Question

The normality of 500ml of ca (oh)2 solution which contains 9.033×10^22 hydroxide ions is

Answer 1

Answer:

$Normality = 48\times 10^{20}\ N$

Explanation:

As per the question,

We know that,

Normality is just another procedure to check the concentration of solute in solution much similar to Molarity.

Mathematically it is represented as,

$Normality = \frac{Weight\ of\ solute\times valency\ factor} {volume\ in\ liters\times molecular\ weight}$

Given:

Weight of solute = 9.033 × 10²²

For calcium hydroxide valence factor is 2.

Volume  = 500 ml = 0.5 l

Molar mass of Ca(OH)₂  =  40+( 16+1) × 2 = 74 gms

So,

$Normality = \frac{Weight\ of\ solute\times valency\ factor} {volume\ in\ liters\times molecular\ weight}$

$Normality = \frac{9.033\times 10^{22}\times 2} {0.5\times 74}$

$Normality = 48\times 10^{20}\ N$

Hence, $Normality = 48\times 10^{20}\ N$