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Mandarinka [93]
3 years ago
12

Calculate the pH of a solution with [H₃O⁺] = 1 × 10¯⁴ M to the correct number of decimal places.

Chemistry
1 answer:
wolverine [178]3 years ago
7 0
I’m not sure 62840462
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Enough of a monoprotic weak acid is dissolved in water to produce a 0.0144 0.0144 M solution. The pH of the resulting solution i
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Answer:

The value of dissociation constant of the monoprotic acid is 1.099\times 10^{-3}.

Explanation:

The pH of the solution = 2.46

pH=-\log[H^+]

2.46=-\log[H^+]

[H^+]=0.003467 M

HA\rightleftharpoons H^++A^-

Initially

0.0144         0      0

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(0.0144-x)       x       x

The expression if an dissociation constant is given by :

K_a=\frac{[A^-][H^+]}{[HA]}

K_a=\frac{x\times x}{(0.0144-x)}

x=[H^+]=0.003467 M

K_a=\frac{0.003467 \times 0.003467 }{(0.0144-0.003467 )}

K_a=1.099\times 10^{-3}

The value of dissociation constant of the monoprotic acid is 1.099\times 10^{-3}.

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what is ( H+) and (OH-) in a healthy person's blood that has a PH of 7.50 assume that the temperature of the blood is 298 K.
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pH = 7.5

\tt [H^+]=10^{-7.5}=3.16\times 10^{-8}

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\tt [OH^-]=10^{-6.5}=3.16\times 10^{-7}

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