Textbook Question
Determine whether or not the mixing of each pair of solutions results in a buffer. b. 50.0 mL of 0.10 M HCl; 35.0 mL of 0.150 M NaOH
Ch.18 - Aqueous Ionic Equilibrium
Chapter 18, Problem 53e
Determine whether or not the mixing of each pair of solutions results in a buffer. e. 125.0 mL of 0.15 M NH3; 150.0 mL of 0.20 M NaOH
Verified step by step guidance1
Identify the components needed for a buffer solution: a weak base and its conjugate acid, or a weak acid and its conjugate base.
Recognize that NH3 (ammonia) is a weak base, and NaOH (sodium hydroxide) is a strong base.
Calculate the moles of NH3 using the formula: moles = concentration (M) \times volume (L).
Calculate the moles of NaOH using the formula: moles = concentration (M) \times volume (L).
Determine if the strong base (NaOH) will convert some of the weak base (NH3) into its conjugate acid (NH4+), and check if there is enough NH3 left to form a buffer.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Buffer Solutions
A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base or a weak base and its conjugate acid. Buffers maintain pH stability, which is crucial in many chemical and biological processes.
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Buffer Solutions
Weak Bases and Conjugate Acids
Weak bases, like ammonia (NH3), partially ionize in solution to form hydroxide ions (OH-) and their conjugate acids. The presence of both the weak base and its conjugate acid in a solution is essential for buffer action. In this case, NH3 can act as a weak base, while NH4+ (ammonium ion) would be its conjugate acid.
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pH and Hydroxide Ion Concentration
The pH of a solution is a measure of its acidity or basicity, determined by the concentration of hydrogen ions (H+). When mixing solutions, the resulting pH depends on the concentrations of acids and bases present. In this scenario, the addition of NaOH, a strong base, will affect the overall pH and the potential for buffer formation with NH3.
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Related Practice
Textbook Question
Determine whether or not the mixing of each pair of solutions results in a buffer. c. 50.0 mL of 0.15 M HF; 20.0 mL of 0.15 M NaOH
Textbook Question
Determine whether or not the mixing of each pair of solutions results in a buffer. d. 175.0 mL of 0.10 M NH3; 150.0 mL of 0.12 M NaOH
Textbook Question
Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH3NH2; 120.0 mL of 0.25 M CH3NH3Cl
Textbook Question
Determine whether or not the mixing of each pair of solutions results in a buffer. c. 165.0 mL of 0.10 M HF; 135.0 mL of 0.050 M KOH
Textbook Question
Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1).
a. What is the pH of blood plasma?