Asked by Meaghan Crowley on Apr 29, 2024
Verified
What is the K of the following reaction: HI ⇌ H+ + I- , if [HI] = 0.15 M and the pH = 1.0?
A) 0.10
B) 0.07
C) 0.06
D) 0.01
HI
A chemical formula representing hydrogen iodide, a diatomic molecule consisting of hydrogen and iodine.
pH
A scale used to specify the acidity or basicity of an aqueous solution, ranging from 0 (acidic) to 14 (basic), with 7 being neutral.
K
The chemical symbol for Potassium, an essential dietary mineral and electrolyte involved in nerve function, muscle contraction, and fluid balance.
- Map out the association between the pH of a solution and the amount of reactants and products present in acid-base equilibria.
- Acquire knowledge of acid-base chemistry principles and use them to determine equilibrium constants and pH values.
Verified Answer
KF
Kelly FoleyMay 01, 2024
Final Answer :
B
Explanation :
The equilibrium constant (K) for the reaction can be calculated using the given concentrations and the pH. The pH of 1.0 implies a [H+] concentration of 10^-1 M. Since HI dissociates into H+ and I-, and the products also involve protons, the concentration of H+ is directly related to the equilibrium. However, without the explicit concentrations of the products, we can't directly calculate K from the given information. The correct answer must be inferred or calculated based on additional information not provided in the question. Given the choices, the selection of 0.07 as the correct answer suggests an assumed calculation or approximation based on the given pH and [HI]. This might involve assumptions about the degree of dissociation of HI and the relationship between the pH and the concentrations of the products at equilibrium.
Learning Objectives
- Map out the association between the pH of a solution and the amount of reactants and products present in acid-base equilibria.
- Acquire knowledge of acid-base chemistry principles and use them to determine equilibrium constants and pH values.