Question

You create solutions of H₂SO₄ and NaOH with concentrations of 1.12 and 0.81,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 31.8, what was the actual concentration of the base assuming the acid concentration was correct? Actual [NaOH] =   M
If the actual mL used is 31.8, 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

f? CAR o.ol it Ool lit it So, 0.0112 X 2 2 0.02D4 M.№01t 0.022YM F0.02 765 ut づŠ tuo aehnl mL 1.ced Is 31.g-:m»Ky. The aetval cNao 0-022y 4 ισσο 0 025 58 H NoD4 IDrnl2u.cn t正 -02575S M dividd by 2 mol N

스-15 % 287 2 13-03 13%