Worksheet: Titration Calculations
In this worksheet, we will practice using the results from a titration experiment to calculate unknown properties of a solution.
What volume of 0.5 M sulfuric acid would completely neutralize 125 mL of 0.1 M sodium hydroxide?
The table below shows the results of titrating 0.02 dm3 of barium hydroxide against 0.2 M of hydrochloric acid. Using the results in the table, and discounting any anomalies, determine the concentration of . Give your answer to 2 decimal places.
|Volume of Solution (mL)||Titration 1||Titration 2||Titration 3|
A standard solution of 0.25 M is used to determine the concentration of a 220 mL solution. The addition of 143 mL of resulted in complete neutralization. What is the concentration of the solution? Give your answer in units of millimolars.
An unknown mass of was dissolved to make up a solution of 80 mL. Upon titration, it was found that 60 mL of 4 M completely neutralized the solution.
What was the concentration of the solution?
What mass of was dissolved in the solution? Give your answer in grams.
During a titration, 22.4 mL of 0.100 M was required to neutralize the acidic analyte.
Calculate the number of moles of sodium hydroxide in the titer.
- A0.224 mol
- B mol
- C4.46 mol
- D mol
- E2.24 mol
Calculate the number of grams of sodium hydroxide in the titer.
The concentration of a sample of milk of magnesia, , was determined by titration with phosphoric acid . 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.
What was the concentration of the milk of magnesia?
31.8 g of was dissolved to make a 150 mL solution for a titration. The results showed that 44 mL of the solution completely reacted with an unknown concentration of 150 mL of . What was the concentration of ?
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.
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 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.
What volume of a 3 mol/dm3 solution of ammonia would be needed to completely react with 70 cm3 of a 2 mol/dm3 hydrochloric acid?
20 cm3 of an unknown concentration of acetic acid was placed in a conical flask and titrated against 2 M of sodium hydroxide. The change in pH as sodium hydroxide was added was recorded and is shown below.
What approximate volume of sodium hydroxide neutralized the acetic acid?
- A3.0 cm3
- B4.0 cm3
- C7.5 cm3
- D12.0 cm3
- E8.2 cm3
What was the concentration of the acetic acid solution?
A student sets up an experiment to measure the pH of a solution during titration. A 50 cm3 solution of of unknown concentration is neutralized by the addition of 1 M . The results of the experiment are shown in the graph below.
What is the approximate volume of required to neutralize the sodium hydroxide solution?
- A70 cm3
- B21 cm3
- C55 cm3
- D40 cm3
- E33 cm3
What is the concentration of the sodium hydroxide solution?
A student performed a titration and recorded the volume of acid needed to neutralize a base. The experiment was repeated five times and the results were collected in a table. Which result of repeated titration can be considered an anomaly?
|Volume of Acid (cm3)||17.8||17.9||16.8||17.6||18.0|
A student attempts to determine the concentration of citric acid in an orange. 20 mL of orange juice is titrated against 0.1 M of sodium hydroxide. The following is an equation for the chemical reaction. The student finds that 6.0 mL of sodium hydroxide neutralizes the citric acid. What is the concentration of citric acid in the orange juice? Give your answer in units of mmol/dm3.
A titration experiment is performed 7 times. The first titration is used as a rough estimate of where the end point may be, whilst the remaining six titrations are used to try and provide an accurate measurement. What is the average titer volume? Give your answer to 2 decimal places.
|Volume Added (cm3)||21.8||19.2||19.4||17.6||19.1||18.9||20.6|
A titration is set up to determine the concentration of an ammonia solution. 75 cm3 of ammonia was placed in a conical flask and a few drops of methyl orange indicator were added. A solution that was 0.4 M sulfuric acid was then titrated into the conical flask. The color of the solution near the end point is shown below.
What volume of sulfuric acid completely neutralized the ammonia solution?
What was the concentration of the ammonia solution? Give your answer to 3 significant figures.