Question

You create solutions of H2S04 and NaOH with concentrations of 1.23 and 0.81,respectively. If you titrate 10.0 mL of the H2S04 solution with the NaOH base you have created, at what volume do you expect to see the equivalence point? mL NaOH = 15.2 X If the actual mL used is 29.9, what was the actual concentration of the base assuming the acid concentration was correct? Actual [NaOH] If the actual mL used is 29.9, what was the actual concentration of the acid aรsuming the base concentration was correct? Actual [H2SO4 ] = what is the %error (+ or-) in each case? %Err = (Actual-Given)/Actual x 100% %error [NaOH] %error [H2SO4 ]-

Answer 1

This question was based on the Molarity and Volume relationship between the two compounds. So using the relationship between M1V1= M2V2 we find the values.