a 0.1873 g sample of pure solid acid, h2x was dissolved in water and titrated with 0.1052 m naoh solution. if 41.89 ml of the naoh solution is needed to reach the equivalence point, calculate the molar mass of the acid.

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bharathparasad577 bharathparasad577 · Answer 1 · 2022-11-24T17:47:51+01:00

The molar mass of given acid H₂X is 85.1g/mol

Mass of the H₂X = 0.1873 grams

Molarity of NaOH = 0.1052 M

Thus, the balanced equation

H₂X (aq) +2 NaOH (aq) → Na₂X (aq) + 2H₂O(l)

Calculating moles of NaOH

For 1 mol H₂X we need 2 moles NaOH to produce 1 mole of Na₂X and 2 moles of H₂O

For 0.0022 moles of H₂X we need 0.0044 moles of NaOH

Volume of the NaOH = moles of NaOH / molarity of NaOH

Volume of the NaOH = 0.0044 moles / 0.1052 M

Volume of the NaOH = 0.04189 L = 41.89 mL

We just need 41.8 mL of NaOH

Since number of moles of H₂X is 0.0022

Number of moles= Mass/ Molar mass

0.0022= 0.1873/ Molar mass

Molar mass= 0.1873 / 0.0022

= 85.1 g/mol

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