Ask Question
4 January, 19:42

A 2.40 M aqueous solution of LiCl has a density of 1.0538 g/mL. If the total mass of the solution is 54.0 g, what masses of solute and solvent are present?

+1
Answers (1)
  1. 4 January, 20:51
    0
    5.21 g of solute (LiCl)

    48.79 g of solvent (water)

    Explanation:

    This is our information

    [LiCl] = 2.40 M → 2.40 moles of salt in 1L of solution

    Density of solution: 1.0538 g/mL (solution mass / solution volume)

    54 g → solution mass

    Let's determine solution volume with density

    1.0538 g/mL = solution mass / solution volume

    1.0538 g/mL = 54 g / solution volume

    Solution volume = 54 g / 1.0538 g/mL → 51.2 mL

    Now, we can know the mass of solute, by molarity.

    In 1 L of solution (1000 mL) we know that we have 2.40 mol of chloride.

    Then, how many moles of chloride, do we have in 51.2mL of solution. We make a rule of three:

    1000 mL has 2.40 moles of LiCl

    51.2 mL would have (51.2. 2.40) / 1000 = 0.123 moles of solute

    We apply molar mass to know the mass (mol. molar mass)

    0.123 moles. 42.39 g/m = 5.21 g of LiCl

    Finally solute mass + solvent mass = solution mass

    5.21 g LiCl + solvent mass = 54 g

    54 g - 5.21 g = solvent mass → 48.79 g
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A 2.40 M aqueous solution of LiCl has a density of 1.0538 g/mL. If the total mass of the solution is 54.0 g, what masses of solute and ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers