To neutralize a 0.5192 g organic acid, 44.0 mL NaOH solution (1.00 ml ~ 1.12 mL HCl ~ 0.0100 g CaCO3) is required. What is the equivalent weight of the organic acid?

To find the equivalent weight of the organic acid, we need to use the concept of equivalent weight, which is the mass of a substance that can react with one equivalent of another substance.

First, let's calculate the number of moles of NaOH used to neutralize the organic acid:
Moles of NaOH = (volume of NaOH solution in L) x (concentration of NaOH in mol/L)
Given that the volume of NaOH is 44.0 mL and assuming the concentration of NaOH is 1.00 mol/L:

Volume of NaOH solution = 44.0 mL = 0.0440 L
Concentration of NaOH = 1.00 mol/L

Moles of NaOH = 0.0440 L x 1.00 mol/L = 0.0440 mol

Next, we need to find the moles of the organic acid. Since the number of moles of NaOH is equivalent to the number of moles of the organic acid, we can directly use the moles of NaOH.

Moles of organic acid = 0.0440 mol

Now, we can calculate the molar mass of the organic acid.

Molar mass of the organic acid = (mass of the organic acid in grams) / (moles of organic acid)

Given that the mass of the organic acid is 0.5192 g:

Molar mass of the organic acid = 0.5192 g / 0.0440 mol = 11.80 g/mol

Therefore, the equivalent weight of the organic acid is 11.80 g/mol.