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Lesson Worksheet: Volumetric Analysis Chemistry
In this worksheet, we will practice describing volumetric analysis and using results from titration experiments to calculate the concentration of a solution.
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.
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.
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 to 2 decimal places? [, , ]
What volume of 0.5 M sulfuric acid would completely neutralize 125 mL of 0.1 M sodium hydroxide?
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.
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. [, , ]
A student performed a neutralization titration. The titration took 80 mL of an 0.500 M solution to neutralize 241 mL of solution. Determine the concentration of in units of millimolar.
- A15.0 millimolars
- B0.166 millimolars
- C1.50 millimolars
- D0.500 millimolars
- E166 millimolars
An aqueous solution of that contains 5 mL of 0.5 M is needed to complete the neutralization of 2.5 M . Determine the final reading in milliliters if the initial reading of the buret was 3.5 mL to the nearest 1 decimal place.
A student performs a neutralization titration. The titration took 80.0 mL of a 0.50 M solution to neutralize 241 mL of solution. Determine the concentration of in units of molarity, giving your answer to 2 decimal places.