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18. Aqueous Equilibrium

Intro to Buffers

18. Aqueous Equilibrium

Intro to Buffers

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Acid-Base Buffers

Acid-Base Buffers

Buffer Creation

Buffer Creation

Intro to Buffers Example

Intro to Buffers Example

Buffer Capacity

Buffer Capacity

Intro to Buffers Example

Intro to Buffers Example

Intro to Buffers Example

Intro to Buffers Example

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Calculating the pH of a Buffer

Calculating the pH of a Buffer

Practice Problem: Henderson-Hasselbalch Equation Calculations

Practice Problem: Henderson-Hasselbalch Equation Calculations

Professor Dave Explains

Derive the Henderson-Hasselblach Equation

Derive the Henderson-Hasselblach Equation

Henderson-Hasselbalch Equation

Henderson-Hasselbalch Equation

Chemistry with Dr. T

Buffer Solutions

Buffer Solutions

The Organic Chemistry Tutor

Buffer solution pH calculations | Chemistry | Khan Academy

Buffer solution pH calculations | Chemistry | Khan Academy

Khan Academy Organic Chemistry

00π productions

Buffers, the Acid Rain Slayer: Crash Course Chemistry #31

Buffers, the Acid Rain Slayer: Crash Course Chemistry #31

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Practice this topic

Multiple Choice

Which one of the following combinations does not create a buffer?

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Multiple Choice

Which of the following combinations can result in the formation of a buffer?

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Multiple Choice

Which of the following combinations can result in the formation of a buffer?

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Multiple Choice

A buffer solution is comprised of 50.0 mL of a 0.100 M HC₂H₃O₂ and 60.0 mL of a 0.100 M NaC₂H₃O₂. Which of the following actions would completely destroy the buffer?

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Multiple Choice

Calculate the pH of a solution formed by mixing 200 mL of a 0.400 M C₂H₅NH₂ solution with 350 mL of a 0.450 M C₂H₅NH₃⁺solution. (K_b of C₂H₅NH₂is 5.6 x 10 ^-4).

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Multiple Choice

Determine how many grams of sodium acetate, NaCH₃CO₂ (MW:82.05 g/mol), you would mix into enough 0.065 M acetic acid CH₃CO₂H (MW:60.05 g/mol) to prepare 3.2 L of a buffer with a pH of 4.58. The K_a is 1.8 x 10^-5.

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Multiple Choice

A buffer solution is made by combining a weak acid with its conjugate salt. What will happen to the pH if the solution is diluted to one-fourth of its original concentration?

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Multiple Choice

Which of the following statements is true about a solution prepared with equal amounts of HNO₂ and NaNO₂?

Multiple Choice

The addition of which of the following would destroy a 1.0 L buffer that is 0.50 M HC₂H₃O₂ and 0.40 M NaC₂H₃O₂?

Multiple Choice

Which of the following would produce a buffer?

Multiple Choice

What is the pH of a 1.0 L buffer solution containing 0.500 M HF and 0.300 M NaF. K_a for HF = 3.5 × 10⁻⁴.

Multiple Choice

Determine the pH of a 1.0 L buffer prepared by adding 0.100 moles of NaOH to 0.250 moles of HF. K_a for HF = 3.5 × 10⁻⁴.

Multiple Choice

What mass of NaC₂H₃O₂ (molar mass = 82.03 g/mol) would need to be added to 0.450 moles of HC₂H₃O₂ to prepare a 1.0 L buffer with a pH = 4.95. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

Multiple Choice

1.0 L of a buffer is prepared to produce a solution that is 0.400 M in HF and 0.250 M in LiF. What is the pH after the addition of 2.5 g of KOH? Assume no volume change.
K_a for HF = 3.5 × 10⁻⁴.

Multiple Choice

Which pairs of compounds are capable of making a buffer? Select all that apply.

a) 1.3 M LiOH and 1.7 M HCOOH c) 0.35 M CH₃CO₂H and 0.35 M NaOH

b) 0.784 M NH₄⁺ and 0.800 M HClO₄ d) 0.80 HNO₃ and 0.15 MgO

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Multiple Choice

Determine which of the following actions will destroy a buffer composed of 0.50 L of 1.44 M H₃PO₄ and 0.60 L of 1.25 M NaH₂PO₄⁻.

a) Addition of 1.45 moles of KH₂PO₄

b) Addition of 0.85 moles of HCl

c) Addition of water

d) Addition of 0.30 moles of Ca(OH)₂

e) Addition of 0.70 moles of HIO₄

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A buffer resists change in ph when ___________ amount of acid or base is added to it.

