Question

Calculate the pH of each solution given the following - Express your answer using one decimal point:

**Part A**

[H3O+] = 7×10^{−4} M

**Part B**

[H3O+] = 7×10^{−9} M

**Part C**

[OH−] = 1×10^{−4} M

**Part D**

[OH−] = 5.0×10^{−11} M

**Part E**

[H3O+] = 5.1×10^{−8} M

**Part F**

[OH−] = 8.3×10^{−4} M

Answer #1

A)

use:

pH = -log [H3O+]

= -log (7*10^-4)

= 3.1549

Answer: 3.2

B)

use:

pH = -log [H3O+]

= -log (7*10^-9)

= 8.1549

Answer: 8.2

C)

use:

pOH = -log [OH-]

= -log (1*10^-4)

= 4

use:

PH = 14 - pOH

= 14 - 4

= 10

Answer: 10.0

D)

use:

pOH = -log [OH-]

= -log (5*10^-11)

= 10.301

use:

PH = 14 - pOH

= 14 - 10.301

= 3.699

Answer: 3.7

E)

use:

pH = -log [H3O+]

= -log (5.1*10^-8)

= 7.2924

Answer: 7.3

F)

use:

pOH = -log [OH-]

= -log (8.3*10^-4)

= 3.0809

use:

PH = 14 - pOH

= 14 - 3.0809

= 10.9191

Answer: 10.9

Calculate the pH of each solution given the following [H3O+] or
[OH−] values.
Part A: [H3O+] = 3×10−4 M
Express your answer using one decimal place.
Part B: [H3O+] = 2×10−9 M
Part C: [OH−] = 4×10−5 M
Part D: [OH−] = 4.5×10−11 M
Part E: [H3O+] = 5.1×10−8 M
Part F: [OH−] = 8.0×10−4 M

Calculate the pH of each solution given the following [H3O+] or
[OH−] values.
a.) [H3O+] = 5.0×10−4 M
Express your answer using two decimal places.
b.) [H3O+] = 6.0×10−9 M
Express your answer using two decimal places.
c.) [OH−] = 4.0×10−5 M
Express your answer using two decimal places.
d.) [OH−] = 1.5×10−11 M
Express your answer using two decimal places.
e.) [H3O+] = 6.8×10−8 M
Express your answer using two decimal places.
f.) [OH−] = 7.8×10−4 M
Express your...

Calculate the pH of each solution.
Part A
[OH−] = 6.8×10−11 M
Express your answer using two decimal places.
Part B
[OH−] = 3.6×10−3 M
Express your answer using two decimal places.
Part C
[OH−] = 8.8×10−12 M
Express your answer using two decimal places.
Part D
[OH−] = 9.4×10−4 M
Express your answer using two decimal places.

Calculate the [H3O+] and [OH-]
for a solution with each of the following pH values.
Express your answer to one significant figure and include
the appropriate units:
1.) What is the [H3O+] for a solution with
pH = 10.60?
[H3O+] =
2.) What is the [OH-] for the solution above?
[OH-] =
3.) What is the [H3O+] for a solution with
pH = 5.3?
[H3O+] =
4.) What is the [OH-] for the solution above?
[OH-] =
5.) What is...

Calculate the [OH−] of each aqueous solution with the following
[H3O+].
Express your answer using two significant figures.
Part 1: soap, 1.2×10−8 M
OH{-} = ?
Part 2: cleanser, 5.2×10−10 M
OH{-} = ?
Part 3: lemon juice, 2.6×10−2 M
OH{-} = ?
Problem 10.33

Calculate the [H3O+] of the following polyprotic acid solution:
0.400 M H3PO4. Express your answer using two significant figures.
[H3O+] = .
Part B Calculate the pH of this solution. Express your answer
using one decimal place. pH =
Part C Calculate the [H3O+] and pH of the following polyprotic
acid solution: 0.370 M H2C2O4. Express your answer using two
significant figures. [H3O+] =
Part D Calculate the pH of this solution. Express your answer
using two decimal places.

Calculate the ph of each solution given the following (H3O.+) or
(OH-) values
Part A- (H3O+ ) = 2.5 x10-8 M
Use TWO decimal places
Ph=_______
Part B- (H3O+) = 6.0 x 10-6M
Use TWO decimal places
Part C- (OH-) = 4.0 x 10-2 M
Use TWO decimal places
Part D - (OH-) = 7.5 x 10-3 M
Use TWO decimal places

Calculate the pH in 0.23 M HCO2H (Ka=1.8×10−4).
Express your answer using two decimal places.
pH =
2.20
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Correct
Part B
Calculate the concentrations of all species present (HCO2H,
HCO−2, H3O+, and OH−) in 0.23M HCO2H .
Express your answers using two significant figures. Enter your
answers numerically separated by commas.
[HCO2H], [HCO−2], [H3O+],[OH−] =
M
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Part C
Also calculate the percent dissociation.
Express your answer using two significant figures.

Complete the following table:
H3O+
OH−
pH
Acidic, Basic, or Neutral?
10.0
Neutral
4×10−5M
1 ×10−2M
12.2
Part A
If the pH of the solution is 10.0, what is the [H3O+]?
Express your answer to one significant figure.
[H3O+] =
M
Part B
If the pH of the solution is 10.0, what is the [OH−]?
Express your answer to one significant figure.
[OH−] =
M
Part C
If the solution is neutral, what is the [H3O+]?
Express your answer to...

Part B
Calculate the pH of a 0.10 M solution of barium
hydroxide, Ba(OH)2.
Express your answer numerically using two decimal places.
ph=
Part C
Calculate the pH of a 0.10 M solution of NaOH.
Express your answer numerically using two decimal places.
ph=
Part D
Calculate the pH of a 0.10 M solution of hydrazine,
N2H4. Kb for hydrazine is 1.3×10−6.
Express your answer numerically using two decimal places.
ph=
Part E
Calculate the pH of a 0.10 M...

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