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Ch.17 - Acids and Bases
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.17 - Acids and BasesProblema 86a
Capitolo 17, Problema 86a

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. a. 8.77×10–3 M LiOH

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Step 1: Identify the strong base and its dissociation. LiOH is a strong base, which means it dissociates completely in water. The dissociation can be represented as: \[ \text{LiOH} \rightarrow \text{Li}^+ + \text{OH}^- \]. Therefore, the concentration of \( \text{OH}^- \) ions is equal to the concentration of the LiOH solution, which is \( 8.77 \times 10^{-3} \text{ M} \).
Step 2: Calculate the \( [\text{OH}^-] \). Since LiOH dissociates completely, \( [\text{OH}^-] = 8.77 \times 10^{-3} \text{ M} \).
Step 3: Use the ion product of water to find \( [\text{H}_3\text{O}^+] \). The ion product of water at 25°C is \( K_w = 1.0 \times 10^{-14} \). Use the formula \( [\text{H}_3\text{O}^+] = \frac{K_w}{[\text{OH}^-]} \) to find \( [\text{H}_3\text{O}^+] \).
Step 4: Calculate the pOH. Use the formula \( \text{pOH} = -\log[\text{OH}^-] \) to find the pOH of the solution.
Step 5: Calculate the pH. Use the relationship \( \text{pH} + \text{pOH} = 14 \) to find the pH of the solution.

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Strong Bases

Strong bases are substances that completely dissociate in water to produce hydroxide ions (OH-). Common examples include alkali metal hydroxides like lithium hydroxide (LiOH). The concentration of the base directly correlates to the concentration of OH- ions in solution, which is crucial for calculating pH and pOH.
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pH and pOH Calculations

pH is a measure of the acidity of a solution, defined as the negative logarithm of the hydrogen ion concentration ([H3O+]). Conversely, pOH measures the basicity, defined as the negative logarithm of the hydroxide ion concentration ([OH-]). The relationship between pH and pOH is given by the equation pH + pOH = 14 at 25°C, allowing for the conversion between these two measures.
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Ion Product of Water

The ion product of water (Kw) is the equilibrium constant for the self-ionization of water, defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C. This relationship is essential for determining the concentrations of H3O+ and OH- in a solution, especially when dealing with strong bases, as it helps to find the corresponding [H3O+] when [OH-] is known.
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