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I am given 4 statements to choose from and find which is correct about a neutral solution:

  1. $K_\mathrm{w} = \pu{1.00\times10^-14 mol^2 dm^{-6}}$
  2. The solution contains only $\ce{H2O}$
  3. $\ce{[H+] = [OH-]}$
  4. $\ce{pH =7}$

I can see that the first statement is wrong as that is only the case at $\pu{25 ^\circ C}$.

The second statement is also incorrect - it can be when $\ce{H+}$ ions and $\ce{OH-}$ are equal in concentration. So I can see that option 3 is correct.

However, I am confused why option 4 is wrong. Why is option 4 wrong?

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    $\begingroup$ What happens to [H+] if Kw =/= 10^-14? Say if it's 10^-12? $\endgroup$ Jun 9, 2017 at 11:41

1 Answer 1

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As the temperature changes the value of $K_\mathrm{w}$ changes(as you wrote) and then the concentration of $\ce{H^+}$ and $\ce{OH^-}$ also changes and now the concentration of $\ce{H^+}$ will not remain $10^{-7}$ and hence the neutral point shifts. Therefore, at any temperature the $\ce{pH}$ of neutral point is not 7.

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  • $\begingroup$ Always welcome. Friend! $\endgroup$ Jun 9, 2017 at 16:04

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