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Study Example 8.1 on page 321. Then, calculate the molarity of a solution made by adding 5.51 g of CaCl2 to enough water to create a solution with a total volume of 2.50 L. Enter only a numerical value in the correct number of significant figures. Use the Periodic Table that is part of your exam to calculate molar mass. Do not enter units in the answer box, but know that the symbol for the unit of this calculation is M

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Answer:

0.0198 M

Explanation:

Given data

  • Mass of CaCl₂ (solute): 5.51 g
  • Volume of solution: 2.50 L

Step 1: Calculate the moles of solute

The molar mass of CaCl₂ is 110.98 g/mol. The moles corresponding to 5.51 g are:

5.51 g × (1 mol/110.98 g) = 0.0496 mol

Step 2: Calculate the molarity of the solution

M = moles of solute / liters of solution

M = 0.0496 mol / 2.50 L

M = 0.0198 M

The Molarity of the solution is 0.0198 M. Molarity is the ratio between the number of moles over Volume of the solution.

Given:

Mass of CaCl₂ (solute): 5.51 g

Volume of solution: 2.50 L

The Calculation for the moles of solute:

The molar mass of CaCl₂ is 110.98 g/mol.

The moles corresponding to 5.51 g are:

5.51 g * (1 mol/110.98 g) = 0.0496 mol

Calculation for Molarity:

M = moles of solute / liters of solution

M = 0.0496 mol / 2.50 L

M = 0.0198 M

Thus, the molarity of the solution is 0.0198 M.

Find more information about Molarity here:

brainly.com/question/17138838

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