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Chapter 15: Problem 22

Which of the following can be classified as buffer solutions? $$ \begin{array}{l}{\text { a. } 0.25 M \mathrm{HBr}+0.25 \mathrm{M} \mathrm{HOBr}} \\ {\text { b. } 0.15 \mathrm{M} \mathrm{HClO}_{4}+0.20 \mathrm{M} \mathrm{RbOH}} \\ {\text { c. } 0.50 \mathrm{M} \mathrm{HOCl}+0.35 \mathrm{MKOCl}}\end{array} $$ $$ \begin{array}{l}{\text { d. } 0.70 M \mathrm{KOH}+0.70 \mathrm{M} \text { HONH_ }} \\ {\text { e. } 0.85 \mathrm{M} \mathrm{H}_{2} \mathrm{NNH}_{2}+0.60 M \mathrm{H}_{2} \mathrm{NNH}_{3} \mathrm{NO}_{3}}\end{array} $$

Short Answer

Expert verified
The buffer solutions are: c. \(0.50 M HOCl + 0.35 M KOCl\) e. \(0.85 M H_2NNH_2 + 0.60 M H_2NNH_3NO_3\)

Step by step solution

01

Identify weak acids/bases and their conjugate pairs in each solution

We need to identify which components are weak acids, weak bases, and their respective conjugate pairs in each solution: a. HBr (strong acid) and HOBr (weak acid) b. HClO₄ (strong acid) and RbOH (strong base) c. HOCl (weak acid) and KOCl (conjugate base of HOCl) d. KOH (strong base) and HONH₂ (weak base) e. H₂NNH₂ (weak base) and H₂NNH₃NO₃ (conjugate acid of H₂NNH₂)
02

Determine if the solutions contain a weak acid/base and their conjugate pairs

A buffer solution must contain a weak acid and its conjugate base, or a weak base and its conjugate acid. We will analyze each solution to see if they meet this criterion: a. This solution contains a strong acid and a weak acid; therefore, it is not a buffer solution. b. This solution contains a strong acid and a strong base; therefore, it is not a buffer solution. c. This solution contains a weak acid and its conjugate base; therefore, it is a buffer solution. d. This solution contains a strong base and a weak base; therefore, it is not a buffer solution. e. This solution contains a weak base and its conjugate acid; therefore, it is a buffer solution.
03

Determine which solutions are buffer solutions

Based on our analysis, we can conclude that the following solutions are buffer solutions: c. 0.50 M HOCl + 0.35 M KOCl e. 0.85 M H₂NNH₂ + 0.60 M H₂NNH₃NO₃

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Most popular questions from this chapter

Consider the titration of 100.0 \(\mathrm{mL}\) of 0.200 $\mathrm{M} \mathrm{HONH}_{2}$ by 0.100 $\mathrm{M} \mathrm{HCl} .\left(K_{\mathrm{b}} \text { for } \mathrm{HONH}_{2}=1.1 \times 10^{-8} .\right)$ a. Calculate the \(\mathrm{pH}\) after 0.0 \(\mathrm{mL}\) of \(\mathrm{HCl}\) has been added. b. Calculate the \(\mathrm{pH}\) after 25.0 \(\mathrm{mL}\) of \(\mathrm{HCl}\) has been added. c. Calculate the \(\mathrm{pH}\) after 70.0 \(\mathrm{mL}\) of HCl has been added. d. Calculate the \(\mathrm{pH}\) at the equivalence point. e. Calculate the pH after 300.0 \(\mathrm{mL}\) of HCl has been added. f. At what volume of HCl added does the pH = 6.04?

Sketch the titration curves for a diprotic acid titrated by a strong base and a triprotic acid titrated by a strong base. List the major species present at various points in each curve. In each curve, label the halfway points to equivalence. How do you calculate the pH at these halfway points?

Some \(\mathrm{K}_{2} \mathrm{SO}_{3}\) and \(\mathrm{KHSO}_{3}\) are dissolved in 250.0 \(\mathrm{mL}\) of solution and the resulting \(\mathrm{pH}\) is \(7.25 .\) Which is greater in this buffer solution, the concentration of \(\mathrm{SO}_{3}^{2-}\) or the concentration of \(\mathrm{HSO}_{3}-7\) If \(\left[\mathrm{SO}_{3}^{2-}\right]=1.0 \mathrm{M}\) in this solution, calculate the concentration of \(\mathrm{HSO}_{3}\) .

Calculate the pH of a solution that is 0.60\(M\) HF and 1.00\(M \mathrm{KF}\)

A 0.210 -g sample of an acid (molar mass \(=192 \mathrm{g} / \mathrm{mol}\) ) is titrated with 30.5 \(\mathrm{mL}\) of 0.108\(M \mathrm{NaOH}\) to a phenolphthalein end point. Is the acid monoprotic, diprotic, or triprotic?
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