Question

Calculate [H3O+] given [OH-] in each aqueous solution.

part A) [OH-] = 3.2x10^-12 M

part B) classify this solution as acidic or basic ^

part C) [OH-] = 3.0x10^-2 M

part D) classify this solution as acidic or basic ^

part E) [OH-] = 1.6x10^-10 M

part F) classify this solution as acidic or basic ^

part G) [OH-] = 1.8x10^-4 M

part H) classify this solution as acidic or basic ^

Sign in MyLab & Mastering <Chapter 14 HW Exercise 14.65 with eText link Calculate (H,0 given (OH- ) in each aqueous solution Part A [OH-] = 32x10 Express your answer using two significant figures. AEO Submit Request Answe Part B Classily this solution as acidic or basic acidic basic Submit Request Answer Part C TOH 3.0x10-2M

Answer 1

A)

Given:

[OH-] = 3.2*10^-12 M

use:

[H3O+] = Kw/[OH-]

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

[H3O+] = (1.0*10^-14)/[OH-]

[H3O+] = (1.0*10^-14)/3.2*10^-12

[H3O+] = 3.125*10^-3 M

Answer: 3.1*10^-3 M

B)

Since [H3O+] > [OH-], solution is acidic

Answer: acidic

C)

Given:

[OH-] = 3.2*10^-2 M

use:

[H3O+] = Kw/[OH-]

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

[H3O+] = (1.0*10^-14)/[OH-]

[H3O+] = (1.0*10^-14)/3.2*10^-2

[H3O+] = 3.125*10^-13 M

Answer: 3.1*10^-13 M

D)

Since [H3O+] < [OH-], solution is basic

Answer: basic

Only 4 parts at a time please