Question

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

Please Answer all parts separately Will be very helpful !!!

Part A

0.20 M HCl

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

[H3O+], [OH−] = ________________ M

Part B

Express your answer to two decimal places.

pH= _______________

Part C

1.6×10⁻² M HNO3

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

[H3O+], [OH−] = ______________ M

Part D

Express your answer to two decimal places.

pH= ______________

Part E

a solution that is 7.1×10⁻² M in HBr and 1.8×10⁻² M in HNO3

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

[H3O+], [OH−] = _____________ M

Part F

Express your answer to two decimal places.

pH= ________________

Part G

a solution that is 0.695 % 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−] = ___________________ M

Part H

Express your answer to three decimal places.

pH= ________________

Answer 1

A)

HCl dissociates completely to give,

[H3O+] = [H+] = 0.20 M

use:

[OH-] = Kw/[H+]

Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC

[OH-] = (1.0*10^-14)/[H+]

[OH-] = (1.0*10^-14)/(0.2)

[OH-] = 5*10^-14 M

Answer: 0.20, 5.0*10^-14 M

B)

use:

pH = -log [H+]

= -log (0.2)

= 0.699

Answer: 0.70

C)

HNO3 dissociates completely to give

[H3O+] = [H+] = [HNO3] = 1.6*10^-2 M

use:

[OH-] = Kw/[H+]

Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC

[OH-] = (1.0*10^-14)/[H+]

[OH-] = (1.0*10^-14)/(1.6*10^-2)

[OH-] = 6.25*10^-13 M

Answer: 1.6*10^-2, 6.2*10^-13 M

D)

use:

pH = -log [H+]

= -log (1.6*10^-2)

= 1.7959

Answer: 1.80

Only 4 parts at a time