The ionic product of water calculated by a student was found to be 1 - 10-16 mol2 l-2 at 50C- What is the nature of a solution with pH - 7 at the same temperature-

K_w = [H^+]^2 = gt; [H^+] =Kw= 1*10^ 8 pH = log[H^+] = 8 (for neutral solution) = gt; Solutions having pH lt; 8, are acidic solutions. = gt; Solution ...

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Standard X

Chemistry

The ionic pro...

Question

The ionic product of water calculated by a student was found to be $1 \times 10^{(- 16)} m o l^{2} l^{- 2}$ at $5^{0}$ C. What is the nature of a solution with pH = 7 at the same temperature?

Neutral

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Acidic

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Basic

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Cannot be predicted.

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Solution

The correct option is B Acidic
$K_{w} = [H^{+}]^{2}$
=> $[H^{+}]$ = $\sqrt{K_{w}}$ = $1 * 10^{- 8}$
$p H = - l o g [H^{+}] = 8$ (for neutral solution)
=> Solutions having pH < 8, are acidic solutions.
=> Solutions having pH > 8, are basic solutions.

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The ionic product of water calculated by a student was found to be 1×10(−16)mol2l−2 at 50C. What is the nature of a solution with pH = 7 at the same temperature?

The correct option is B AcidicKw=[H+]2 => [H+] =√Kw= 1∗10−8 pH=−log[H+]=8 (for neutral solution) => Solutions having pH < 8, are acidic solutions. => Solutions having pH > 8, are basic solutions.

The ionic product of water calculated by a student was found to be $1 \times 10^{(- 16)} m o l^{2} l^{- 2}$ at $5^{0}$ C. What is the nature of a solution with pH = 7 at the same temperature?

The correct option is B Acidic
$K_{w} = [H^{+}]^{2}$
=> $[H^{+}]$ = $\sqrt{K_{w}}$ = $1 * 10^{- 8}$
$p H = - l o g [H^{+}] = 8$ (for neutral solution)
=> Solutions having pH < 8, are acidic solutions.
=> Solutions having pH > 8, are basic solutions.