Question

1. Write a balanced chemical equation for the reaction of sodium hydroxide solution with solid citric acid, H3C6H5O7. 2. Determine the molarity of a sodium hydroxide solution if 37.34 mL of it are required to neutralize 1.922 g of citric acid.

Answer 1

Answer:

0.8 M

Explanation:

Equation of the reaction;

H3C6H5O7(aq) + 3NaOH(aq) ----> Na3C6H5O7(aq) + 3H2O(l)

Number of moles of citric acid = mass/molar mass = 1.922g/192 g/mol= 0.01 moles

If 1 mole of citric acid reacts with 3 moles of NaOH

0.01 moles of citric acid will react with 0.01× 3/1 = 0.03 moles

But concentration = number of moles/volume = 0.03 × 1000/37.34

= 0.8 M