3 years ago

11

Chemistry

1 answer:

Ad libitum [116K]3 years ago

8 0

Explanation:

No because the person on the bike is going faster then the person on foot.

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4.0625

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A 5.22 × 10−3−mol sample of HY is dissolved in enough H2O to form 0.088 L of solution. If the pH of the solution is 2.37, what i

OleMash [197]

Answer:

3.07 × 10⁻⁴

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$pH = -log [H^{+} ]\\\[ [H^{+} ] = antilog -pH = antilog -2.37 = 4.27 \times 10^{-3} M$

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$Ca = \frac{5.22 \times 10^{-3} mol }{0.088L} = 0.0593M$

Step 3: Calculate the acid dissociation constant (Ka)

We will use the following expression.

$Ka = \frac{[H^{+}]^{2} }{Ca} = \frac{(4.27 \times 10^{-3} )^{2} }{0.0593} = 3.07 \times 10^{-4}$

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