Textbook Question
Determine the [H3O+] and pH of a 0.100 M solution of benzoic acid.
Ch.16 - Acids and Bases
Chapter 16, Problem 66
Determine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8×10–4.) a. 0.250 M b. 0.0500 M c. 0.0250 M
Verified step by step guidance1
1. The first step is to write the ionization equation for HF. HF is a weak acid, so it partially ionizes in water to form H+ and F-. The equation is: HF ⇌ H+ + F-.
2. Next, set up the ICE (Initial, Change, Equilibrium) table. For a 0.250 M HF solution, the initial concentrations are [HF] = 0.250 M, [H+] = 0 and [F-] = 0. The change in concentration is -x for HF and +x for H+ and F-. At equilibrium, the concentrations are [HF] = 0.250 - x, [H+] = x and [F-] = x.
3. The third step is to write the expression for the acid dissociation constant (Ka) and substitute the equilibrium concentrations from the ICE table. Ka = [H+][F-] / [HF] = (x)(x) / (0.250 - x) = 6.8 * 10^-4.
4. Solve the equation for x, which represents the concentration of H+ ions. If x is less than 5% of the initial concentration of HF, then the simplifying assumption that x is small is valid. If x is greater than 5% of the initial concentration, then the assumption is not valid and you would need to use the quadratic formula to solve for x.
5. Once you have the concentration of H+ ions, you can calculate the pH of the solution using the formula pH = -log[H+]. Repeat these steps for the other concentrations of HF.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Equilibrium
Acid-base equilibrium involves the balance between an acid and its conjugate base in solution. For weak acids like hydrofluoric acid (HF), this equilibrium can be described by the dissociation constant (Ka), which quantifies the extent to which the acid donates protons (H+) to the solution. Understanding this concept is crucial for calculating pH and determining the concentration of ions in solution.
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Triprotic Acid Equilibrium
pH Calculation
pH is a measure of the hydrogen ion concentration in a solution, calculated using the formula pH = -log[H+]. For weak acids, the pH can be determined from the equilibrium expression derived from the acid dissociation constant (Ka). This calculation often requires setting up an ICE (Initial, Change, Equilibrium) table to find the concentration of H+ ions at equilibrium.
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Assumption of Small x
In weak acid calculations, the assumption that 'x' (the change in concentration due to dissociation) is small simplifies the math. This assumption is valid when the initial concentration of the acid is significantly higher than Ka. However, if the initial concentration is low (close to the value of Ka), this assumption may not hold, leading to inaccurate results. Identifying when this assumption is valid is essential for accurate pH calculations.
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04:23Low-Spin Complexes are associated with large Δ values and High-Spin Complexes are associated with small Δ values.
Related Practice
Textbook Question
Determine the [H3O+] and pH of a 0.200 M solution of formic acid.
Textbook Question
Determine the pH of an HNO2 solution of each concentration. In which cases can you not make the simplifying assumption that x is small? a. 0.500 M b. 0.100 M c. 0.0100 M
Textbook Question
A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka) for the acid.
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