Question

11.A student titrated a diprotic weak acid (H2A) with 0.100 M NaOH. The titration required 22.58 mL of NaOH solution to reach the equivalence point. How many moles of diprotic acid were present

Answer 1

Moles of diprotic acid present were:

A mole of diprotic acid contains 0.0023 moles $H_{2}A$.

Law of dilution:

Titrations are conducted using the law of dilution.

The number of moles of solute divided by the arrangement's volume in liters is known as molarity.

The number of moles per liter of solution is referred to as molarity. Additionally, we write it as M. Furthermore, we employ the following equation to determine molarity:

Molarity = moles of solute/liter of solution.

Calculation:

Moles of acid = moles of base

n = M/V

Moles of $H_{2}A$ = Moles of NaOH used

Therefore,  0.100 x 0.02258L = 0.0023 mol $H_{2}A$

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