Question

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

Answer #1

A)

we have below equation to be used:

pH = -log [H3O+]

= -log (3*10^-4)

= 3.5

B)

we have below equation to be used:

pH = -log [H3O+]

= -log (2*10^-9)

= 8.7

C)

we have below equation to be used:

pOH = -log [OH-]

= -log (4*10^-5)

= 4.4

we have below equation to be used:

PH = 14 - pOH

= 14 - 4.4

= 9.6

D)

we have below equation to be used:

pOH = -log [OH-]

= -log (4.5*10^-11)

= 10.3

we have below equation to be used:

PH = 14 - pOH

= 14 - 10.3

= 3.7

E)

we have below equation to be used:

pH = -log [H3O+]

= -log (5.1*10^-8)

= 7.3

F)

we have below equation to be used:

pOH = -log [OH-]

= -log (8*10^-4)

= 3.1

we have below equation to be used:

PH = 14 - pOH

= 14 - 3.1

= 10.9

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 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 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

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...

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...

calculate the {H3O+} and {OH-} for a solution with the
following pH values:
{H3O},{OH-} =
(separate by a comma on each)
1. pH= 10.3 (one significant figured)
2. pH=6.0 (one Sig fig)
3. pH= 7.35 (two sig fig)
4. pH=6.1 (one Sig fig)
5. pH= 1.24 (two sig fig)

Calculate the [H3O+] and [OH−] for a solution with the following pH
values: pH=10.6 Express your answers using one significant figure
separated by a comma. pH=4.9 Express your answers using one
significant figure separated by a comma. pH=7.10 pH=6.7 pH=1.72

calculate the {H3O+} and {OH-} for a solution with the
following oH values:
{H3O},{OH-} =
(separate by a comma on each)
1. pH= 10.3 (one significant figured)
2. pH=6.0 (one Sig fig)
3. pH= 7.35 (two sig fig)
4. pH=6.1 (one Sig fig)
5. pH= 1.24 (two sig fig)

What are the [H3O+] and [OH−] for a solution with each of the
following pH values?
Express your answers using one significant figure separated by a
comma.
a)pH = 3.2
b)pH = 6.4
c)pH = 8.76
d)pH = 12.00

For each strong base solution, determine [H3O+], [OH−], pH, and
pOH.
E) 1.7×10−4 M KOH for [OH-0, [H3O+]
F) 1.7×10−4 M KOH for pH, pOH
G) 5.1×10−4 M Ca(OH)2
H) 5.1×10−4 M Ca(OH)2

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