Question

calculate the pH of a solution containing 5.6g KOH/250ml​

Answer 1

Answer:

.40 mol/L Explanation: The formula for molar concentration c is c = moles litres Moles = 5.6 g KOH × 1 mol KOH 56.11 g KOH = 0.0998 mol KOH Litres = 250 mL × 1 L 1000 mL = 0.2500 L c = 0.0998 mol 0.2500 L = 0.40 mol/L

Explanation:

Answer 2

Answer:

Therefore the pH of the solution containing 5.6 grams of KOH in 250ml is 13.602.

Explanation:

The given data:

Mass of KOH = 5.6 grams

The volume of the solution = 250 ml

The molar mass of KOH = 56 g/mol

From these the molarity of KOH = $\frac{5.6}{56}$×$\frac{1000}{250}$ = 0.4M

Therefore, the concentration of OH⁻ ions = 0.4M

pOH = -log[OH⁻] = -log[0.4] = 0.398

We know that pH+pOH = 14

pH = 14 - pOH = 14 - 0.398 = 13.602

Therefore the pH of the solution containing 5.6 grams of KOH in 250ml is 13.602.