Chemistry Chapter: Acid-Base Equilibria

What is the equilibrium constant expression for the autoionization of water?

If the concentration of hydroxide ions ([OH-]) in a solution is 1.0 x 10^-10 M, what is the concentration of hydronium ions ([H3O+]) at 25°C?

A solution with a pH of 11 would best be described as what?

Which of the following statements accurately describes the autoionization of water?

What is the pOH of a solution with a hydronium ion concentration of 1.0 x 10^-3 M at 25°C?

In the Henderson-Hasselbalch equation, what does the term 'pKa' represent?

A buffer solution is prepared by mixing 0.10 M CH3COOH and 0.10 M CH3COONa. What is the pH of this buffer if the Ka for CH3COOH is 1.8 x 10^-5?

Which of the following statements is TRUE about a buffer solution?

What is the pH of a solution containing 0.10 M HCOOH and 0.10 M HCOO- if the pKa of HCOOH is 3.75?

A buffer solution is prepared by mixing 0.20 M NH3 and 0.10 M NH4Cl. If the Kb for NH3 is 1.8 x 10-5, what is the pH of this buffer solution?

What is the pH of a buffer solution consisting of 0.10 M H2CO3 and 0.10 M HCO3- if the Ka for H2CO3 is 4.3 x 10^-7?

A buffer solution is prepared by mixing 0.25 M HF and 0.50 M NaF. What is the pH of this buffer if the Ka for HF is 7.2 x 10^-4?

A solution containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74 (pKa for CH3COOH is 4.74). If 0.01 mol of NaOH is added to 1 L of this buffer solution, what is the new pH of the solution?

A student is performing an acid-base titration using a burette filled with a standardized sodium hydroxide solution. During the titration, they observe that the solution in the burette has air bubbles. Why is this a problem?

In a titration, a drop of phenolphthalein indicator is added to the analyte solution. What color change would the student expect to observe as the titration progresses?

A student carefully added 10.0 mL of hydrochloric acid to a clean Erlenmeyer flask. After the titrant was added, the student observed that the solution in the flask was still acidic. What should the student do next?

Why is it important to record the initial and final burette readings to the nearest 0.1mL during a titration?

In the titration, a student records the initial burette reading as 10.0 mL and the final reading as 25.5 mL. What is the total volume of sodium hydroxide solution used in the titration?

The normality of a solution is defined as the number of equivalents of solute per liter of solution. What is the normality of a 0.1 M solution of sodium hydroxide (NaOH)?

What is the primary purpose of using indicators like phenolphthalein in a titration?

A student is titrating a solution of hydrochloric acid (HCl) with a standard sodium hydroxide solution (NaOH). What is the significance of the equivalence point in this titration?

In the equilibrium reaction given, what would happen if the initial concentration of CH3COOH is increased to 0.20M, while the initial concentration of H3O+ is kept constant at 0.10M?

Why is the Cl− ion considered a spectator ion in the reaction shown?

What is the significance of the statement 'x is very small' in the calculation of Ka?

In the calculation of Ka, why is (0.10 − x) approximated to 0.10?

A solution containing 0.20 M CH3COOH and 0.30 M CH3COONa acts as a buffer. Which of the following statements accurately describes the role of CH3COONa in this buffer?

What is the pH of a buffer solution after the addition of a small amount of strong base, like NaOH?

A buffer is defined as a solution that resists changes in pH. Why does a buffer solution resist such changes?

Why is the addition of a small amount of acid or base to a buffer solution less likely to cause a significant change in pH, whereas the same amount of acid or base added to an unbuffered solution would cause a larger pH change?

What is the approximate hydroxide ion concentration, [OH-], in a 0.040 M solution of ammonia (NH3)?

What is the value of [NH3] at equilibrium in a 0.040 M ammonia solution, considering the approximation method used in the content?

If the approximation method used in the content is deemed invalid for a 0.040 M ammonia solution, how would you proceed to find the equilibrium concentration of ammonia?

Which of the following is NOT a valid assumption for the use of the approximation method in calculating equilibrium concentrations of a weak base like ammonia?

What is the value of the pOH of a 0.040 M ammonia solution, assuming the approximation method is valid?

What is the pH of a 0.040 M ammonia solution, given that the pOH is 11.23?

What is the effect on the equilibrium position of the ammonia ionization reaction in water when the common ion (e.g., ammonium ion) is added?

Which of the following statements correctly describes the common ion effect?

Why is a weak acid-base conjugate pair necessary for effective buffer solutions?

Explain why the equilibrium concentrations of acetic acid (CH3COOH) and acetate ions (CH3COO-) in a buffer solution are assumed to be similar to their starting concentrations.

How does a buffer solution containing acetic acid and sodium acetate neutralize the addition of a base (OH-)?

What is the main reason why the pH of blood is maintained at around 7.4?

How does the Henderson-Hasselbalch equation relate to the pH of a buffer solution?

Which of these statements accurately describes the principle underlying the functioning of a buffer solution?

Which of the following scenarios would NOT be a suitable application of a buffer solution?

How does the concentration of the buffer components affect its buffering capacity?