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Chapter 15: Problem 23

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 can neutralize added H+ ions and OH- ions as follows: When H+ ions are added: \( H^{+} (aq) + HCO_{3}^{-} (aq) \rightarrow H_{2}O (l) + CO_{2} (g) \) When OH- ions are added: \( OH^{-} (aq) + CO_{3}^{2-} (aq) \rightarrow CO_{3}^{2-} (aq) + H_{2}O (l) \) These reactions help to minimize changes in pH when acids or bases are added to the buffer solution.

Step by step solution

01

Write equations for the dissociation of NaHCO3 and Na2CO3 in water

When NaHCO3 and Na2CO3 are dissolved in water, they will dissociate as follows: NaHCO3 (aq) → Na+ (aq) + HCO3- (aq) Na2CO3 (aq) → 2Na+ (aq) + CO3^2- (aq)
02

Write equation for HCO3- reacting with H+ ions

When H+ ions are added to the buffer solution, they will react with HCO3- ions present in the solution. The reaction equation can be written as: H+ (aq) + HCO3- (aq) → H2O (l) + CO2 (g) In this reaction, the added H+ ions are consumed by HCO3- ions, preventing a significant change in pH of the solution.
03

Write equation for CO3^2- reacting with OH- ions

When OH- ions are added to the buffer solution, they will react with CO3^2- ions present in the solution. The reaction equation can be written as: OH- (aq) + CO3^2- (aq) → CO3^2- (aq) + H2O (l) In this reaction, the added OH- ions are consumed by CO3^2- ions, preventing a significant change in pH of the solution. To summarize, the buffer made by dissolving NaHCO3 and Na2CO3 in water can neutralize added H+ ions via reaction with HCO3- ions, and neutralize added OH- ions via reaction with CO3^2- ions. These reactions help to minimize changes in pH when acids or bases are added to the buffer solution.

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Most popular questions from this chapter

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