Answer :
Answer:
0.0338 moles of sodium bicarbonate are required to react with 0.9 mL 100% sulphuric acid solution
Explanation:
Equation of the reaction:
Na₂CO₃(aq) + H₂SO₄(aq) ---> Na₂SO₄(aq) + H₂O(l) + CO₂(g)
Since the concentration of the sulphuric acid is not given in the question, the assumption is made that the sulphuric acid solution is 100% sulphuric acid solution.
The density of 100% concentrated sulfuric acid is 1.839 g/mL.
Amount of acid in 0.9 mL solution = 0.9 mL * 1.839 g/mL = 1.655 g
Number of moles of acid in 1.655 g = mass/molar mass
Molar mass of H₂SO₄ = 98 g/mol
Number of moles of acid in 1.471 g = 1.655 g / 98 g/mol = 0.0169 moles
From the equation of reaction, 1 mole of H₂SO₄ reacts with 2 moles of Na₂CO₃
0.0169 moles of H₂SO₄ will react with 0.0169 * 2 moles of Na₂CO₃ = 0.0338 moles
Therefore, 0.0338 moles of sodium bicarbonate are required to react with 0.9 mL 100% sulphuric acid solution