A solution has [OH−]
[
O
H
−
]
= 2.1×10−2 M
M
. Use the ion product constant of water
Kw=[H3O+][OH−]
K
w
=
[
H
3
O
+
]
[
O
H
−
]
to find the [H3O+]
[
H
3
O
+
]
of the solution.
We know that:
Kw = [H3O+][OH−]
Plugging in the given value for [OH−]:
Kw = [H3O+](2.1×10−2 M)
Rearranging the equation to solve for [H3O+]:
[H3O+] = Kw/[OH−]
[H3O+] = (1.0×10−14)/(2.1×10−2 M)
[H3O+] = 4.76×10−13 M
Therefore, the [H3O+] of the solution is 4.76×10−13 M.
A 125 mL
m
L
bubble of hot gases at 213 ∘C
∘
C
and 1.87 atm
a
t
m
is emitted from an active volcano.
Part A
What is the final temperature, in degrees Celsius, of the gas in the bubble outside the volcano if the final volume of the bubble is 136 mL
m
L
and the pressure is 0.800 atm
a
t
m
and if the amount of gas does not change?
A sample of argon gas has a volume of 735 mL
m
L
at a pressure of 1.20 atm
a
t
m
and a temperature of 112 ∘C
∘
C
. What is the final volume of the gas, in milliliters, when the pressure and temperature of the gas sample are changed to the following, if the amount of gas does not change?
664mmHg and 274 K
To find the [H3O+] concentration of the solution, we can use the ion product constant of water (Kw). The ion product constant of water is defined as Kw = [H3O+][OH-].
Given that [OH-] = 2.1 × 10^-2 M, we can rearrange the equation to solve for [H3O+].
Kw = [H3O+][OH-]
Substituting the known value for Kw (which is dependent on temperature) and the given value for [OH-], we get:
Kw = [H3O+](2.1 × 10^-2 M)
Now, divide both sides of the equation by the known value of [OH-]:
Kw /[OH-] = [H3O+]
Substituting the known value for Kw (at the given temperature) and [OH-], we can calculate [H3O+].