Finding Impurity of a Sample of Sodium Bicarbonate
Have you ever wondered how pure the chemicals you’re using are? It’s important to know the purity of the chemicals we use in various experiments to ensure accurate results. In this article, we’ll look at a question based on finding the impurity of a sample of sodium bicarbonate and how to solve it.
The Question
Here’s the question:
12.5g of commercial sodium bicarbonate gives 3 g of carbon dioxide. What is the percentage in purity in the sample?
The equation above is the balanced equation for the reaction between sodium bicarbonate and hydrochloric acid. It shows that 2 moles of sodium bicarbonate react with 1 mole of hydrochloric acid to give 1 mole of carbon dioxide, 1 mole of water, and 1 mole of sodium carbonate.
Solving the Problem
Let’s start by finding the molar mass of sodium bicarbonate, which is 84 g/mol. The molar mass of carbon dioxide is 44 g/mol.
We can use stoichiometric calculations to find the expected yield of carbon dioxide. From the balanced equation, we know that 2 moles of sodium bicarbonate gives 1 mole of carbon dioxide. Therefore:
So we expect:
The expected yield of carbon dioxide is:
However, the obtained product is 3 g. We can now calculate the percentage yield:
*** QuickLaTeX cannot compile formula:
\[\text{% yield} = \frac{3 \text{ g}}{3.27 \text{ g}} \times 100\% = 91.74\%\]
*** Error message:
File ended while scanning use of \text@.
Emergency stop.
Conclusion
Based on our calculations, the percentage purity of the sample is 91.74%. This means that the sample contains an impurity of about 8.26%.
It’s important to note that the answer given in the question is 8%. This is incorrect, as our calculation shows that the percentage purity is actually 91.74%. It’s important to double-check your answers and calculations to ensure accuracy.
Final Thoughts
Calculating the purity of a sample of a chemical is an important task in various scientific fields. It’s important to understand the concept of percentage yield and how to calculate it to ensure accurate results. By following the steps outlined in this article, you can easily calculate the percentage purity of a sample of sodium bicarbonate, or any other chemical.
Question Based On Finding Impurity of a Sample of Sodium Bicarbonate
Finding Impurity of a Sample of Sodium Bicarbonate
Have you ever wondered how pure the chemicals you’re using are? It’s important to know the purity of the chemicals we use in various experiments to ensure accurate results. In this article, we’ll look at a question based on finding the impurity of a sample of sodium bicarbonate and how to solve it.
The Question
Here’s the question:
12.5g of commercial sodium bicarbonate gives 3 g of carbon dioxide. What is the percentage in purity in the sample?
The equation above is the balanced equation for the reaction between sodium bicarbonate and hydrochloric acid. It shows that 2 moles of sodium bicarbonate react with 1 mole of hydrochloric acid to give 1 mole of carbon dioxide, 1 mole of water, and 1 mole of sodium carbonate.
Solving the Problem
Let’s start by finding the molar mass of sodium bicarbonate, which is 84 g/mol. The molar mass of carbon dioxide is 44 g/mol.
We can use stoichiometric calculations to find the expected yield of carbon dioxide. From the balanced equation, we know that 2 moles of sodium bicarbonate gives 1 mole of carbon dioxide. Therefore:
So we expect:
The expected yield of carbon dioxide is:
However, the obtained product is 3 g. We can now calculate the percentage yield:
*** QuickLaTeX cannot compile formula: \[\text{% yield} = \frac{3 \text{ g}}{3.27 \text{ g}} \times 100\% = 91.74\%\] *** Error message: File ended while scanning use of \text@. Emergency stop.Conclusion
Based on our calculations, the percentage purity of the sample is 91.74%. This means that the sample contains an impurity of about 8.26%.
It’s important to note that the answer given in the question is 8%. This is incorrect, as our calculation shows that the percentage purity is actually 91.74%. It’s important to double-check your answers and calculations to ensure accuracy.
Final Thoughts
Calculating the purity of a sample of a chemical is an important task in various scientific fields. It’s important to understand the concept of percentage yield and how to calculate it to ensure accurate results. By following the steps outlined in this article, you can easily calculate the percentage purity of a sample of sodium bicarbonate, or any other chemical.