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AnnyKZ [126]
3 years ago
9

A 0.1873 g sample of a pure, solid acid, H2X (a diprotic acid) was dissolved in water and titrated with 0.1052 M NaOH solution.

If the molar mass of H2X is 85.00 g/mol, calculate the volume of NaOH solution needed in the titration.
Chemistry
1 answer:
puteri [66]3 years ago
6 0

Answer:

We need 41.8 mL of NaOH

Explanation:

<u>Step 1:</u> Data given

Mass of H2X = 0.1873 grams

Molarity of NaOH solution = 0.1052 M

Molar mass of H2X = 85.00 g/mol

<u>Step 2</u>: The balanced equation

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

<u>Step 3:</u> Calculate moles of H2X

Moles H2X = mass H2X / Molar mass H2X

Moles H2X = 0.1873 grams / 85.00 g/mol

Moles H2X = 0.0022 moles

<u>Step 4:</u> Calculate 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

<u />

<u>Step 5</u>: Calculate volume of NaOH

Volume of NaOH = moles of NaOH / molarity of NaOH

Volume of NaOH = 0.0044 moles / 0.1052 M

Volume NaOH =  0.0418 L = 41.8 mL

We need 41.8 mL of NaOH

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<em />

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