A solution of 0.2 M sulfuric acid is titrated with a 0.2 M basic solution. In three to five sentences, explain how you can use the results of the titration as evidence for the ratio of sulfuric acid and the base in the balanced chemical reaction for the titration.

Answer 1

If the base is monobasic, such as KOH, then
2KOH + H2SO4 ==> K2SO4 + 2H2O
If the base is dibasic, such as Ba(OH)2, then
Ba(OH)2 + H2SO4 ==> BaSO4 + 2H2O
If the base is tribasic, such as Al(OH)3. then
2Al(OH)3 + 3H2SO4 ==> Al2(SO4)3 + 6H2O
In the titration, moles H2SO4 = moles base at the equivalence point. Since the molarity of acid and base are the same and moles = M x L, the ratio of volume (mL) H2SO4 to volume (mL) base will tell you if you have case 1, case 2, or case 3 from above. 1 :1(acid:base) will be a dibasic (case 2). 1:2 (1 mL acid to 2 mL base) will be case 1 above. And a 3 mL acid: 2 mL base will be case 3 above. That's more than 5 sentences but I wanted to be sure you understand it so put this in your own words and follow the instructions in the problem.