6) Find the pH of the following solutions:

a) 0.00010 M HClO4

b) 2.35 x 10-3 M HI

c) 4.678 x 10-5 M HNO3

d) 0.0000877 M HCl

e) 0.00020 M HF

f) 0.0000061 M H3O+

g) 4.3 x 10-3 M NaOH (This is a base! Remember you will be finding pOH first!)

h) 6.7 x 10-9 M KOH (This is a base! Remember you will be finding pOH first!)

i) 0.00044 M HCl

j) C

Question

Emery Franklin

Chemistry

11 October, 11:22

6) Find the pH of the following solutions:

a) 0.00010 M HClO4

b) 2.35 x 10-3 M HI

c) 4.678 x 10-5 M HNO3

d) 0.0000877 M HCl

e) 0.00020 M HF

f) 0.0000061 M H3O+

g) 4.3 x 10-3 M NaOH (This is a base! Remember you will be finding pOH first!)

h) 6.7 x 10-9 M KOH (This is a base! Remember you will be finding pOH first!)

i) 0.00044 M HCl

j) C

+4

Answers (2)

Know the Answer?

Jaylen Mccullough · Answer 1

pH is the negative logarithm of hydrogen (oxonium) ion concentration of aqueous solutions.

Explanation:

Recall that pH is defined as the negative logarithm of hydrogen ion concentration. We are going to apply that definition here.

a) 0.00010 M HClO4

pH = - log[0.00010]

pH = 4

b) 2.35 x 10-3 M HI

pH = - log[2.35 x 10-3 ]

pH = 2.63

c) 4.678 x 10-5 M HNO3

pH = - log[4.678 x 10-5]

pH = 4.3

d) 0.0000877 M HCl

pH=-log[0.0000877]

pH = 4.1

e) 0.00020 M HF

pH = - log[0.00020]

pH = 3.7

f) 0.0000061 M H3O+

pH = - log[0.0000061]

pH = 5.2

g) 4.3 x 10-3 M NaOH

pOH = - log[OH^-]

pOH = - log[ 4.3 x 10-3 ]

pOH = 2.4

But

pH + pOH = 14

Therefore

pH = 14-pOH

pH = 14 - 2.4

pH = 11.6

h) 6.7*10^-9 M KOH

pOH = - log[OH^-]

pOH = - log[ 6.7 x 10-9 ]

pOH = 8.2

But

pH + pOH = 14

Therefore

pH = 14-pOH

pH = 14 - 8.2

pH=5.8

I) 0.00044M HCl

pH = - log[0.00044]

pH = 3.4

Nathanial Patel · Answer 2

Answer: A. 4 B. 2.6 C. 4.3 D. 4.1 E. 3.7 F. 5.8 G. 11.6 H. 5.8 I. 3.4

Explanation:

A. 0.00010 M HClO4

pH = - log [1.0 x 10^-4]

= 4 - log 1 = 4

B. 2.5 x 10^-3 M HI

pH = - log [2.5 x 10^-3]

= 3 - log 2.5

= 3 - 0.398 = 2.6

C. 4.678 x 10^M HNO3

pH = - log [4.678 x 10^-5]

= 5 - 0.7 = 4.3

D. 0.0000877M HCL

pH = - log [8.77 x 10^-5]

= 5 - 0.943 = 4.057 = 4.1

E. 0.00020M HF

pH = - log [2.0 x10^-4]

= 4 - 0.301 = 3.7

F. 0.0000061M H3O+

pH = - log [ 6.1 x 10^-6]

= 6 - 0.785 = 5.2

G. 4.3 x 10^-3 M NaOH

Finding pOH first, we have

pOH = - log [4.3 x 10-3]

= 3 - 0.633 = 2.4

pH + pOH = 14

pH = 14 - 2.4 = 11.6

H. 6.7 x 10^-9 M KOH

Finding pOH, we have,

pOH = - log [6.7 x 10^-9]

= 9 - 0.826 = 8.17 = 8.2

pH + pOH = 14

pH = 14 - 8.2 = 5.8

I. 0.00044 M HCl

pH = - log [ 4.4 x 10^-4]

= 4 - 0.64 = 3.36 = 3.4