Consider the titration of HC 2 H 3 O 2 with NaOH. If it requires 0.00339 mol of
ID: 795895 • Letter: C
Question
Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?
Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?
Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?
Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?
Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?
Consider the titration of HC2H3O2 with NaOH. If it requires 0.00339 mol of NaOH to reach the endpoint, and if we had originally placed 16.53 mL of HC2H3O2 in the Erlenmeyer flask to be analyzed, what is the molarity of the original HC2H3O2 solution?
Explanation / Answer
No. of moles = MV
where M= molarity
V = volume of solution (litres)
No. of moles of NaOH= 0.00339 mol
For titration,
M1v1 = M2v2
0.00339 = M2 * (16.53 /1000)
M2= 3.39/ 16.53
= 0.205M answer