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Ch.16 - Acids and Bases
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.16 - Acids and BasesProblema 81
Capitolo 16, Problema 81

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. a. 0.15 M NaOH b. 1.5×10–3 M Ca(OH)2 c. 4.8×10–4 M Sr(OH)2 d. 8.7×10–5 M KOH

Guida verificata passo dopo passo
1
Identify the strong base: Calcium hydroxide, Ca(OH)_2, is a strong base that dissociates completely in water.
Write the dissociation equation: Ca(OH)_2 \(\rightarrow\) Ca^{2+} + 2OH^{-}.
Calculate [OH^-]: Since each formula unit of Ca(OH)_2 produces two OH^- ions, multiply the concentration of Ca(OH)_2 by 2 to find [OH^-].
Calculate [H_3O^+]: Use the water dissociation constant, K_w = 1.0 \(\times\) 10^{-14}, and the relationship [H_3O^+][OH^-] = K_w to find [H_3O^+].
Determine pH and pOH: Use the formulas pOH = -\(\log\)[OH^-] and pH = 14 - pOH to find the pH and pOH 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 and alkaline earth metal hydroxides, such as calcium hydroxide (Ca(OH)2). The concentration of the base directly influences the concentration of OH- ions in solution.
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Strong Acid-Strong Base Titration

pH and pOH Calculations

pH and pOH are measures of the acidity and basicity of a solution, respectively. pH is calculated as the negative logarithm of the hydronium ion concentration ([H3O+]), while pOH is 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.
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pH and pOH Calculations

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 allows for the calculation of [H3O+] from [OH-] and vice versa, which is essential for determining the pH and pOH of a solution when the concentration of a strong base is known.
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Production of Hydrogen Example
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