<h3>
Answer:</h3>
The molecular weight of unknown acid is 33.33 g
<h3>
Explanation:</h3>
- The reaction between an acid and a base such as NaOH is called a neutralization reaction.
- Neutralization titration may be used to standardize a solution or determine the concentration of solution whose molarity is unknown.
- The balanced equation for reaction between an acid and Sodium hydroxide is
HX(aq)+ NaOH(aq) → NaX(aq)+ H₂O(l)
We need to determine the molecular weight of the acid;
<h3>Step 1: Moles of Sodium hydroxide </h3>
Number of moles is given by multiplying molarity and volume of the solution.
Number of moles = Molarity × Volume
= 0.103 M × 0.04365 L
= 0.0045 Moles NaOH
<h3>Step 2: Moles of the acid </h3>
The mole ratio of the acid to NaOH is 1:1
Therefore; the moles of the acid will be 0.0045 moles
<h3>Step 3: Molecular weight of the acid </h3>
Moles of the acid that reacted are 0.0045 moles
Mass of the acid in 0.0045 moles is 0.1500 g
Therefore;
Molecular weight = mass ÷ moles
= 0.1500 g ÷ 0.0045 moles
= 33.33 g/mol
Therefore, the molecular weight of the acid in grams is 33.33 g