Volumetric Analysis and Calculations
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i) Using the information from the figure, complete the table below. (3 marks)
| | 1 | 2 | 3 |
|---|---|---|---|
| Final burette reading/cm$^3$ | | | |
| Initial burette reading/cm$^3$ | | | |
| Volume of solution X used/cm$^3$ | | | |
ii) Calculate the volume of X needed to neutralise 25 cm$^3$ of Y. (1 mark)
iii) Calculate the concentration of sulfuric acid in solution X in mol dm$^{-3}$. (1 mark)
iv) Calculate the number of moles of sulfuric acid used in the titration. (1 mark)
v) Write a balanced equation for the reaction. (2 marks)
vi) Determine the number of moles of sodium hydroxide in the 25.0 cm$^3$ of solution Y used. (1 mark)
vii) Calculate the concentration of sodium hydroxide in solution Y in mol dm$^{-3}$. (1 mark)
This question includes visual content: A diagram shows three pairs of burette readings labeled 'titration 1', 'titration 2', and 'titration 3'. Each titration has a 'before' and 'after' burette scale. - Titration 1: 'before' is 0.0, 'after' is 17.8. - Titration 2: 'before' is 2.0, 'after' is 19.8. - Titration 3: 'before' is 4.0, 'after' is 22.0. Below the diagram is a table titled 'Titration number' with columns 1, 2, 3 and rows for 'Final burette reading/cm^3', 'Initial burette reading/cm^3', and 'Volume of solution X used/cm^3'.
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Step by Step Written Solution
Hi Taliah, let's work through this titration problem together by reading the burette values and performing the chemical calculations.
Titration Analysis
First, we need to read the volume of solution X from the burettes. For Titration one, the liquid level is at point four cubic centimeters before and seventeen point eight after.
i) Reading the Burette
| Titration | 1 | 2 | 3 |
|---|---|---|---|
| Final (cm^3) | 17.8 | 19.8 | 22.6 |
| Initial (cm^3) | 0.4 | 2.5 | 4.8 |
| Volume (cm^3) | 17.4 | 17.3 | 17.8 |
We subtract the initial reading from the final reading to get the volume used for each trial. For Titration two, it is nineteen point eight minus two point five, which equals seventeen point three. For Titration three, twenty-two point six minus four point eight gives seventeen point eight.
In part two, we calculate the average volume of X needed to neutralize twenty-five cubic centimeters of Y. We take the mean of our titration results.
ii) Average Volume of X
The sum is fifty-two point five, and dividing by three gives us an average volume of seventeen point five cubic centimeters.
For part five, let's write the balanced chemical equation. Sulfuric acid reacts with sodium hydroxide to produce sodium sulfate and water.
v) Balanced Equation
Looking at parts three and four, we'll assume a standard concentration for solution X. If the concentration of sulfuric acid is zero point one moles per cubic decimeter, we can find the moles used.
iii & iv) Moles of H2SO4
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