Mulitple choice
What is the concentration of H^+ in solution given the [OH^-]= 1.32x10^-4
a)7.58x10^-11M
b)1.32x10^-11M
C)1.0x10^14M
d)not enough information
E)none of the above
so is it c? how did u get that please show me how?
As we are not given Kw in the question, my answer would have d)
To determine the concentration of H+ in solution given the concentration of OH-, you can use the concept of the autoionization of water. In pure water at 25 degrees Celsius, the concentration of H+ ions (also known as the hydronium ion) is equal to the concentration of OH- ions.
The autoionization of water can be represented by the following equation:
H2O ⇌ H+ + OH-
Given that [OH-] is 1.32x10^-4, we can assume that the solution is not neutral but basic because [OH-] is greater than the concentration of H+ in pure water (which is 1x10^-7).
Since the concentration of H+ ([H+]) must be equal to the concentration of OH- ([OH-]) in a neutral solution, we can determine that the concentration of H+ is also 1.32x10^-4 (based on the given information).
The correct answer is:
E) none of the above (1.32x10^-4 M)
(H^+)(OH^-) = Kw = 1E-14
I honestly hope you're kidding.
The equation I wrote will work ALL problems with one of the two given and you want to calculate the other.
(H^+)(OH^-) = 1E-14
(1.32E-4)(OH^-) = 1E-14
(OH^-) = 1E-14/1.32E-4.
Just punch in the numbers on your calculator and turn the crank. Out comes the answer. It is not c.