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18. Aqueous Equilibrium

Henderson-Hasselbalch Equation

18. Aqueous Equilibrium

Henderson-Hasselbalch Equation

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Henderson-Hasselbalch Equation

Henderson-Hasselbalch Equation

Henderson-Hasselbalch Equation Example

Henderson-Hasselbalch Equation Example

Calculating Buffer Range

Calculating Buffer Range

Henderson-Hasselbalch Equation Example

Henderson-Hasselbalch Equation Example

Practice this topic

Multiple Choice

The K_b of C₆H₅NH₂ (aniline) is 3.9 × 10⁻¹⁰. Determine pH of a buffer solution made up of 500 mL of 1.4 M C₆H₅NH₂ and 230 mL of 2.3 M C₆H₅NH₃⁺.

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Multiple Choice

Determine the buffer component concentration ratio (CB/WA) for a buffer with a pH of 4.7. K_a of boric acid (H₃BO₃) is 5.4 × 10⁻¹⁰.

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Multiple Choice

Calculate mass of NaN₃ that needs be added to 1.8 L of 0.35 M HN₃ in order to make a buffer with a pH of 6.5. K_a of hydrazoic acid is 1.9 × 10⁻⁵.

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Multiple Choice

Which of the following weak acid-conjugate base combinations would result in an ideal buffer solution with a pH of 9.4?

a) formic acid (HCHO₂) and sodium formate (K_a = 1.8 x 10^-4)

b) benzoic acid (HC₇H₅O₂) and potassium benzoate (K_a = 6.5 x 10^-5)

c) hydrocyanic acid (HCN) and lithium cyanide (K_a = 4.9 x 10^-10)

d) iodic acid (HIO₃) and sodium iodate (K_a = 1.7 x 10^-1)

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Textbook Question

Which of the following mixtures has the highest pH? (a) Equal volumes of 1.0 M HCl and 1.0 M NaOH (b) Equal volumes of 0.1 M HNO3 and 0.1 M KOH (c) Equal volumes of 0.1 M HCN and 0.1 M NaOH (d) Equal volumes of 0.1 M NaF and 0.1 M HCl

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Textbook Question

A buffer contains a weak acid, HA, and its conjugate base. The weak acid has a pKa of 4.5, and the buffer has a pH of 4.3. Without doing a calculation, state which of these possibilities are correct at pH 4.3. (a) 3HA4 = 3A-4, (b) 3HA4 7 3A-4, or (c) 3HA4 6 3A-4. [Section 17.2]

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Textbook Question

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. (Ka = 3.5 x 10^-4) (a) 4.11 (b) 3.82 (c) 3.46 (d) 3.09

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Textbook Question

(a) Calculate the pH of a buffer that is 0.12 M in lactic acid and 0.11 M in sodium lactate.

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Textbook Question

You are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and any amount you need of sodium fluoride (NaF). (b) How many grams of sodium fluoride should be added to prepare the buffer solution? Neglect the small volume change that occurs when the sodium fluoride is added.

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Textbook Question

You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid 1C6H5COOH2 and any amount you need of sodium benzoate 1C6H5COONa2. (b) How many grams of sodium benzoate should be added to prepare the buffer? Neglect the small volume change that occurs when the sodium benzoate is added.

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Textbook Question

A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (c) What is the pH of the buffer after the addition of 0.02 mol of HNO3?

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Textbook Question

A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (b) What is the pH of the buffer after the addition of 0.02 mol of KOH?

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Textbook Question

A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (a) What is the pH of this buffer?

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Textbook Question

(b) What is the ratio of HCO3 - to H2CO3 in an exhausted marathon runner whose blood pH is 7.1?

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Textbook Question

(a) What is the ratio of HCO3 - to H2CO3 in blood of pH 7.4?

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Textbook Question

You have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN, and NaCN. How many milliliters of each solution would you use to make approximately 1 L of the buffer?

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Textbook Question

Use the Henderson–Hasselbalch equation to calculate the pH of each solution in Problem 29.

