Calcium chloride when dissolved in water dissociates into its ions according to the following equation. ${CaCl}_{2} (aq) \to {Ca}_{}^{2 +} (aq) + 2 {Cl}_{}^{-} (aq)$ . Calculate the number of ions obtained from ${CaCl}_{2}$ when $222 g$ of it is dissolved in water.

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Solution

Step 1: Finding the molecular mass of Calcium chloride:
The molecular mass of $1 mole$ of ${CaCl}_{2}$ = $111 g$
So, for the $2 moles of {CaCl}_{2}$ would be equivalent to $222 g$ .
As the 1 formula unit of ${CaCl}_{2}$ is giving 3 ions.
So, $2 moles$ of ${CaCl}_{2}$ would give = $2 \times 3 = 6 ions$ .
Step 2: Finding the total number of ions dissolved.
Because $Number of ions = Number of moles of ions \times Avogadro number$
$As, Avogadro number = 6.023 \times 10^{23}$
Therefore, $Number of ions = 6 \times 6.023 \times 10^{23}$
$Number of ions = 36.132 \times 10^{23}$
Therefore, the number of ions obtained from ${CaCl}_{2}$ when $222 g$ of it is dissolved in water = $3.6132 \times 10^{24} ions$

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