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Textbook Question

The beaker on the right contains 0.1 M acetic acid solution with methyl orange as an indicator. The beaker on the left contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate with methyl orange. (b) Which solution is better able to maintain its pH when small amounts of NaOH are added? Explain. [Sections 17.1 and 17.2]

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Textbook Question

The following diagram represents a buffer composed of equal concentrations of a weak acid, HA, and its conjugate base, A-. The heights of the columns are proportional to the concentrations of the components of the buffer. (c) Which of the three represents a situation that cannot arise from the addition of either an acid or a base? [Section 17.2]

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Textbook Question

The following diagram represents a buffer composed of equal concentrations of a weak acid, HA, and its conjugate base, A-. The heights of the columns are proportional to the concentrations of the components of the buffer. (a) Which of the three drawings, (1), (2), or (3), represents the buffer after the addition of a strong acid? [Section 17.2]

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Textbook Question

What is the pH of a buffer solution prepared by dissolving 0.250 mol of NaH2PO4 and 0.075 mol of NaOH in enough water to make 1.00 L of solution? (Ka (H2PO4-) = 6.2 X 10^-8) (a) 6.32 (b) 6.83 (c) 7.21 (d) 7.71

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Textbook Question

Bars of iron are put into each of the three beakers as shown here. In which beaker—A, B, or C—would you expect the iron to show the most corrosion ? [Section 20.8]

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Textbook Question

A solution containing sulfide ions is added to a solution of 0.036 M Cu2+ and 0.044 M Fe2+. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? (a) 1.4 x 10^-16 M, FeS (b) 3.6 x 10^-35 M, CuS (c) 3.6 x 10^-35 M, FeS (d) 1.4 x 10^-16 M, C

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Textbook Question

Which of the following solutions is a buffer? (a) A solution made by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M NaOH, (b) a solution made by mixing 100 mL of 0.100 M CH3COOH and 500 mL of 0.100 M NaOH, (c) A solution made by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M HCl, (d) A solution made by mixing 100 mL of 0.100 M CH3COOK and 50 mL of 0.100 M KCl.

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Textbook Question

You have to prepare a pH = 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH3COOH, H3PO4, HCOONa, CH3COONa, and NaH2PO4. Which solutions would you use?

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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. Which solutions would you use?

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Textbook Question

A buffer contains significant amounts of acetic acid and sodium acetate. Write equations showing how this buffer neutralizes added acid and added base.

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Textbook Question

Consider the following table of standard reduction potentials:

(b) Which substances can be oxidized by B2+? Which can be reduced by D?

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Textbook Question

A buffer contains significant amounts of ammonia and ammonium chloride. Write equations showing how this buffer neutralizes added acid and added base.

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Textbook Question

The following pictures represent solutions that contain one or more of the compounds H2A, NaHA, and Na2A, where H2A is a weak diprotic acid. (Na+ ions and solvent water molecules have been omitted for clarity.)

(b) Which solution has the greatest buffer capacity?

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Textbook Question

The following pictures represent solutions that contain one or more of the compounds H2A, NaHA, and Na2A, where H2A is a weak diprotic acid. (Na+ ions and solvent water molecules have been omitted for clarity.)

(a) Which of the solutions are buffer solutions?

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Textbook Question

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

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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

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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

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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

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Textbook Question

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 100.0 mL of 0.10 M NH3; 100.0 mL of 0.15 M NH4Cl

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Textbook Question

Determine whether or not the mixing of each pair of solutions results in a buffer. e. 105.0 mL of 0.15 M CH3NH2; 95.0 mL of 0.10 M HCl

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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

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Textbook Question

Determine whether or not the mixing of each pair of solutions results in a buffer. b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl

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Textbook Question

The fluids within cells are buffered by H2PO4- and HPO42 - . b. Could a buffer system employing H3PO4 as the weak acid and H2PO4- as the weak base be used as a buffer system within cells? Explain.

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Textbook Question

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. d. 1.35 g HI

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Textbook Question

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH

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Textbook Question

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. c. 1.25 g HBr

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Textbook Question

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. a. 250 mg NaOH

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Textbook Question

Which of the following gives a buffer solution when equal volumes of the two solutions are mixed? (a) 0.10 M NH3 and 0.10 M HCl (b) 0.20 M NH3 and 0.10 M HCl (c) 0.10 M NH4Cl and 0.10 M NH3 (d) 0.20 M NH4Cl and 0.10 M NaOH

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Textbook Question

Which of the following solutions has the greater buffer capacity: 100 mL of 0.30 M HNO2-0.30 M NaNO2 or 100 mL of 0.10 M HNO2-0.10 M NaNO2? Explain.

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Textbook Question

You need a buffer solution that has pH = 7.00. Which of the following buffer systems should you choose? Explain. (a) H3PO4 and H2PO4 - (b) H2PO4- and HPO42- (c) HPO42- and PO43-

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Textbook Question

Consider a buffer solution that contains equal concentrations of H2PO4- and HPO42-. Will the pH increase, decrease, or remain the same when each of the following substances is added? (a) Na2HPO4 (b) HBr (c) KOH (d) KI (e) H3PO4 (f) Na3PO4

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Textbook Question

Two buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and sodium formate (HCOONa) to enough water to make 1.00 L of solution. Buffer A is prepared using 1.00 mol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 mol of each. (b) Which buffer will have the greater buffer capacity?

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Textbook Question

Consider a galvanic cell that utilizes the following half-reactions: (d) Will AgCl precipitate if 10.0 mL of 0.200 M NaCl is added to the solution in part (c)? Will AgBr precipitate if 10.0 mL of 0.200 M KBr is added to the resulting solution?

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Which of the following solutions represents a good buffer system?

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A solution that resists a change in ph when an acid or base is added to it is a(n) __________.

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Select the statement that best describes a buffer. see concept 3.3 (page)

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A(n) is a substance or a mixture of substances that act to resist changes in pH.

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Which of the following is a means of creating a buffer of H₂CO₃/NaHCO₃₃?

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Which of the following solutions is a good buffer system?

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Which of the following aqueous solutions are good buffer systems?

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