Lesson Worksheet: Volumetric Analysis Chemistry

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In this worksheet, we will practice describing volumetric analysis and using results from titration experiments to calculate the concentration of a solution.

Q1:

A titration experiment was performed to determine the concentration of sulfuric acid using a known concentration of potassium hydroxide. 100 mL of sulfuric acid was placed in a conical flask and a few drops of phenolphthalein indicator were added. A 0.6 M solution of potassium hydroxide was then slowly added into the conical flask. The amount of potassium hydroxide added and any observations were recorded.

Volume of KOH Added (mL) 35.4 35.6 35.8 36.0 36.2 36.4 36.6 36.8 37.0 37.2 37.4 37.6
Observations Colorless Colorless Colorless Pink color that fades quickly to colorless Pink color that fades quickly to colorless Pink color that fades slowly to colorless Pink color that fades slowly to colorless Pink color that lasts ~30 seconds Pink Pink Pink Pink

At what volume was the end point of the reaction reached?

What was the concentration of the sulfuric acid? Give your answer to 3 decimal places.

Q2:

A 30 mL solution of nitric acid was titrated against a 0.1 M solution of potassium hydroxide. The addition of 26.6 mL of potassium hydroxide was found to neutralize the nitric acid. What is the concentration of the nitric acid? Give your answer to 2 decimal places.

Q3:

The concentration of a sample of milk of magnesia, Mg(OH)2, was determined by titration with phosphoric acid (HPO)34. 30 mL of milk of magnesia required 54.8 mL of 0.5 M phosphoric acid to neutralize it. The equation for this reaction is shown: 2HPO+3Mg(OH)6HO+Mg(PO)3422342

What was the concentration of the milk of magnesia?

Q4:

31.8 g of NaCO23 was dissolved to make a 150 mL solution for a titration. The results showed that 44 mL of the NaCO23 solution completely reacted with an unknown concentration of 150 mL of HSO24. What was the concentration of HSO24 to 2 decimal places? [Na=23g/mol, C=12g/mol, O=16g/mol]

Q5:

What volume of 0.5 M sulfuric acid would completely neutralize 125 mL of 0.1 M sodium hydroxide?

Q6:

A standard solution of 0.25 M HSO24 is used to determine the concentration of a 220 mL LiOH solution. The addition of 143 mL of HSO24 resulted in complete neutralization. What is the concentration of the LiOH solution? Give your answer in units of millimolars.

Q7:

During a titration, 22.4 mL of 0.100 M NaOH was required to neutralize the acidic analyte.

Calculate the number of moles of sodium hydroxide in the titer.

  • A0.224 mol
  • B2.24×10 mol
  • C4.46 mol
  • D4.46×10 mol
  • E2.24 mol

Calculate the number of grams of sodium hydroxide in the titer. [Na=23g/mol, O=16g/mol, H=1g/mol]

Q8:

A student performed a neutralization titration. The titration took 80 mL of an 0.500 M NaOH solution to neutralize 241 mL of HCl solution. Determine the concentration of HCl in units of millimolar.

  • A15.0 millimolars
  • B0.166 millimolars
  • C1.50 millimolars
  • D0.500 millimolars
  • E166 millimolars

Q9:

An aqueous solution of NaOH that contains 5 mL of 0.5 M is needed to complete the neutralization of 2.5 M HBr. Determine the final reading in milliliters if the initial reading of the buret was 3.5 mL to the nearest 1 decimal place.

Q10:

A student performs a neutralization titration. The titration took 80.0 mL of a 0.50 M NaOH solution to neutralize 241 mL of HCl solution. Determine the concentration of HCl in units of molarity, giving your answer to 2 decimal places.

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