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Ch.17 - Acids and Bases
Tro - Chemistry: A Molecular Approach 6th Edition
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Tutti i libri di testoTro 6th EditionCh.17 - Acids and BasesProblema 86d
Capitolo 17, Problema 86d

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. d. 5.0×10–4 M Ca(OH)2

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Identify that calcium hydroxide, Ca(OH)_2, is a strong base and dissociates completely in water.
Write the dissociation equation: Ca(OH)_2 \(\rightarrow\) Ca^{2+} + 2OH^{-}.
Calculate the concentration of OH^{-} ions. Since each formula unit of Ca(OH)_2 produces two OH^{-} ions, multiply the concentration of Ca(OH)_2 by 2.
Use the concentration of OH^{-} to find pOH using the formula: \(\text{pOH}\) = -\(\log\)[OH^{-}].
Calculate the pH using the relationship: \(\text{pH}\) + \(\text{pOH}\) = 14.

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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 affects 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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