The concentration of hydroxide ions in a solution of nitric acid 0.2 M is:
a. 2 x 10-14 M
b. 5 x 10-14 M
c. 5 x 10-7 M
d. 2 x 10-1 M
IS IT D)?
HNO3. H+ is .2M
concOH=1E-14/.2=you do the math.
I think the answer is B
[H+]=0.2M
find the concentration of [OH-] by dividing 1x10^-14 by 0.2M.
you will get an answer of 5 x 10^-14.
D) 2 x 10-1 M? Well, that would be quite a joker of a concentration! But unfortunately, that's not the right answer. Nitric acid is a strong acid, which means it completely dissociates in water. So in a 0.2 M solution of nitric acid, the concentration of hydroxide ions would be negligible. You can't find what's not there! So the correct answer is actually none of the above. Keep searching, my friend!
No, the concentration of hydroxide ions in a solution of nitric acid (HNO3) is negligible, as nitric acid is a strong acid and completely dissociates into H+ ions and NO3- ions in solution. Therefore, the correct answer would be none of the options provided.
To determine the concentration of hydroxide ions (OH-) in a solution of nitric acid (HNO3), we can use the balanced chemical equation for the dissociation of nitric acid:
HNO3 → H+ + NO3-
Since nitric acid does not contain hydroxide ions, its concentration does not directly contribute to the concentration of hydroxide ions. Therefore, the concentration of hydroxide ions in the solution of nitric acid will be negligible.
The correct answer is a. 2 x 10^-14 M, as this value represents the concentration of hydroxide ions in pure water at 25°C, which is the value for the equilibrium constant of water.
It's important to note that nitric acid is a strong acid, meaning it completely dissociates in water. However, its dissociation only produces hydronium ions (H+), not hydroxide ions (OH-).