Consider the following reaction. HSO4 – (aq) + H2O (l) H3O+ (aq) + SO4 2–(aq) Ka = 0.012 If the initial concentrations are [HSO4–] = 0.50 M, [H3O+] = 0.020 M, and [SO4 2–] = 0.060 M, what are the equilibrium concentrations of the products and reactants?
Consider the following reaction. HSO4 – (aq) + H2O (l) H3O+ (aq) + SO4 2–(aq) Ka = 0.012 If the initial concentrations are [HSO4–] = 0.50 M, [H3O+] = 0.020 M, and [SO4 2–] = 0.060 M, what are the equilibrium concentrations of the products and reactants?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.52QE: Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium...
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Consider the following reaction.
HSO4 – (aq) + H2O (l) H3O+ (aq) + SO4 2–(aq)
Ka = 0.012
If the initial concentrations are [HSO4–] = 0.50 M, [H3O+] = 0.020 M, and [SO4 2–] = 0.060 M, what are the equilibrium concentrations of the products and reactants?
Expert Solution
Step 1
Given : Ka = 0.012
initial concentrations are [HSO4–] = 0.50 M, [H3O+] = 0.020 M, and [SO4 2–] = 0.060 M
Products are : H3O+ (aq) + SO4^2– (aq)
Reactants are : HSO4^– (aq) + H2O (l)
so, Concentration of H2O is always fixed , so no need to find concentration of water at equilibrium as it will be
1M always.
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