Question

The value of the ionic product constant for water $\left(K_w\right)$ at ${60}^o$C is $9.6\times {10}^{14}$ $M^2$. What is the $\left[H_3{O}^{+}\right]$ of a neutral aqueous solution at ${60}^o$C and an aqueous sol ion with a pH = 7.0 at ${60}^o$respectively ?

• A. $3.1\times {10}^{-7}$ acidic
• B. $3.1\times {10}^{-7}$ neutral
• C. $3.1\times {10}^{-8}$ basic
• D. $3.1\times {10}^{-7}$ basic

Answer 1

The correct option is A $3.1\times {10}^{-7}$ acidic

$K_w=9.6\times {10}^{-14}=C_{H_3{O}^{+}}.C_{{OH}^{-}}=C_{H_3{O}^{+}}^2[\because C_{H_3{O}^{+}}=C_{{OH}^{-}}]$

$\therefore C_{H_3{O}^{+}}=\sqrt{9.6\times {10}^{-14}}=3.1\times {10}^{-7}$ acidic