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Chapter 15: Problem 52

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

Short Answer

Expert verified
None of these mixtures form a buffered solution.

Step by step solution

01

Option a: Mixing 0.2 M HNO3 and 0.4 M NaNO3

HNO3 is a strong acid, and its conjugate base is NO3-. NaNO3 is a salt containing the NO3- ion. In this case, we do not have a weak acid/weak base and its conjugate present in the mixture. Therefore, it cannot form a buffered solution. Option a is incorrect.
02

Option b: Mixing 0.2 M HNO3 and 0.4 M HF

In this case, we have a strong acid (HNO3) mixed with a weak acid (HF). The conjugate base of HF is F-. There is no conjugate base present in the mixture, and therefore, it cannot form a buffered solution. Option b is incorrect.
03

Option c: Mixing 0.2 M HNO3 and 0.4 M NaF

In this case, we have a strong acid (HNO3) mixed with a salt (NaF) that contains the conjugate base (F-) of a weak acid (HF). Even though we have a weak acid and its conjugate base, they are not in the same mixture. The HNO3 will not form a buffer with F-. Option c is incorrect.
04

Option d: Mixing 0.2 M HNO3 and 0.4 M NaOH

In this case, we have a strong acid (HNO3) mixed with a strong base (NaOH). Neither of them have weak conjugate partners, and therefore, this mixture cannot form a buffered solution. Option d is incorrect. After evaluating all options, we can conclude that none of these mixtures form a buffered solution.

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Most popular questions from this chapter

A best buffer has about equal quantities of weak acid and conjugate base present as well as having a large concentration of each species present. Explain.

When a diprotic acid, \(\mathrm{H}_{2} \mathrm{~A}\), is titrated with \(\mathrm{NaOH}\), the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at \(100.0 \mathrm{~mL} \mathrm{NaOH}\) added, what volume of \(\mathrm{NaOH}\) added corresponds to the second equivalence point? b. For the following volumes of \(\mathrm{NaOH}\) added, list the major species present after the \(\mathrm{OH}^{-}\) reacts completely. i. \(0 \mathrm{~mL}\) NaOH added ii. between 0 and \(100.0 \mathrm{~mL}\) NaOH added iii. \(100.0 \mathrm{~mL} \mathrm{NaOH}\) added iv. between \(100.0\) and \(200.0 \mathrm{~mL} \mathrm{NaOH}\) added v. \(200.0 \mathrm{~mL} \mathrm{NaOH}\) added vi. after \(200.0 \mathrm{~mL} \mathrm{NaOH}\) added c. If the \(\mathrm{pH}\) at \(50.0 \mathrm{~mL} \mathrm{NaOH}\) added is \(4.0\) and the \(\mathrm{pH}\) at \(150.0 \mathrm{~mL} \mathrm{NaOH}\) added is \(8.0\), determine the values \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) for the diprotic acid.

Potassium hydrogen phthalate, known as KHP (molar mass = \(204.22 \mathrm{~g} / \mathrm{mol}\) ), can be obtained in high purity and is used to determine the concentration of solutions of strong bases by the reaction $$\mathrm{HP}^{-}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{P}^{2-}(a q)$$ If a typical titration experiment begins with approximately \(0.5 \mathrm{~g}\) KHP and has a final volume of about \(100 \mathrm{~mL}\), what is an appropriate indicator to use? The \(\mathrm{p} K_{\mathrm{a}}\) for \(\mathrm{HP}^{-}\) is \(5.51\).

Calculate the volume of \(1.50 \times 10^{-2} M \mathrm{NaOH}\) that must be added to \(500.0 \mathrm{~mL}\) of \(0.200 M \mathrm{HCl}\) to give a solution that has \(\mathrm{pH}=2.15\)

Calculate the \(\mathrm{pH}\) of each of the following solutions. a. \(0.100 M\) propanoic acid \(\left(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}, K_{\mathrm{a}}=1.3 \times 10^{-5}\right)\) b. \(0.100 M\) sodium propanoate \(\left(\mathrm{NaC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}\right)\) c. pure \(\mathrm{H}_{2} \mathrm{O}\) d. a mixture containing \(0.100 \mathrm{M} \mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}\) and \(0.100 \mathrm{M}\) \(\mathrm{NaC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}\)
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