Question

Find the pOH of a solution made by dissolving 10.4g of HCl in a 500mL solution of water

Answer 1

The pOH of a solution : 13.756

Further explanation

Mass HCl=10.4 g

mol HCl (MW=36.5 g/mol) :

$\tt mol=\dfrac{mass}{MW}=\dfrac{10.4}{36.5}=0.285$

Volume of HCl = 500 ml = 0.5 L

$\tt M=\dfrac{n}{V}\\\\M=\dfrac{0.285}{0.5}=0.57~M$

HCl ⇒ H⁺ + Cl⁻

[H⁺]=[HCl]=0.57 M

pH= - log[H⁺]

pH=-log[0.57]=0.244

pH+pOH=14

pOH=14-0.244

pOH=13.756