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Chapter 15: Problem 15

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 \(\overline{\mathrm{OH}}^{-}\).

Short Answer

Expert verified
The buffer neutralizes added H⁺ and OH⁻ ions through the reactions: \[ HCO_3^- + H^+ \rightarrow H_2CO_3 \] and \[ CO_3^{2-} + OH^- \rightarrow HCO_3^- \]

Step by step solution

01

Write the dissociation equations for NaHCO₃ and Na₂CO₃.

When dissolved in water, NaHCO₃ and Na₂CO₃ dissociate as follows: For NaHCO₃: \[ NaHCO_3 \rightarrow Na^+ + HCO_3^- \] For Na₂CO₃: \[ Na_2CO_3 \rightarrow 2Na^+ + CO_3^{2-} \]
02

Identify the acidic and basic species in the buffer.

In the buffer solution, HCO₃⁻ acts as the acidic species, and CO₃²⁻ acts as the basic species.
03

Write the equation for neutralization of H⁺ ions by HCO₃⁻.

When H⁺ ions are added to the buffer solution, HCO₃⁻ will react with them to neutralize the H⁺ ions. The reaction can be represented as follows: \[ HCO_3^- + H^+ \rightarrow H_2CO_3 \]
04

Write the equation for the neutralization of OH⁻ ions by CO₃²⁻.

When OH⁻ ions are added to the buffer solution, CO₃²⁻ will react with them to neutralize the OH⁻ ions. The reaction can be represented as follows: \[ CO_3^{2-} + OH^- \rightarrow HCO_3^- \] With these equations, we have found how the buffer solution neutralizes both H⁺ and OH⁻ ions added to it.

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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 \(0.50 \mathrm{M} \mathrm{HCl}\), calculate the \(\mathrm{pH}\) under the following conditions. a. after \(50.0 \mathrm{~mL}\) of \(0.50 \mathrm{M} \mathrm{HCl}\) has been added b. at the stoichiometric point

Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.

Figure \(15.4\) shows the pH curves for the titrations of six different acids by \(\mathrm{NaOH}\). Make a similar plot for the titration of three different bases by \(0.10 M\) HCl. Assume \(50.0 \mathrm{~mL}\) of \(0.20 \mathrm{M}\) of the bases and assume the three bases are a strong base \((\mathrm{KOH})\), a weak base with \(K_{\mathrm{b}}=1 \times 10^{-5}\), and another weak base with \(K_{\mathrm{b}}=1 \times 10^{-10}\)

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

Methyl red has the following structure: CN(C)c1ccc(N=Nc2ccccc2C(=O)O)cc1 It undergoes a color change from red to yellow as a solution gets more basic. Calculate an approximate \(\mathrm{pH}\) range for which methyl red is useful. What is the color change and the \(\mathrm{pH}\) at the color change when a weak acid is titrated with a strong base using methyl red as an indicator? What is the color change and the \(\mathrm{pH}\) at the color change when a weak base is titrated with a strong acid using methyl red as an indicator? For which of these two types of titrations is methyl red a possible indicator?
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