Question

Complete the following table.
(The first row is completed for you.)

[H3O+]	[OH−]	pOH	pH	Acidic or Basic
1.0×10−8	1.0×10−6	6.00	8.00	basic
_____	_____	_____	3.65	_____
2.7×10−9	_____	_____	_____	_____
_____	_____	_____	13.39	_____
_____	7.6×10−11	_____	_____	_____

Part A

Complete the first column of the table.

Express your answers using two significant figures. Enter your answers in order given in the table separated by commas.

[H3O+] =	nothing	M

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Part B

Complete the second column of the table.

Express your answers using two significant figures. Enter your answers in order given in the table separated by commas.

[OH−] =	nothing	M

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Part C

Complete the third column of the table.

Express your answers using two decimal places. Enter your answers in order given in the table separated by commas.

pOH =	nothing

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Part D

Complete the fourth column of the table.

Express your answers using two decimal places. Enter your answers in order given in the table separated by a comma.

pH =	nothing

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Part E

Complete the fifth column of the table.

Enter your answers as words acidic or basic. Enter your answers in order given in the table separated by commas.

Answer 1

for row 2:

POH = 14 - pH

= 14 - 3.65

= 10.35

use:

pH = -log [H+]

3.65 = -log [H+]

[H+] = 2.239*10^-4 M

use:

pOH = -log [OH-]

10.35 = -log [OH-]

[OH-] = 4.467*10^-11 M

Since pH < pOH, this is acidic in nature

Row 2:

[H+] = 2.239*10^-4

[OH-] = 4.467*10^-11

pH = 3.65

pOH = 10.35

acidic

2) for row 3:

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)/(2.7*10^-9)

[OH-] = 3.704*10^-6 M

use:

pH = -log [H+]

= -log (2.7*10^-9)

= 8.5686

use:

pOH = -log [OH-]

= -log (3.704*10^-6)

= 5.4314

Since pH > pOH, this is basic in nature

row 3:

[H+] = 2.7*10^-9

[OH-] = 3.704*10^-6

pH = 8.5686

pOH = 5.4314

basic

3) for row 4:

POH = 14 - pH

= 14 - 13.39

= 0.61

use:

pH = -log [H+]

13.39 = -log [H+]

[H+] = 4.074*10^-14 M

use:

pOH = -log [OH-]

0.61 = -log [OH-]

[OH-] = 0.2455 M

Since pH > pOH, this is basic in nature

row 4:

[H+] = 4.074*10^-14

[OH-] = 0.2455

pH = 13.39

pOH = 0.61

basic

4) for row 5:

use:

[H+] = Kw/[OH-]

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

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

[H+] = (1.0*10^-14)/7.6*10^-11

[H+] = 1.316*10^-4 M

use:

pH = -log [H+]

= -log (1.316*10^-4)

= 3.8808

use:

pOH = -log [OH-]

= -log (7.6*10^-11)

= 10.1192

Since pH < pOH, this is acidic in nature

row 5:

[H+] = 1.316*10^-4

[OH-] = 7.6*10^-11

pH = 3.8808

pOH = 10.1192

acidic

a)

2.2*10^-4, 2.7*10^-9, 4.1*10^-14, 1.3*10^-4

b)

4.5*10^-11, 3.7*10^-6, 2.5*10^-1, 7.6*10^-11

c)

10.35, 5.43, 0.61, 10.12

d)

3.65, 8.57, 13.39, 3.88

e)

acidic, basic, basic, acidic