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Chapter 14: Problem 19

A certain buffer is made by dissolving \(\mathrm{NaHCO}_{3}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) in some water. Write equations to show how this buffer neutralizes added \(\mathrm{H}^{+}\) and \(\mathrm{OH}^{-}\).

Short Answer

Expert verified
The buffer made by dissolving NaHCO3 and Na2CO3 in water neutralizes added H+ and OH- ions through the following reactions: 1. Reaction of bicarbonate ion (HCO3-) with H+ ions: \( HCO_3^-(aq) + H^+(aq) \rightarrow H_2CO_3(aq) \) 2. Reaction of carbonate ion (CO3^2-) with H+ ions: \( CO_3^{2-}(aq) + H^+(aq) \rightarrow HCO_3^-(aq) \) 3. Reaction of bicarbonate ion (HCO3-) with OH- ions: \( HCO_3^-(aq) + OH^-(aq) \rightarrow H_2O(l) + CO_3^{2-}(aq) \)

Step by step solution

01

Identify the buffer components when they are dissolved in water

When NaHCO3 and Na2CO3 are dissolved in water, they will dissociate and form their respective ions: 1. \( NaHCO_3(s) \rightarrow Na^+(aq) + HCO_3^-(aq) \) 2. \( Na_2CO_3(s) \rightarrow 2Na^+(aq) + CO_3^{2-}(aq) \)
02

Write the equation for the reaction of bicarbonate ion with H+ ions

The bicarbonate ion (HCO3-) will react with the H+ ion, neutralizing it and forming carbonic acid (H2CO3). We can represent this reaction as follows: \( HCO_3^-(aq) + H^+(aq) \rightarrow H_2CO_3(aq) \)
03

Write the equation for the reaction of carbonate ion with H+ ions

The carbonate ion (CO3^2-) will also react with the H+ ion, neutralizing it and forming bicarbonate ion (HCO3-). We can represent this reaction as follows: \( CO_3^{2-}(aq) + H^+(aq) \rightarrow HCO_3^-(aq) \)
04

Write the equation for the reaction of bicarbonate ion with OH- ions

The bicarbonate ion (HCO3-) can also react with the added OH- ion. In this reaction, the bicarbonate ion (HCO3-) will donate a proton (H+) to the OH- ion, forming water (H2O) and the carbonate ion (CO3^2-). We can represent this reaction as follows: \( HCO_3^-(aq) + OH^-(aq) \rightarrow H_2O(l) + CO_3^{2-}(aq) \) With these four equations, we can now demonstrate how the given buffer consisting of NaHCO3 and Na2CO3 neutralizes added H+ and OH- ions through the reactions with bicarbonate and carbonate ions in the buffer system.

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Most popular questions from this chapter

In the titration of \(50.0 \mathrm{mL}\) of \(1.0 \mathrm{M}\) methylamine, \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) \(\left(K_{\mathrm{b}}=4.4 \times 10^{-4}\right),\) with \(0.50 M\) HCl, calculate the pH under the following conditions. a. after \(50.0 \mathrm{mL}\) of \(0.50 \mathrm{M}\) HCl has been added b. at the stoichiometric point

Calculate the \(\mathrm{pH}\) of each of the following solutions. a. \(0.100 M\) HONH \(_{2}\left(K_{\mathrm{b}}=1.1 \times 10^{-8}\right)\) b. \(0.100 M\) HONH \(_{3}\) Cl c. pure \(\mathrm{H}_{2} \mathrm{O}\) d. a mixture containing 0.100 \(M \mathrm{HONH}_{2}\) and \(0.100 \mathrm{M}\) \(\mathrm{HONH}_{3} \mathrm{Cl}\)

You have \(75.0 \mathrm{mL}\) of \(0.10 \mathrm{M}\) HA. After adding \(30.0 \mathrm{mL}\) of \(0.10 M \mathrm{NaOH},\) the \(\mathrm{pH}\) is \(5.50 .\) What is the \(K_{\mathrm{a}}\) value of \(\mathrm{HA} ?\)

A \(10.00-g\) sample of the ionic compound \(\mathrm{NaA}\), where \(\mathrm{A}^{-}\) is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 \(M\) HCl. After 500.0 mL HCl was added, the pH was \(5.00 .\) The experimenter found that 1.00 L of \(0.100 M\) HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the \(p\) H of the solution at the stoichiometric point of the titration.

Consider the titration of \(100.0 \mathrm{mL}\) of \(0.100 \mathrm{M}\) HCN by \(0.100 M \mathrm{KOH}\) at \(25^{\circ} \mathrm{C} .\left(K_{\mathrm{a}} \text { for } \mathrm{HCN}=6.2 \times 10^{-10} .\right)\) a. Calculate the \(\mathrm{pH}\) after \(0.0 \mathrm{mL}\) of \(\mathrm{KOH}\) has been added. b. Calculate the \(\mathrm{pH}\) after \(50.0 \mathrm{mL}\) of \(\mathrm{KOH}\) has been added. c. Calculate the \(\mathrm{pH}\) after \(75.0 \mathrm{mL}\) of \(\mathrm{KOH}\) has been added. d. Calculate the \(\mathrm{pH}\) at the equivalence point. e. Calculate the pH after 125 mL of KOH has been added.
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