In an aqueous solution, [H₃O⁺] is 1.0 × 10⁻⁶ M. What is [OH⁻]? A) 1.0 × 10⁻⁹ M B) 1.0 × 10⁻⁸ M C) 1.0 × 10⁻⁶ M D) 1.0 × 10⁸ M

Question

Quizplus · Accepted Answer

The given equation is:
HSB(O)OP+ H2O ⇋ OH- + H3O+ + S(O)OP 
Ka = [H3O+][S(O)OP]/ [HSB(O)OP] 
Given [HSB(O)OP] = 1.0 × 10^-6 M
Therefore, Ka = [H3O+][S(O)OP]/ (1.0 × 10^-6 M) 
Let [OH-] = x 
[S(O)OP] = (1.0 × 10^-6 - x) M 
Ka = 1.2 × 10^-2 
Now,  Ka = [H3O+][S(O)OP]/ (1.0 × 10^-6 M) 
1.2 × 10^-2 = [H3O+](1.0 × 10^-6 - x)/ (1.0 × 10^-6 M) 
Solving for x, we get 
x = 1.0 × 10^-8 M 
Therefore, [OH-] = 1.0 × 10^-8 M or 1.0 × 10^-8 M

In an Aqueous Solution, [H3O+] Is 1

In an Aqueous Solution, [H₃O⁺] Is 1