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Chapter 16: Problem 37

Do all titrations of samples of strong monoprotic acids with solutions of strong bases have the same pH at their equivalence points? Explain why or why not.

Short Answer

Expert verified
Answer: Yes, all titrations of samples of strong monoprotic acids with solutions of strong bases have the same pH at their equivalence points, which is 7. This is because, at the equivalence point, the number of moles of H+ ions from the acid equal the number of moles of OH- ions from the base, producing a neutral solution and having equal [H鈦篯 and [OH鈦籡 concentrations.

Step by step solution

01

1. Understanding strong acids and strong bases

Strong acids are chemicals that completely dissociate into their ions when dissolved in water. This results in a high concentration of H+ ions in the solution. Examples of strong acids include hydrochloric acid (HCl), sulphuric acid (H鈧係O鈧�), and nitric acid (HNO鈧�). Likewise, strong bases completely dissociate into their respective ions when dissolved in water, having a high concentration of OH- ions. Examples of strong bases include sodium hydroxide (NaOH) and potassium hydroxide (KOH).
02

2. Understanding the equivalence point in a titration

The equivalence point in a titration is the point at which the moles of the titrant (typically a strong base in our case) added are equal to the moles of the analyte (typically a strong monoprotic acid in our case). This means that the reaction between the strong acid and strong base is complete, producing a neutral solution (in the case of a strong monoprotic acid and strong base). At the equivalence point, the number of moles of H+ from the acid equals the number of moles of OH- from the base, forming H2O.
03

3. Calculating the pH at the equivalence point

To determine the pH at the equivalence point, we need to know the concentration of OH- ions or H+ ions in the solution at that moment. As mentioned before, at the equivalence point, the number of moles of H+ is equal to the number of moles of OH-, which means that the solution is neutral. Since water is produced as a result of the reaction, it is essential to consider the ionization of water: H鈧侽 鈬� H鈦� + OH鈦� When the solution is neutral, the concentration of H鈦� and OH鈦� ions are equal ([H鈦篯=[OH鈦籡=1x10^(-7) M), and the pH is calculated as: pH = -log[H鈦篯 For a neutral solution ([H鈦篯=1x10^(-7)), we obtain a pH of 7 at the equivalence point.
04

4. Answering the question: Do all strong monoprotic acids and strong bases titrations have the same pH at their equivalence points?

Yes, titrations of samples of strong monoprotic acids with solutions of strong bases have the same pH at their equivalence points, which is 7. This is because, at the equivalence point, the number of moles of H+ ions from the acid equal the number of moles of OH- ions from the base, producing a neutral solution and having equal [H鈦篯 and [OH鈦籡 concentrations.

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Most popular questions from this chapter

People with diabetes can have elevated levels of two acids in their blood: \(\beta\) -hydroxybutyric acid \(\left(\mathrm{p} K_{\mathrm{a}}=4.72\right)\) and acetoacetic acid \(\left(\mathrm{p} K_{\mathrm{a}}=3.58\right)\) (EQUATION CAN'T COPY) The presence of these acids lowers the \(\mathrm{pH}\) of blood and can serve to diagnose diabetes. a. Which acid yields a solution with the lower \(\mathrm{pH}\) if \(0.100 M\) solutions are prepared? b. Which acid will dissociate to a greater degree? c. What is the pH of a solution that contains \(15.8 \mathrm{mM}\) of acetoacetic acid and \(10.8 \mathrm{m} M\) sodium acetoacetate? d. What is the \(\mathrm{pH}\) of a solution of \(90 \mathrm{mg} / \mathrm{L}\) \beta-hydroxybutyric acid and 90 mg/L \(\beta\) -hydroxybutyrate anion after \(100 \mu \mathrm{L}\) of \(0.100 M\) HCl has been added?

What masses of bromoacetic acid and sodium bromoacetate are needed to prepare \(1.00 \mathrm{L}\) of \(\mathrm{pH}=3.00\) buffer if the total concentration of the two components is \(0.200 M ?\)

Why does a solution of a weak acid and its conjugate base control pH better than a solution of the weak acid alone?

Which cation will precipitate first as a carbonate mineral from an equimolar solution of \(\mathrm{Mg}^{2+}, \mathrm{Ca}^{2+},\) and \(\mathrm{Sr}^{2+} ?\)

Suppose you have 100 mL of each of the following solutions. In which will the most \(\mathrm{CaCO}_{3}\) dissolve? (a) \(0.1 M \mathrm{NaCl} ;\) (b) \(0.1 M \mathrm{Na}_{2} \mathrm{CO}_{3} ;\) (c) \(0.1 \mathrm{M} \mathrm{NaOH}\) (d) \(0.1 M \mathrm{HCl}\)
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