Worksheet: Titration Calculations

In this worksheet, we will practice using titer volumes measured in a titration to calculate the analyte concentration or solute composition.

Q1:

Sulfuric acid (HSO)24 is a diprotic acid. A 36.3 mL aliquot of 0.0529 M aqueous sulfuric acid was titrated against 0.0411 M aqueous sodium hydroxide. Calculate the volume of the sodium hydroxide solution needed to reach the endpoint of the titration.

Q2:

Phosphoric acid (HPO)34 is a triprotic acid. A 13.8 mL aliquot of 0.176 M aqueous phosphoric acid was titrated against 0.110 M aqueous sodium hydroxide. Calculate the volume of sodium hydroxide solution needed to reach the endpoint of the titration.

Q3:

Oxalic acid (CHO)224 is a diprotic acid. A solid sample with a mass of 0.7984 g, containing oxalic acid, was titrated against 0.2283 M aqueous sodium hydroxide. Calculate the percent mass of oxalic acid in the sample given that 37.98 mL of the sodium hydroxide solution was needed to reach the endpoint of the titration.

Q4:

Sulfuric acid (HSO)24 is a diprotic acid. A 31.5 mL aliquot of aqueous sulfuric acid was titrated against 0.0134 M aqueous sodium hydroxide. Calculate the molar concentration of the aqueous sulfuric acid given that 23.9 mL of the sodium hydroxide solution was needed to reach the endpoint of the titration.

Q5:

A 20 mL sample of aqueous nitric acid (HNO)3 is titrated against a 0.047 M solution of barium hydroxide (Ba(OH)2). What is the concentration of the nitric acid if an average volume of 55 mL of barium hydroxide solution is needed to reach the end-point of the titration?

Q6:

Adding aqueous mercury(II) nitrate to aqueous chloride ions results in the precipitation of mercury(II) chloride, as shown. 2Cl()+Hg(NO)()2NO()+HgCl()3232aqaqaqs

Calculate the concentration of chloride ions in a 0.250 mL aqueous sample if 1.46 mL of 0.825 mM aqueous mercury(II) nitrate is required for the end point to be reached.

Q7:

A solution of NaCN is titrated against a standard 0.0100 M solution of AgNO3. When cyanide ions are in excess, the silver ions react to produce the soluble Ag(CN)2 complex. However, when silver ions are in excess, solid AgCN precipitates. If AgCN begins to precipitate after the addition of 28.72 mL of the AgNO3 titrant, how many grams of NaCN are present in the analyte solution?

Nagwa uses cookies to ensure you get the best experience on our website. Learn more about our Privacy Policy.