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4 years ago

15

Find the hydroxide ion concentration of a HBr solution with a pH of 4.75

1 answer:

Sunny_sXe [5.5K]4 years ago

8 0

1st find the pOH = 14 - 4.75 = 9.25
then do 10^-9.25 = 5.62x10^-10 OH- concentration

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As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the po

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$K_{sp} = [CH_{3}COO^{-}][X^{+}]$

$[CH_{3}COO^{-}] = \frac{K_{sp}}{[X^{+}]} = \frac{9.40 \cdot 10^{-6}}{5.00 \cdot 10^{-3}} = 1.88 \cdot 10^{-3} M$

By entering the values of [CH₃COO⁻] and Ka, into equation (2) we can calculate [H₃O⁺]:

$[H_{3}O^{+}] = \frac{1.74 \cdot 10^{-5}*[1.00]}{[1.88 \cdot 10^{-3}]} = 9.26 \cdot 10^{-3} M$

Hence, the pH is:

$pH = -log [H_{3}O^{+}] = -log [9.26 \cdot 10^{-3}] = 2.03$

Therefore, the pH must be 2.03 to yield a solution in which the concentration of X⁺ is 5.00x10⁻³M.

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