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ad-work [718]
3 years ago
15

Calculate the [ OH − ] and the pH of a solution with an [ H + ] = 0.090 M at 25 °C . [ OH − ] = M pH = Calculate the [ H + ] and

the pH of a solution with an [ OH − ] = 0.00098 M at 25 °C . [ H + ] = M pH = Calculate the [ H + ] and the [ OH − ] of a solution with a pH = 10.15 at 25 °C . [ H + ] = M [ OH − ] =
Chemistry
1 answer:
Valentin [98]3 years ago
3 0

Answer:  a) [OH^-]=1.09\times 10^{-13} and pH = 1.04

b) [H^+]=1.02\times 10^{-11}  and pH=10.99

c) [H^+]=7.08\times 10^{-11} and [OH^-]=1.41\times 10^{-4}

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

pH=-\log [H^+]

pOH=-\log [OH^-]

pH+pOH=14

a) [H^+]=0.090M

pH=-\log [0.090]=1.04

pOH=14-1.04=12.96

12.96=-log[OH^-]

[OH^-]=1.09\times 10^{-13}

b) [OH^-]=0.00098M

pOH=-\log [0.00098]=3.01

pH=14-3.01=10.99

10.99=-log[H^+]

[H^+]=1.02\times 10^{-11}

c) pH=10.15

10.15=-\log [H^+]

[H^+]=7.08\times 10^{-11}

pOH=14-10.15=3.85

3.85=-log[OH^-]

[OH^-]=1.41\times 10^{-4}

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