Titrations: Equivalence Point and Midpoint

5 mols of a base salt was titrated with hydrochloric acid. How many moles of hydrochloric acid are needed to reach the equivalence point?

How many moles of acetic acid does 3 L of a 4 M acetic acid solution contain?

10 mL of 4 M HCl was titrated with an unknown concentration of ammonia to reach the equivalence point. How many moles of ammonia did the starting ammonia solution contain?

If a 3 L solution contains 2 mols of NaCl then the molarity of the solution with respect to NaCl is:

If 5 mL of 0.5 M NaOH was needed to reach the equivalence point when titrated with 2mL of acetic acid. Then the original concentration of the 2 mL acetic acid solution was:

If 100 mL of 0.1 M weak base was needed to reach the equivalence point when titrated with 9 mL of strong acid. Then the original concentration of the strong acid solution was:

How many moles of hydroxide would a 10 mole sample of Mg(OH)₂ produce if it fully dissociated in solution?

60 mL of 0.2 M Ca(OH)₂ was titrated with an unknown concentration of citric acid to reach the equivalence point. How many moles of citric acid did the starting solution contain?

10 mols of base was titrated with acid to reach the equivalence point. How many moles of acid need to be added to the solution to reach the midpoint?

An unknown acid reached its half-equivalence point at a pH of 6.62. Based on this which of the following is the most likely identity of the unknown acid?

Ethanoic acid (pKa = 4.76) was titrated with 3 mols of NaOH to reach the equivalence point. Approximately how many liters of 2 M NaOH are needed to titrate the same ethanoic acid solution to a pH of 4.8?