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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.18 - Aqueous Ionic EquilibriumProblema 64
Capitolo 18, Problema 64

A 1.0-L buffer solution is 0.125 M in HNO2 and 0.145 M in NaNO2. Determine the concentrations of HNO2 and NaNO2 after the addition of each substance: a. 1.5 g HCl b. 1.5 g NaOH c. 1.5 g HI

Guida verificata passo dopo passo
1
Step 1: Calculate the moles of HCl added.
Step 2: Write the balanced chemical equation for the reaction between HCl and the buffer components.
Step 3: Determine the initial moles of HNO2 and NaNO2 in the buffer solution.
Step 4: Use the stoichiometry of the reaction to find the change in moles of HNO2 and NaNO2 after the addition of HCl.
Step 5: Calculate the new concentrations of HNO2 and NaNO2 by dividing the final moles by the total volume of the solution.

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Buffer Solutions

A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. In this case, HNO2 (a weak acid) and NaNO2 (its conjugate base) form a buffer that helps maintain the pH when HCl is added.
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03:02
Buffer Solutions

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates the pH of a buffer solution to the concentrations of its acid and conjugate base. It is expressed as pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the base and [HA] is the concentration of the acid. This equation is essential for calculating the pH changes in the buffer after the addition of HCl.
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02:40
Henderson-Hasselbalch Equation

Stoichiometry of Acid-Base Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. When HCl, a strong acid, is added to the buffer, it reacts with the weak base (NaNO2) to form HNO2. Understanding the stoichiometric relationships allows for the determination of the new concentrations of HNO2 and NaNO2 after the reaction.
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Acid-Base Reaction
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Domanda del libro di testo

The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of monoprotic acids, one weak and one strong. Both titrations were carried out with the same concentration of strong base.

(i) What is the approximate pH at the equivalence point of each curve?

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Domanda del libro di testo

The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of monoprotic acids, one weak and one strong. Both titrations were carried out with the same concentration of strong base.

(ii) Which graph corresponds to the titration of the strong acid and which one to the titration of the weak acid?

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Domanda del libro di testo

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. c. 1.25 g HBr

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Domanda del libro di testo

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. d. 1.35 g HI

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Domanda del libro di testo

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH

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