Asked by Alexa Carranza on May 07, 2024
Verified
What is the pH in the following reaction: HI ⇌ H+ + I- , if the [HI] = 0.250 M and K = 1 × 10-6?
A) 3.30
B) 5.00
C) 2.50
D) 0.25
HI
Hydroiodic acid, a diatomic molecule consisting of one hydrogen atom and one iodine atom, known for being a strong acid.
K
The chemical symbol for Potassium, a soft, silvery-white metallic element that is highly reactive with water.
pH
A scale used to specify the acidity or basicity of an aqueous solution, with values ranging from 0 (very acidic) to 14 (very basic).
- Associate the pH value of a solution with the concentrations of reactants and products in the context of acid-base equilibrium.
- Estimate the pH of a solution through the quantification of an acid or base’s concentration and the equilibrium constant.
Verified Answer
ZK
Zybrea KnightMay 09, 2024
Final Answer :
A
Explanation :
The pH of the solution can be calculated using the dissociation constant (K) and the concentration of HI. Given K = 1 × 10^-6 and [HI] = 0.250 M, we can set up the equation for the dissociation of HI into H+ and I- ions. Since K is small, we can assume that the change in concentration of HI due to dissociation is negligible, and thus [H+] ≈ [I-] at equilibrium. Using the formula K = [H+][I-]/[HI], we find that [H+]^2 = K[HI] = (1 × 10^-6)(0.250) = 2.5 × 10^-7. Taking the square root gives [H+] = 1.58 × 10^-4 M. The pH is then calculated using pH = -log[H+], which gives a pH of approximately 3.30.
Learning Objectives
- Associate the pH value of a solution with the concentrations of reactants and products in the context of acid-base equilibrium.
- Estimate the pH of a solution through the quantification of an acid or base’s concentration and the equilibrium constant.