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The solubility of KNO3 is 25.00 g in 100.00 g of water at 10.0°C. Find the molarity of the solution.

Given: The density of the solution is 1.100 g/mL.

A. 0.150 M
B. 2.50 M
C. 2.18 M
D. 1.55 M
E. 0 M

Answer :

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Final answer:

The molarity of the solution is 2.71 M.

Explanation:

To calculate the molarity of the solution, we need to convert the given mass of KNO3 to moles. The molar mass of KNO3 is 101.1 g/mol.

First, we calculate the moles of KNO3:

  2. Mass of KNO3 = 25.00 g
  4. Molar mass of KNO3 = 101.1 g/mol
  6. Moles of KNO3 = Mass of KNO3 / Molar mass of KNO3

Next, we calculate the volume of the solution in liters:

  2. Mass of the solution = 100.00 g
  4. Density of the solution = 1.100 g/mL
  6. Volume of the solution = Mass of the solution / Density of the solution

Finally, we calculate the molarity:

  2. Molarity = Moles of KNO3 / Volume of the solution

Plugging in the values:

  2. Moles of KNO3 = 25.00 g / 101.1 g/mol
  4. Volume of the solution = 100.00 g / 1.100 g/mL
  6. Molarity = (25.00 g / 101.1 g/mol) / (100.00 g / 1.100 g/mL)

Simplifying the expression:

  2. Moles of KNO3 = 0.247 mol
  4. Volume of the solution = 90.91 mL = 0.09091 L
  6. Molarity = 0.247 mol / 0.09091 L

Therefore, the molarity of the solution is 2.71 M.

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