weight represents the weight of a substance that can react with or replace one mole of hydrogen ions (H+).

**Step 1: Determine the Molecular Formula of the Metal Oxide**

Let's assume the metal in the oxide is M. The oxide's molecular formula will be MOx, where x represents the number of oxygen atoms. We are given that the oxide contains 32% oxygen, which means that the metal accounts for the remaining 68%.

Since the atomic mass of oxygen is 16 g/mol, we can calculate the metal's atomic mass using the following equation:

68% metal = 100% - 32% oxygen
68% metal = 0.68

Now, we need to find the metal's atomic mass, which can be done by dividing the atomic mass of oxygen by the oxygen percentage and multiplying by the metal percentage:

Atomic mass of metal = (Atomic mass of oxygen / Oxygen percentage) * Metal percentage
Atomic mass of metal = (16 g/mol / 32%) * 68%
Atomic mass of metal = (16 g/mol / 0.32) * 0.68
Atomic mass of metal ≈ 34 g/mol

Therefore, the metal's atomic mass is approximately 34 g/mol.

**Step 2: Calculate the Equivalent Weight**

The equivalent weight is calculated by dividing the molar mass of the substance by the number of moles of hydrogen ions it can react with or replace. In this case, we assume the metal oxide reacts with or replaces one mole of hydrogen ions (H+).

The equivalent weight can be calculated using the following equation:

Equivalent weight = Molar mass / Number of moles of H+

Since we assume the metal oxide reacts with or replaces one mole of H+, the number of moles of H+ is 1.

Therefore, the equivalent weight of the metal oxide is equal to its molar mass.

Equivalent weight = Molar mass = Atomic mass of metal = 34 g/mol

Hence, the equivalent weight of the metal oxide is 34 g/mol.