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Ch.10 Acids and Bases and Equilibrium
Timberlake - Chemistry: An Introduction to General, Organic, and Biological Chemistry 14th Edition
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTimberlake 14th EditionCh.10 Acids and Bases and EquilibriumProblema 108a
Capitolo 10, Problema 108a

Determine each of the following for a 0.100 M HBr solution:
a. [H3O+]

Guida verificata passo dopo passo
1
Step 1: Recognize that HBr is a strong acid, meaning it completely dissociates in water. The dissociation reaction can be written as: HBr → H⁺ + Br⁻. Since it dissociates completely, the concentration of [H⁺] (or equivalently [H₃O⁺]) will be equal to the initial concentration of HBr.
Step 2: Identify the given concentration of HBr, which is 0.100 M. This means that for every mole of HBr, 1 mole of H⁺ ions is produced.
Step 3: Use the relationship between the concentration of HBr and [H₃O⁺]. Since HBr dissociates completely, [H₃O⁺] = [HBr]. Therefore, [H₃O⁺] is equal to 0.100 M.
Step 4: Write the final expression for [H₃O⁺] as [H₃O⁺] = 0.100 \(\text{ M}\). This is the hydronium ion concentration in the solution.
Step 5: Verify the logic by recalling that strong acids like HBr fully dissociate, so the concentration of [H₃O⁺] directly matches the initial molarity of the acid.

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Strong Acids and Ionization

Strong acids, like HBr, completely dissociate in water, meaning that all the acid molecules break apart into ions. For a 0.100 M HBr solution, this results in a concentration of H⁺ ions equal to the concentration of the acid, which is 0.100 M. This complete ionization is crucial for calculating the hydronium ion concentration.
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Strong Acids and Bases

Hydronium Ion Concentration

The concentration of hydronium ions, [H₃O⁺], in a solution is a measure of the acidity of that solution. In the case of strong acids, the concentration of H₃O⁺ is directly derived from the concentration of the acid. For a 0.100 M HBr solution, the [H₃O⁺] is also 0.100 M, reflecting the complete dissociation of the acid.
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Percent Concentrations Concept 1

pH Scale

The pH scale quantifies the acidity or basicity of a solution, with lower values indicating higher acidity. It is calculated using the formula pH = -log[H₃O⁺]. For a 0.100 M HBr solution, knowing the [H₃O⁺] allows us to calculate the pH, which is an essential aspect of understanding the solution's properties.
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The pH Scale
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