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Exercise 15.55 For each strong acid solutions, determine [H3O+],[OH−], and pH. Part A 0.23 M HCl...

Exercise 15.55

For each strong acid solutions, determine [H3O+],[OH−], and pH.

Part A

0.23 M HCl

Enter your answers numerically separated by a comma. Express your answer using two significant figures.


[H3O+], [OH−] =

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Part B

Express your answer to two decimal places.


pH =

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Part C

2.6×10⁻² M HNO3

Enter your answers numerically separated by a comma. Express your answer using two significant figures.


[H3O+], [OH−] =

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Part D

Express your answer to two decimal places.


pH =

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Part E

a solution that is 5.6×10⁻² M in HBr and 2.3×10⁻² M in HNO3

Enter your answers numerically separated by a comma. Express your answer using two significant figures.


[H3O+], [OH−] =

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Part F

Express your answer to two decimal places.


pH =

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Part G

a solution that is 0.815% HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)

Enter your answers numerically separated by a comma. Express your answer using three significant figures.


[H3O+], [OH−] =

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Part H

Express your answer to three decimal places.


pH =

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Solutions

Expert Solution

Part A

Since HCl is a strong monoprotic acid hence

[H3O^+] = [HCl] = 0.23 M

pH = - log [H3O^+] = - log 0.23 = -( - 0.64) = 0.64

pH = 0.64

pOH = 14.00 - pH = 14.00 - 0.64 = 13.36

We know [OH^-] = 10^-pOH = 10^-13.36 M = 0.0004365 M = 4.365 * 10^-4 M

Part C :-

Similarly [H3O^+] = [HNO3] = 2.6 * 10^-2 M

pH = - log(2.6 * 10^-2) = - log 2.6 + 2 log 10 = -0.41 + 2 * 1 = 1.59

pOH = 14.00 - 1.59 = 12.41

[OH^-] = 10^-pOH = 10^-12.41 = 3.89 * 10^-13 M

Part E

Since HBr and HNO3 are strong monoprotic acid hence

[H3O^+] = (5.6 * 10^-2 + 2.3 * 10^-2) M = 7.9 * 10^-2 M

pH = - log(7.9 * 10^-2) M = - log 7.9 + 2 log 10 = - 0.898 + 2 * 1 = 1.10

pH = 1.10

pOH = 14.00 - 1.10 = 12.90

[OH^-] = 10^-12.90 M = 1.26 * 10^-13 M

queen_honey_blossom answered 1 year ago

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