pH & pOH (College Board AP® Chemistry): Exam Questions

A student is analyzing the pH of a solution and finds that the pOH is 4.25 at 25°C.

Using the ionization constant of water (K_w), determine the pH of the solution and explain why pH + pOH = 14 at this temperature.

i) Calculate the pH of the solution using your answer from part (a). Show all working.

ii) Identify whether the solution is acidic, basic, or neutral based on your answer from part (i). Justify your answer by comparing the pH to 7.

If the temperature increases above 25°C, predict how the pH of pure water will change. Justify your answer.

At 50 °C, the ionization constant of water (K_w) is 5.47 × 10⁻¹⁴.

Write the balanced chemical equation for the autoionization of water.

Determine the pH of pure water at 50 °C. Show all working.

Explain how an increase in temperature affects the value of K_w and the pH of pure water. Justify your answer based on the enthalpy change of the autoionization of water

A student investigates how temperature affects the pH of water and how different bases behave in aqueous solution. They perform a series of tests on pure water, 0.0025 M Ba(OH)₂, and a solution of ammonia (NH₃) at 25 °C and 40 °C. The K_b of NH₃ is 1.8 × 10^-5.

At 40 °C, the ionization constant for water is K_w = 2.92 × 10^-14.

Calculate the pH of pure water at this temperature.

At 25 ^oC, the student prepares a solution of 0.0025 M Ba(OH)₂.

Calculate the pH of this solution, assuming complete dissociation.

The student prepares a solution of ammonia (NH₃) at 25 ^oC. The solution is intended to have the same pH as the 0.0025 M Ba(OH)₂ solution from part (b).

Calculate the required concentration of NH₃.

K_b(NH₃) = 1.8 × 10^-5

Assume no change in volume due to ionization.

Explain why the required concentration of NH₃ is higher than that of Ba(OH)₂,
even though the pH values are the same.

At 60 °C, the student measures the pH of pure water to be 6.50.
Does this indicate the water is acidic? Justify your answer.

A 50.0 mL solution of 0.100 M HCl is mixed with 25.0 mL of 0.200 M NaOH at 25°C.

Determine whether the final solution is acidic, basic, or neutral. Show all calculations to justify your answer.

A student prepares two solutions:

Solution A: A neutral solution at 25°C

Solution B: A neutral solution at 50°C

The student claims that both solutions have the same pH. Evaluate this claim and justify your answer using the relationship between pH, pOH, and K_w.

A student is given 50.0 mL of a solution of Na₂CO₃(aq) of unknown concentration. To determine the concentration of the solution, the student mixes the solution with excess 1.0 M Ca(NO₃)₂(aq) , causing a precipitate to form. The balanced equation for the reaction is shown below.

Na₂CO₃ (aq) + Ca(NO₃)₂ (aq) → 2NaNO₃ (aq) + CaCO₃ (s)

Write the net ionic equation for the reaction that occurs when the solutions of Na₂CO₃ and Ca(NO₃)₂ are mixed.

The diagram below is incomplete. Draw in the species needed to accurately represent the major ionic species remaining in the solution after the reaction has been completed.

The student filters and dries the precipitate of CaCO₃ (molar mass 100.1 g/mol) and records the data in the table below.

Determine the number of moles of Na₂CO₃ in the original 50.0 mL of solution.

The student realizes that the precipitate was not completely dried and claims that as a result, the calculated Na₂CO₃ molarity is too low. Do you agree with the student’s claim? Justify your answer.

After the precipitate forms and is filtered, the liquid that passed through the filter is tested to see if it can conduct electricity. What would be observed? Justify your answer.

The student decides to determine the molarity of the same Na₂CO₃ solution using a second method. When Na₂CO₃ is dissolved in water, CO₃²⁻(aq) hydrolyzes to form HCO₃⁻  (aq), as shown by the following equation.

 CO₃²⁻(aq) + H₂O(l)  → HCO₃⁻(aq) + OH⁻ (aq)          

 K_b = = 2.1 × 10⁻⁴

The student decides to first determine [OH⁻] in the solution, then use that result to calculate the initial concentration of CO₃²⁻(aq).

i) Identify a laboratory method (not titration) that the student could use to collect data to determine [OH⁻] in the solution.

ii) Explain how the student could use the measured value in part (f)(i) to calculate the initial concentration of CO₃²⁻(aq). (Do not do any numerical calculations.)

In the original Na₂CO₃ solution at equilibrium, is the concentration of HCO₃⁻(aq) greater than, less than, or equal to the concentration of CO₃²⁻(aq) ? Justify your answer.

The student needs to make a CO₃²⁻ / HCO₃⁻ buffer. Is the Na₂CO₃ solution suitable for making a buffer with a pH of 6 ? Explain why or why not.

A 0.0200 M solution of barium hydroxide (Ba(OH)₂ is prepared at 25°C.

Write the dissociation equation for Ba(OH)₂ in water and explain how it differs from monoprotic bases.

Calculate the hydroxide ion concentration in the solution. Justify your calculation based on stoichiometry.

Determine the pH of the solution at 25 °C. Show all work with correct significant figures.

If the concentration of Ba(OH)₂ is doubled, determine the effect on the pH of the solution. Justify your answer with appropriate calculations. Show all work.

At 25 °C, the ionization constant of water, K_w​, is 1.00×10⁻¹⁴. At 50 °C, the value of K_w increases to 5.47 x 10⁻¹⁴.

Calculate the pH and pOH of pure water at 50°C. Show all working.

A student claims that since pH is lower at higher temperatures, water becomes acidic. Evaluate this claim and justify your answer using equilibrium principles and the relationship between pH and pOH.