In Order To Prepare A 0.668 M Aqueous Solution Of Potassium Iodide (KI), How Many Grams Of Potassium Iodide Must Be Added To 3.69 Kg Of Water? Answer To 1 Decimal Place.

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Introduction

Preparing a solution of a specific concentration is a crucial task in various fields, including chemistry, biology, and medicine. In this article, we will focus on preparing a 0.668 m aqueous solution of potassium iodide (KI). To achieve this, we need to calculate the amount of potassium iodide required to be added to a given volume of water. In this case, we have 3.69 kg of water, and we need to determine the mass of potassium iodide that must be added to it.

Understanding Molarity

Molarity (m) is a measure of the concentration of a solution, expressed as the number of moles of solute per liter of solution. It is calculated using the formula:

m = moles of solute / liters of solution

In this case, we are given a molarity of 0.668 m, which means that there are 0.668 moles of potassium iodide per liter of solution.

Calculating the Number of Moles of Potassium Iodide

To calculate the number of moles of potassium iodide required, we need to know the volume of the solution. Since we are adding the potassium iodide to 3.69 kg of water, we can assume that the volume of the solution will be approximately equal to the volume of the water. The density of water is approximately 1 g/mL, so we can calculate the volume of the water as follows:

Volume of water (L) = mass of water (g) / density of water (g/mL) = 3690 g / 1 g/mL = 3.69 L

Now, we can calculate the number of moles of potassium iodide required using the formula:

moles of KI = molarity (m) x volume of solution (L) = 0.668 m x 3.69 L = 2.46 mol

Calculating the Mass of Potassium Iodide

To calculate the mass of potassium iodide required, we need to know the molar mass of potassium iodide. The molar mass of potassium iodide is approximately 166.0 g/mol.

Mass of KI (g) = moles of KI x molar mass of KI (g/mol) = 2.46 mol x 166.0 g/mol = 408.36 g

Rounding the Answer to 1 Decimal Place

Since we are asked to round the answer to 1 decimal place, we can round the mass of potassium iodide to 408.4 g.

Conclusion

In this article, we have calculated the mass of potassium iodide required to prepare a 0.668 m aqueous solution. We have used the formula for molarity and the molar mass of potassium iodide to determine the number of moles of potassium iodide required, and then calculated the mass of potassium iodide required. The final answer is 408.4 g.

Additional Information

  • The molar mass of potassium iodide is approximately 166.0 g/mol.
  • The density of water is approximately 1 g/mL.
  • The volume of the solution is approximately equal to the volume of the water.

References

  • CRC Handbook of Chemistry and Physics, 97th Edition.
  • International Union of Pure and Applied Chemistry (IUPAC) Compendium of Chemical Terminology.

To calculate the number of moles of potassium iodide in a 0.668 m solution, we can use the formula:

moles of KI = molarity (m) x volume of solution (L) = 0.668 m x 3.69 L = 2.46 mol

To calculate the mass of potassium iodide in a 0.668 m solution, we can use the formula:

mass of KI (g) = moles of KI x molar mass of KI (g/mol) = 2.46 mol x 166.0 g/mol = 408.36 g

Rounding the Answer to 1 Decimal Place

Since we are asked to round the answer to 1 decimal place, we can round the mass of potassium iodide to 408.4 g.

Conclusion

In this article, we have calculated the mass of potassium iodide required to prepare a 0.668 m aqueous solution. We have used the formula for molarity and the molar mass of potassium iodide to determine the number of moles of potassium iodide required, and then calculated the mass of potassium iodide required. The final answer is 408.4 g.

Additional Information

  • The molar mass of potassium iodide is approximately 166.0 g/mol.
  • The density of water is approximately 1 g/mL.
  • The volume of the solution is approximately equal to the volume of the water.

References

  • CRC Handbook of Chemistry and Physics, 97th Edition.
  • International Union of Pure and Applied Chemistry (IUPAC) Compendium of Chemical Terminology.
    Frequently Asked Questions (FAQs) About Preparing a Potassium Iodide Solution ====================================================================================

Q: What is the molarity of a 0.668 M potassium iodide solution?

A: The molarity of a 0.668 M potassium iodide solution is 0.668 moles of potassium iodide per liter of solution.

Q: How many grams of potassium iodide are required to prepare a 0.668 M solution?

A: To calculate the mass of potassium iodide required, we need to know the molar mass of potassium iodide. The molar mass of potassium iodide is approximately 166.0 g/mol. Using the formula:

mass of KI (g) = moles of KI x molar mass of KI (g/mol) = 2.46 mol x 166.0 g/mol = 408.36 g

Q: What is the volume of the solution required to prepare a 0.668 M solution?

A: Since we are adding the potassium iodide to 3.69 kg of water, we can assume that the volume of the solution will be approximately equal to the volume of the water. The density of water is approximately 1 g/mL, so we can calculate the volume of the water as follows:

Volume of water (L) = mass of water (g) / density of water (g/mL) = 3690 g / 1 g/mL = 3.69 L

Q: How do I calculate the number of moles of potassium iodide required to prepare a 0.668 M solution?

A: To calculate the number of moles of potassium iodide required, we can use the formula:

moles of KI = molarity (m) x volume of solution (L) = 0.668 m x 3.69 L = 2.46 mol

Q: What is the molar mass of potassium iodide?

A: The molar mass of potassium iodide is approximately 166.0 g/mol.

Q: How do I round the answer to 1 decimal place?

A: To round the answer to 1 decimal place, we can round the mass of potassium iodide to 408.4 g.

Q: What are some additional things I should know about preparing a potassium iodide solution?

A: Some additional things you should know about preparing a potassium iodide solution include:

  • The density of water is approximately 1 g/mL.
  • The volume of the solution is approximately equal to the volume of the water.
  • The molar mass of potassium iodide is approximately 166.0 g/mol.

Q: Where can I find more information about preparing a potassium iodide solution?

A: You can find more information about preparing a potassium iodide solution in the following resources:

  • CRC Handbook of Chemistry and Physics, 97th Edition.
  • International Union of Pure and Applied Chemistry (IUPAC) Compendium of Chemical Terminology.

Conclusion

In this article, we have answered some frequently asked questions about preparing a potassium iodide solution. We have covered topics such as the molarity of a 0.668 M solution, the mass of potassium iodide required, the volume of the solution, and the molar mass of potassium iodide. We have also provided some additional information and resources for further learning.