What is the normality of a solution containing 20 g of H₂SO₄ (MW = 98)in 500 mL of buffer?

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of H₂SO₄ in the solution: n = m/MW = 20 g / 98 g/mol = 0.204 mole Next, we need to determine the volume of the solution in liters: 500 mL = 0.5 L Finally, we can calculate the normality (N) using the formula: N = (equivalents of solute) / (volume of solution in liters) Since H₂SO₄ can donate one hydrogen ion (H+) in solution, it has one equivalent per mole. Therefore, the number of equivalents in the solution is equal to the number of moles of H₂SO₄. N = 0.204 eq / 0.5 L = 0.408 N ≈ 0.82 N. Therefore, the best choice is C, with a normality of 0.82 N.

What Is the Normality of a Solution Containing 20 G