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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 52
Capitolo 17, Problema 52

A 100.0-mL buffer solution is 0.100 M in NH3 and 0.125 M in NH4Br. What mass of HCl can this buffer neutralize before the pH falls below 9.00?

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First, we need to calculate the pOH from the given pH. We can use the formula pOH = 14 - pH.
Next, we need to calculate the concentration of OH- ions using the formula [OH-] = 10^-pOH.
Then, we need to calculate the concentration of NH3 in the buffer solution. We know that the concentration of NH3 is 0.100 M.
Now, we need to calculate the concentration of NH4+ ions in the buffer solution. We know that the concentration of NH4+ is 0.125 M.
Finally, we can calculate the mass of HCl that the buffer can neutralize. We know that the reaction between NH3 and HCl produces NH4+ and Cl-. Therefore, the amount of HCl that can be neutralized is equal to the amount of NH3 present in the buffer. We can use the formula mass = volume x concentration x molar mass to calculate the mass of HCl.

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Buffer Solutions

Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. In this case, the NH3/NH4Br system acts as a buffer, maintaining the pH around 9.00 despite the addition of HCl.
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Buffer Solutions

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates the pH of a buffer solution to the concentration of its acidic and basic components. It is expressed as pH = pKa + log([A-]/[HA]). For the NH3/NH4+ buffer, knowing the pKa allows us to calculate how much HCl can be added before the pH drops below a specified value.
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Henderson-Hasselbalch Equation

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to form water and a salt. In this scenario, HCl (strong acid) will react with NH3 (weak base) to form NH4Cl and water. The extent of this reaction determines how much HCl can be added to the buffer before the pH changes significantly.
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Lewis Dot Structures: Neutral Compounds
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