posted by Anon on .
A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point.
5.00ml of 1.00M NaOH, 200 mL of 1.00M NaOH, 100 mL of 1.00M NaOH, 10,0 mL of 1.00 M NaOH, 150 mL of 1.00M NaOH, 50.0 mL of 1.00M NaOH
HCl + NaOH ==> NaCl + H2O
mols HCl initally = M x L = 1.00 M x 0.1 L = 0.1 mol HCl.
M x L = 1.00 x 0.005L = 0.005 mols must be before.
1.00 x 0.200L = 0.2 mol must be after (02 is more than 0.1 HCl).
1.00 x 0.100L =0.1 mol must be at the equivalence point.