Open Question
Find the pH of each mixture of acids. a. 0.075 M in HNO3 and 0.175 M in HC7H5O2 b. 0.020 M in HBr and 0.015 M in HClO4 c. 0.095 M in HF and 0.225 M in HC6H5O d. 0.100 M in formic acid and 0.050 M in hypochlorous acid
Ch.17 - Acids and Bases
Chapter 17, Problem 82b
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. b. 0.0112 M Ba(OH)2
Verified step by step guidance1
Determine the concentration of hydroxide ions, [OH^-], from the dissociation of Ba(OH)_2. Since Ba(OH)_2 is a strong base, it dissociates completely in water. Each formula unit of Ba(OH)_2 produces two OH^- ions. Therefore, [OH^-] = 2 \times 0.0112 \, M.
Calculate the concentration of hydronium ions, [H_3O^+], using the relationship between [OH^-] and [H_3O^+]. The product of [OH^-] and [H_3O^+] is equal to the ion product of water, K_w = 1.0 \times 10^{-14} \, at \, 25^\circ C. Use the formula [H_3O^+] = \frac{K_w}{[OH^-]}.
Determine the pOH of the solution using the formula pOH = -\log[OH^-].
Calculate the pH of the solution using the relationship between pH and pOH: pH + pOH = 14.
Summarize the results: [OH^-], [H_3O^+], pH, and pOH for the 0.0112 M Ba(OH)_2 solution.
Verified Solution
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 Ba(OH)2. The concentration of the base directly correlates to the concentration of OH- ions in solution.
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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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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+] when [OH-] is known, and vice versa, which is essential for determining pH and pOH in strong base solutions.
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Related Practice
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