The number of ions in $2.2 \times 10^{- 3}$ moles of $Ca {(OH)}_{2} are$

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$14.2 \times 10^{20}$

$10^{20}$

$11 \times 10^{20}$

$39.6 \times 10^{20}$

answer is D.

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Detailed Solution

The balanced chemical reaction is,

$1 Ca {(OH)}_{2} \to 1 \underset{⏟ 3 ions}{{Ca}^{+ 2} + 2 {OH}^{-}}$

In one $Ca {(OH)}_{2}$ molecule 3 ions will present

1 Mole of $Ca {(OH)}_{2}$ has Avogadro’s number, $6 \times 10^{23} of Ca {(OH)}_{2}$ molecules.

One mole of $Ca {(OH)}_{2}$ molecules $= 3 \times 6 \times 10^{23} ions$

Number of ions present in $2.2 \times 10^{- 3} moles of Ca {(OH)}_{2}$

$\frac{2.2 \times 10^{- 3} \times 18 \times 10^{23}}{1 mol Ca {(OH)}_{2}} = 39.6 \times 10^{20} i o n s$

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