Question

Calculate the concentration of hydronium and hydroxide ions in a 0.050 M solution of nitric acid.

Answer 1

The concentration of hydronium ions (H3O+) and hydroxide ions (OH-) in a 0.050 M solution of nitric acid is 0.050 M and 2.0 × 10^-13 M, respectively.

Step-by-step explanation:

The concentration of hydronium ions (H3O+) and hydroxide ions (OH-) in a solution can be determined using the equation for water dissociation:

Kw = [H3O+][OH-]

For a strong acid like nitric acid (HNO3), it completely dissociates in water, so the concentration of hydronium ions is equal to the initial concentration of the acid:

[H3O+] = 0.050 M

Since the concentration of hydronium ions and hydroxide ions in a neutral solution is equal (Kw = 1.0 × 10^-14), the concentration of hydroxide ions can be calculated

[OH-] = Kw / [H3O+]

[OH-] = (1.0 × 10^-14) / (0.050) = 2.0 × 10^-13 M

Therefore, in a 0.050 M solution of nitric acid, the concentration of hydronium ions is 0.050 M and the concentration of hydroxide ions is 2.0 × 10^-13 M.

Answer 2

Make an ICE box,
HNO3 + H2O --> H3O+ + NO3-
I. 0.05M. 0M. 0M
C. -x. +x. +x.
E. 0.05M-x. x. x.

You would need k to them find x using the following equation:

k = [H3O+][NO3-]/[HNO3]