Question

You create solutions of H2SO4 and NaOH with concentrations of 1.13 and 0.84, respectively. If you titrate 10.0 mL of the H2SO4 solution with the NaOH base you have created, at what volume do you expect to see the equivalence point? ml NaOH = If the actual mL used is 30.6, what was the actual concentration of the base assuming the acid concentration was correct? Actual (NaOH) = L M If the actual mL used is 30.6, what was the actual concentration of the acid assuming the base concentration was correct? Actual [H2SO4 ] = M What is the %error (+ or -) in each case? %Err = (Actual - Given)/Actual x 100% %error [NaOH] = %error (H2SO4) =

Answer 1

Comment in case of any doubt.

→ Hy sou gives aht (dibasic) and NaOH gives 1 Oh. (monoacidre), so at equivalence mmoles of NaOH = ax mnoles of the sou millimales - 0.84 mol X Vanoin = ax 1.13 mol x 10ml » Vraoh = [2619 mL of No0H mmoles of 4t given by Hesou - Actual [naor] =12x1.13 mex some = 0.739 M=(0.74M] 30.6ml mondes of Oh given by NADH - Actual [H₂SO4] = 10.84 mnd + 30.6 ml? L = 1.2852=1.29M 2x loml aht per Hagou Î 0.74 % error (Naor] = 3 - 0.74 - 0.84 -X100 = 1 – 13.5% % error [H₂SO4] = 1.29-1.13 (12.11% Î - X100 = 1 1. 29