Calculate the concentration of H₃O⁺ in a solution that contains 5.5 × 10^-5 mol L^-1 OH^- at 25 °C.Also identify the solution as acidic,basic,or neutral. A)1.8 × 10^-10 mol L^-1,basic B)1.8 × 10^-10 mol L^-1,acidic C)5.5 × 10^-10 mol L^-1,neutral D)9.2 × 10^-1 mol L^-1,acidic E)9.2 × 10^-1 mol L^-1,basic

Question

Quizplus · Accepted Answer

To calculate the concentration of HS1U1B13S1U1B0OS1U1P1+S1S1P0, we need to use the equilibrium constant expression:
Kb = [HS1U1B13S1U1B0O][S1U1P1+S1S1P0]/[HS1U1B13S1U1B0OS1U1P1]
At 25°C, the Kb value for HS1U1B13S1U1B0O is 1.3 × 10S1U1P1-12S1S1P0.
We are given the concentration of OHS1U1P1-S1S1P0 as 5.5 × 10S1U1P1-5S1S1P0 mol LS1U1P1-1S1S1P0.
Let x be the concentration of HS1U1B13S1U1B0O that reacts with OH-S1U1P1-S1S1P0 to form HS1U1B13S1U1B0OS1U1P1- and S1S1P0:
Kb = (x)(x)/[HS1U1B13S1U1B0O - x]
1.3 × 10S1U1P1-12S1S1P0 = xS1U1P1-2[S1U1B13S1U1B0O - x]
Assuming that x << [HS1U1B13S1U1B0O], we can simplify the equation to:
1.3 × 10S1U1P1-12S1S1P0 = xS1U1P1-2[HS1U1B13S1U1B0O]
x = sqrt(Kb[HS1U1B13S1U1B0O]) = sqrt(1.3 × 10S1U1P1-12S1S1P0 × 5.5 × 10S1U1P1-5S1S1P0) = 1.8 × 10S1U1P1-10S1S1P0 mol LS1U1P1-1S1S1P0
Since the concentration of HS1U1B13S1U1B0OS1U1P1- is equal to x and the concentration of S1U1P1+S1S1P0 is equal to 5.5 × 10S1U1P1-5S1S1P0 mol LS1U1P1-1S1S1P0, the concentration of HS1U1B13S1U1B0O is (5.5 × 10S1U1P1-5S1S1P0 - x) mol LS1U1P1-1S1S1P0.
Since the concentration of OH-S1U1P1-S1S1P0 is greater than the concentration of HS1U1B13S1U1B0OS1U1P1-, the solution is basic. Therefore, the best choice is A.

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