Answered: Consider that titration of 30.0 ml of…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

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Question

Consider that titration of 30.0 ml of 0.265m weak base B (Kb = 1.3×10^-10) with 0.150M HI. a) What would be the pH of the solution after the addition of 20.0 mL of HI b) How many mL of HI would be required to reach the halfway point

Expert Solution

Step 1

Given:

Volume of the weak base = 30.0 mL

Concentration of the base = 0.265 M

Concentration of HI = 0.150 M

K_b = 1.3 $\times$ 10^-10

Therefore, calculating pK_b as:

$\begin{array}{rcl} p K_{b} & = & - \log_{10} K_{b} \\ = & - \log_{10} (1.3 \times 10^{- 10}) \\ = & 9.886 \end{array}$

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