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Chapter 15: Problem 58

Which of the following mixtures would result in a buffered solution when 1.0 \(\mathrm{L}\) of each of the two solutions are mixed? $$ \begin{array}{l}{\text { a. } 0.2 M \mathrm{HNO}_{3} \text { and } 0.4 \mathrm{M} \mathrm{NaNO}_{3}} \\ {\text { b. } 0.2 \mathrm{M} \mathrm{HNO}_{3} \text { and } 0.4 \mathrm{M} \mathrm{HF}}\end{array} $$ $$ \begin{array}{l}{\text { c. } 0.2 M \mathrm{HNO}_{3} \text { and } 0.4 \mathrm{M} \mathrm{NaF}} \\ {\text { d. } 0.2 \mathrm{M} \mathrm{HNO}_{3} \text { and } 0.4 \mathrm{M} \mathrm{NaOH}}\end{array} $$

Short Answer

Expert verified
The buffered solution is obtained when mixing 1.0 L of mixture b (0.2 M HNO$_{3}$ and 0.4 M HF) and 1.0 L of mixture c (0.2 M HNO$_{3}$ and 0.4 M NaF) as it combines a weak acid (HF) and its conjugate base (F-).

Step by step solution

01

Identify the strong acids and bases

In the given mixtures, some strong acids and bases, like HNO3 and NaOH, can be identified, which won't be part of a buffer system.
02

Identify weak acids and their conjugate bases

In the given mixtures, we can identify weak acids like HF (Hydrofluoric acid) along with their conjugate base like NaF (Sodium Fluoride). The conjugate base of HF is F- (Fluoride ion) and can be found in NaF.
03

Match the suitable weak acid and its conjugate base pair

Since mixture b has the weak acid HF and mixture c has its conjugate base NaF when these two solutions are mixed (1.0 L each), it will result in a buffered solution as the mixed solution will contain the weak acid and its conjugate base pair (HF and F-). So the combination of mixture b and mixture c will result in a buffered solution when mixed in equal volumes.

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Most popular questions from this chapter

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 \(\mathrm{HSO}_{3}\) .

Th pH of blood is steady at a value of approximately 7.4 as a result of the following equilibrium reactions: $$ \mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \leftrightharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \leftrightharpoons \mathrm{HCO}_{3}-(a q)+\mathrm{H}^{+}(a q) $$ The actual buffer system in blood is made up of $\mathrm{H}_{2} \mathrm{CO}_{3}\( and \)\mathrm{HCO}_{3}$ - One way the body keeps the pH of blood at 7.4 is by regulating breathing. Under what blood ph conditions will the body increase breathing and under what blood pH conditions will the body decrease breathing? Explain.

You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain

Malonic acid $\left(\mathrm{HO}_{2} \mathrm{CCH}_{2} \mathrm{CO}_{2} \mathrm{H}\right)$ is a diprotic acid. In the titration of malonic acid with NaOH, stoichiometric points occur at \(\mathrm{pH}=3.9\) and $8.8 . \mathrm{A} 25.00-\mathrm{mL}$ sample of malonic acid of unknown concentration is titrated with 0.0984 \(\mathrm{M}\) NaOH, requiring 31.50 \(\mathrm{mL}\) of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution.

What concentration of \(\mathrm{NH}_{4} \mathrm{Cl}\) is necessary to buffer a \(0.52-M\) \(\mathrm{NH}_{3}\) solution at $\mathrm{pH}=9.00 ?\left(K_{\mathrm{b}} \text { for } \mathrm{NH}_{3}=1.8 \times 10^{-5} .\right)$
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