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Orlov [11]
2 years ago
5

Calculate the concentration of OH in a solution that contains 3.9 10-4 M H30 at 25°C. Identify the solution as acidic, basic or

neutral. A) 2.6 x 10-11 M, acidic OB) 2.6x 10-11 M, basic OC) 3.9x 10-4 M, neutral D) 2.7 10-2 M, basic
Chemistry
1 answer:
Norma-Jean [14]2 years ago
8 0

Answer:

Option A) 2.6 × 10⁻¹¹ M, acidic.

Explanation:

The ion-product constant of water K_{\rm w} gives a relationship between \rm [H_3O^{+}] and \rm [OH^{-}]:

K_{\rm w} = \rm [H_3O^{+}]\cdot [OH^{-}].

The exact value of K_{\rm w} depends on the temperature. Under \rm 25^{\circ}C, K_{\rm w} \approx 1^{-14}.

The question states that \rm [H_3O^{+}] = 3.9\times 10^{-4}\; M. As a result,

\begin{aligned} {\rm [OH^{-}]} &= \frac{K_{\rm w}}{[{\rm H_3O^{+}}]}\\ &\approx\frac{1^{-14}}{3.9\times 10^{-4}} && \rm {\leftarrow Only~under~25^{\circ}C.}\atop{}\\&\approx \rm 2.6\times 10^{-11}\; M\end{aligned}.

  • A solution is acidic if \rm [H_3O^{+}] > [OH^{-}].
  • A solution is neutral if \rm [H_3O^{+}] = [OH^{-}].
  • A solution is acidic if \rm [H_3O^{+}] < [OH^{-}].

\rm [H_3O^{+}] > [OH^{-}] for this solution. As a result, this solution is acidic.

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See explanation

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