Question
2.8 g of KOH is dissolved in a 500 mL solution at 298 K. What is the p^H of solution ? (molar mass of KOH = 56 g/mol)
MHT CET
Chemistry
Ionic Equilibrium
2026
MHT CET 2026 (11 April Shift 2)
MHT CET Chemistry Question (2026) — Solution
Options
- A. 1
- B. 8
- C. 11
- D. 13
Answer
D. 13
Step-by-step solution
Moles of KOH = 2.8 56 = 0.05 mol Volume of solution = 500 mL = 0.5 L Molarity of KOH = 0.05 0.5 = 0.1 M Since KOH is a strong base, it dissociates completely in water. [OH^ - ] = 0.1 M = 10^ -1 M pOH = - [OH^ - ] = - (10^ -1 ) = 1 At 298 K, pH + pOH = 14 pH = 14 - 1 = 13 Answer: 13
Related: Chemistry — Ionic Equilibrium · All PYQ Banks