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What is the molarity of a solution made by dissolving 39.4 g of lithium chloride (LiCl) in enough water to make 1.59 L of solution?

- Molar Mass of Li: 6.94 g/mol
- Molar Mass of Cl: 35.45 g/mol

Answer :

To determine the molarity of the solution, we will follow these steps:

1. Calculate the Molar Mass of Lithium Chloride (LiCl):
- The molar mass of lithium (Li) is 6.94 g/mol.
- The molar mass of chlorine (Cl) is 35.45 g/mol.
- Add these together to find the molar mass of LiCl:
[tex]\[
\text{Molar mass of LiCl} = 6.94\, \text{g/mol (Li)} + 35.45\, \text{g/mol (Cl)} = 42.39\, \text{g/mol}
\][/tex]

2. Calculate the Moles of Lithium Chloride:
- We are given 39.4 g of lithium chloride.
- Use the formula to find moles:
[tex]\[
\text{Moles of LiCl} = \frac{\text{Mass of LiCl}}{\text{Molar mass of LiCl}}
\][/tex]
- Substitute the values:
[tex]\[
\text{Moles of LiCl} = \frac{39.4\, \text{g}}{42.39\, \text{g/mol}} \approx 0.9295 \, \text{mol}
\][/tex]

3. Calculate the Molarity of the Solution:
- Molarity is defined as the number of moles of solute per liter of solution.
- Use the formula:
[tex]\[
\text{Molarity} = \frac{\text{Moles of LiCl}}{\text{Volume of solution in L}}
\][/tex]
- Given the volume of the solution is 1.59 L, substitute the values:
[tex]\[
\text{Molarity} = \frac{0.9295 \, \text{mol}}{1.59 \, \text{L}} \approx 0.5846 \, \text{M}
\][/tex]

Therefore, the molarity of the solution is approximately 0.5846 M.

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