Which one of the following statements is correct?

Options

A. Bronsted-Lowry theory could not explain the acidic nature of `BCl_(3)`
B. The pH of 0.01 M NaOH solution is 2
C. The ionic product of water at `25^(circ)C is 10^(-10) mol^(2) L^(-2)`
D. The pH of a solution can be calculated using the equation, `pH = -"log" [H^(+)]`

Answer

A

Explanation

pH of 0.01 NaOH,`pOH = -"log"[H^(-)] = -"log"(0.01) = -"log"(10^(-2)) = 2`
pH = 14 - pOH = 14 - 2 = 12
Ionic product of water at `25^(circ)C is 10^(-14)mol^(2)//L^(2)`
Equation used for calculating `p^(H)` of a solution is `pH = -"log"[H^(+)]`
Bronsted-lowry theory could not explain the acidic nature of `BCl_(3)`