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Chapter 17: Problem 44

Explain whether the equivalence point of each of the following titrations should be below, above, or at pH 7: (a) \(\mathrm{NaHCO}_{3}(\text { aq) titrated with } \mathrm{NaOH}(\mathrm{aq}) ; \text { (b) } \mathrm{HCl}(\mathrm{aq})\) titrated with \(\mathrm{NH}_{3}(\mathrm{aq}) ;\) (c) KOH(aq) titrated with HI(aq).

Short Answer

Expert verified
(a) Above 7, (b) Below 7, (c) At 7

Step by step solution

01

Identify the Acid-Base Pairs

Look at each pair and evaluate if they are strong or weak acids or bases. For (a) NaHCO3 (a weak base) is being titrated with NaOH (a strong base), for (b) HCl (a strong acid) is titrated with NH3 (a weak base), and for (c) KOH (a strong base) is titrated with HI (a strong acid).
02

Determine the pH at Equivalence Point for Each Pair

The pH at the equivalence point for a titration between a strong acid and a strong base is 7. If the base is weak and the acid is strong, the pH will be less than 7, and if the acid is weak and the base is strong, the pH will be more than 7. Applying this understanding to each pair, (a) should have a pH above 7 because it is a strong base with a weak base, (b) should have a pH below 7 because it is a strong acid with a weak base, and (c) should have a pH of 7 because it is a strong acid with a strong base.

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Most popular questions from this chapter

Consider a solution containing two weak monoprotic acids with dissociation constants \(K_{\mathrm{HA}}\) and \(K_{\mathrm{HB}}\). Find the charge balance equation for this system, and use it to derive an expression that gives the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) as a function of the concentrations of \(\mathrm{HA}\) and HB and the various constants.

Determine the following characteristics of the titration curve for \(20.0 \mathrm{mL}\) of \(0.275 \mathrm{M} \mathrm{NH}_{3}(\mathrm{aq})\) titrated with \(0.325 \mathrm{M} \mathrm{HI}(\mathrm{aq})\) (a) the initial \(\mathrm{pH}\) (b) the volume of \(0.325 \mathrm{M} \mathrm{HI}(\mathrm{aq})\) at the equivalence point (c) the \(\mathrm{pH}\) at the half-neutralization point (d) the \(\mathrm{pH}\) at the equivalence point

Calculate the pH at the points in the titration of \(25.00 \mathrm{mL}\) of \(0.160 \mathrm{M} \mathrm{HCl}\) when (a) \(10.00 \mathrm{mL}\) and \((\mathrm{b}) 15.00 \mathrm{mL}\) of 0.242 M KOH have been added.

Both sodium hydrogen carbonate (sodium bicarbonate) and sodium hydroxide can be used to neutralize acid spills. What is the pH of \(1.00 \mathrm{M} \mathrm{NaHCO}_{3}(\mathrm{aq})\) and of \(1.00 \mathrm{M} \mathrm{NaOH}(\mathrm{aq}) ?\) On a per-liter basis, do these two solutions have an equal capacity to neutralize acids? Explain. On a per-gram basis, do the two solids, \(\mathrm{NaHCO}_{3}(\mathrm{s})\) and \(\mathrm{NaOH}(\mathrm{s}),\) have an equal capacity to neutralize acids? Explain. Why do you suppose that \(\mathrm{NaHCO}_{3}\) is often preferred to \(\mathrm{NaOH}\) in neutralizing acid spills?

Calculate the \(\mathrm{pH}\) of a buffer that is (a) \(0.012 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\left(K_{\mathrm{a}}=6.3 \times 10^{-5}\right)\) and 0.033 \(\mathrm{M} \mathrm{NaC}_{6} \mathrm{H}_{5} \mathrm{COO}\) (b) \(0.408 \mathrm{M} \mathrm{NH}_{3}\) and \(0.153 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\)
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