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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

A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After \(23.75 \mathrm{mL}\) of the weak acid solution has been added to \(50.0 \mathrm{mL}\) of the \(0.100 \mathrm{M} \mathrm{NaOH}\) solution, the \(\mathrm{pH}\) of the resulting solution is \(10.50 .\) Calculate the original concentration of the solution of weak acid.

A buffer is made using \(45.0 \mathrm{mL}\) of \(0.750 \mathrm{M} \mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}\left(K_{\mathrm{a}}=\right.\) \(1.3 \times 10^{-5}\) ) and \(55.0 \mathrm{mL}\) of \(0.700 \mathrm{M} \mathrm{NaC}_{3} \mathrm{H}_{5} \mathrm{O}_{2} .\) What volume of 0.10 \(M\) NaOH must be added to change the pH of the original buffer solution by \(2.5 \% ?\)

Consider \(1.0 \mathrm{L}\) of a solution that is \(0.85 \mathrm{M} \mathrm{HOC}_{6} \mathrm{H}_{5}\) and \(0.80 M \mathrm{NaOC}_{6} \mathrm{H}_{5} .\left(K_{\mathrm{a}} \text { for } \mathrm{HOC}_{6} \mathrm{H}_{5}=1.6 \times 10^{-10} .\right)\) a. Calculate the \(\mathrm{pH}\) of this solution. b. Calculate the \(\mathrm{pH}\) after 0.10 mole of HCl has been added to the original solution. Assume no volume change on addition of HCl. c. Calculate the \(\mathrm{pH}\) after 0.20 mole of \(\mathrm{NaOH}\) has been added to the original buffer solution. Assume no volume change on addition of NaOH.

You make 1.00 L of a buffered solution \((p H=4.00)\) by mixing acetic acid and sodium acetate. You have \(1.00 M\) solutions of each component of the buffered solution. What volume of each solution do you mix to make such a buffered solution?

Acid-base indicators mark the end point of titrations by "magically" turning a different color. Explain the "magic" behind acid-base indicators.
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