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A 5.00-g quantity of a diprotic acid is dissolved in water and made up to exactly 250 ml. Calculate the molar mass of the acid if 25.0 ml of this solution required 11.1 ml of 1.00 m KOH for neutralization. assume that both protons of the acid are titrated.
Accepted Answer
Here's how to solve the problem:
1. Calculate moles of KOH:
- Moles KOH = (volume KOH)
(concentration KOH)
- Moles KOH = (11.1 mL)
(1.00 mol/L) = 0.0111 mol
2. Calculate moles of diprotic acid:
- Since the acid is diprotic, it requires 2 moles of KOH per mole of acid.
- Moles of acid = (0.0111 mol KOH) / 2 = 0.00555 mol
3. Calculate molar mass:
- Molar mass = (mass of acid) / (moles of acid)
- Molar mass = (5.00 g) / (0.00555 mol) = 900 g/mol
Therefore, the molar mass of the diprotic acid is 900 g/mol.
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