Asked by Anon
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
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
Answers
Answered by
DrBob222
HCl + NaOH ==> NaCl + H2O
mols HCl initally = M x L = 1.00 M x 0.1 L = 0.1 mol HCl.
NaOH
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.
Etc.
mols HCl initally = M x L = 1.00 M x 0.1 L = 0.1 mol HCl.
NaOH
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.
Etc.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.