A 0.1873 g sample of a pure, solid acid, H₂X was dissolved in water and titrated with 0.1052 M NaOH solution. The balanced equation for the neutralization reaction occurring is
H₂X(aq) + 2NaOH(aq) $\to$ Na₂X(aq) + 2H₂O(l)
If the molar mass of H₂X is 85.00 g/mol, calculate the volume of NaOH solution needed in the titration.

Question

A 0.1873 g sample of a pure, solid acid, H₂X was dissolved in water and titrated with 0.1052 M NaOH solution. The balanced equation for the neutralization reaction occurring is
H₂X(aq) + 2NaOH(aq)

\to

Na₂X(aq) + 2H₂O(l)
If the molar mass of H₂X is 85.00 g/mol, calculate the volume of NaOH solution needed in the titration.

Quizplus · Accepted Answer

The Answer of A 0.1873 g sample of a pure, solid acid, H₂X was dissolved in water and titrated with 0.1052 M NaOH solution. The balanced equation for the neutralization reaction occurring is H₂X(aq) + 2NaOH(aq) $\to$ Na₂X(aq) + 2H₂O(l) If the molar mass of H₂X is 85.00 g/mol, calculate the volume of NaOH solution needed in the titration.

A 01873 G Sample of a Pure, Solid Acid, H2X Was

A 01873 G Sample of a Pure, Solid Acid, H₂X Was