Question

1. How many grams of CaCl2 would be required to produce a 3.5 M (molar) solution with a volume of 2.0 L?

Answer 1

How many grams of CaCl2 would be required to produce a 3.5 M (molar) solution with a volume of 2.0 L?

**Solution:**

We use the equation of molar concentration:

$$C _ {M} = \frac {m}{M \cdot V}.$$

From periodic table we determine the molar mass of $\mathrm{CaCl}_2$ it equates:

$\mathrm{M(CaCl_2)} = 40.078 + 35.453\cdot 2 = 110.984\mathrm{g / mol}$

The mass of $\mathrm{CaCl}_2$ calculate from the formula above: $m = C_{M} \cdot M \cdot V = 3.5 \cdot 110.984 \cdot 2.0 = 776.888 \, \text{g}$ .

**Answer:** The mass of $\mathrm{CaCl}_2$ is 776.888 g.