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Textbook Question

Use the Henderson–Hasselbalch equation to calculate the pH of each solution. c. a solution that contains 10.0 g of HC2H3O2 and 10.0 g of NaC2H3O2 in 150.0 mL of solution

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Textbook Question

Calculate the pH of the solution that results from each mixture. a. 50.0 mL of 0.15 M HCHO2 with 75.0 mL of 0.13 M NaCHO2

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Textbook Question

Calculate the pH of the solution that results from each mixture. b. 125.0 mL of 0.10 M NH3 with 250.0 mL of 0.10 M NH4Cl

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Textbook Question

Calculate the ratio of NaF to HF required to create a buffer with pH = 4.00.

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Textbook Question

Calculate the ratio of CH3NH2 to CH3NH3Cl concentration required to create a buffer with pH = 10.24.

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Textbook Question

What mass of sodium benzoate should you add to 150.0 mL of a 0.15 M benzoic acid solution to obtain a buffer with a pH of 4.25? (Assume no volume change.)

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Textbook Question

A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. b. What is the pH after addition of 150.0 mg of HBr?

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Textbook Question

A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. a. What is the initial pH of this solution?

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Textbook Question

A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. c. What is the pH after addition of 85.0 mg of NaOH?

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Textbook Question

For each solution, calculate the initial and final pH after adding 0.010 mol of NaOH. c. 250.0 mL of a buffer solution that is 0.255 M in CH3CH2NH2 and 0.235 M in CH3CH2NH3Cl

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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?

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Textbook Question

Which buffer system is the best choice to create a buffer with pH = 9.00? For the best system, calculate the ratio of the masses of the buffer components required to make the buffer. HF/KF HNO2/KNO2 NH3/NH4Cl HClO/KClO

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Textbook Question

Calculate the pH of a buffer solution that is 0.20 M in HCN and 0.12 M in NaCN. Will the pH change if the solution is diluted by a factor of 2? Explain.

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Textbook Question

Calculate the pH of 0.375 L of a 0.18 M acetic acid–0.29 M sodium acetate buffer before and after the addition of (a) 0.0060 mol of KOH. Assume that the volume remains constant.

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Textbook Question

Use the Henderson–Hasselbalch equation to calculate the pH of a buffer solution that is 0.25 M in formic acid (HCO2H) and 0.50 M in sodium formate (HCO2Na).

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Textbook Question

The ratio of HCO3- to H2CO3 in blood is called the 'bicarb number' and is used as a measure of blood pH in hospital emergency rooms. A newly diagnosed diabetic patient is admitted to the emergency room with ketoacidosis and a bicarb number of 10. Calculate the blood pH. Ka for carbonic acid at room temperature (37 degrees Celsius) os 7.9 x 10^-7).

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Textbook Question

In what volume ratio should you mix 1.0 M solutions of NH4Cl and NH3 to produce a buffer solution having pH = 9.80?

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Textbook Question

Give a recipe for preparing a CH3CO2H-CH3CO2Na buffer solution that has pH = 4.44.

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Textbook Question

Derive an equation similar to the Henderson–Hasselbalch equation relating the pOH of a buffer to the pKb of its base component.

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Textbook Question

A 1.0-L buffer solution initially contains 0.25 mol of NH3 and 0.25 mol of NH4Cl. In order to adjust the buffer pH to 8.75, should you add NaOH or HCl to the buffer mixture? What mass of the correct reagent should you add?

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Textbook Question

What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that is buffered at a pH of 4.55 and has a freezing point of -2.0 °C? (Assume complete dissociation of sodium benzoate and a density of 1.01 g/mL for the solution.)

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Textbook Question

A 1.000 L sample of HCl gas at 25°C and 732.0 mm Hg was absorbed completely in an aqueous solution that contained 6.954 g of Na2CO3 and 250.0 g of water. (a) What is the pH of the solution?

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buffer 2: 50.0 mL of 0.18 M NH₃ with 5.0 mL of 0.36 M HBr.

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What is the pH of a solution of 0.300 M HNO₂ containing 0.100 M NaNO₂? (K_a of HNO₂ is 4.5 × 10^–4)

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What is the ratio of [A^–]/[HA] at pH 5.75? The pK_a of formic acid (methanoic acid, H–COOH) is 3.75.

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What ratio of NaCN to HCN is needed to prepare a pH 10.00 buffer? (K_a of HCN is 4.9 × 10^-10)

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How much more acetic acid (pK_a = 4.76) than acetate should be in solution to maintain a pH of 4.00?

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Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 m HBrO (K_a = 2.5 × 10^-9)

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