A 0.10 M solution of hydrazine (N2H4, K b = 1.7×10 - 6) containing an unknown concentration of hydrazine hydrochloride (N2H5Cl) has a pH of 7.50. What is the concentration of N2H5Cl in the solution?

A) 1.26 M B) 0.54 M C) 5.8 M D) 0.10 M E) 0.72 M A) 1.26 M B) 0.54 M C) 5.8 M D) 0.10 M E) 0.72 M

Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH4Cl in 1.00 L of 0.15 M NH3. K b = 1.8×10 - 5 for NH3.

A) 9.43 B) 4.56 C) 11.34 D) 2.72 E) 4.74 A) 9.43 B) 4.56 C) 11.34 D) 2.72 E) 4.74

What is the volume of 0.0175 M Ba(OH)2 required to neutralize 10.0 mL of 0.0300 M HCl?

A) 10.0 mL B) 34.2 mL C) 17.1 mL D) 8.6 mL E) 4.3 mL A) 10.0 mL B) 34.2 mL C) 17.1 mL D) 8.6 mL E) 4.3 mL

A buffer was prepared such that the pH was 5.20. If the solution contains 0.400 moles of acetic acid (CH3COOH) per liter, what is the concentration of the acetate ion (CH3COO - ) in this solution? The p K a for acetic acid is 4.74.

A) 0.40 M B) 0.14 M C) 4.2×10 - 3 M D) 6.3×10 - 6 M E) 1.1 M A) 0.40 M B) 0.14 M C) 4.2×10 - 3 M D) 6.3×10 - 6 M E) 1.1 M

Calculate the pH of a solution formed when 1.5 L oF4.5×10 - 3 M HCl is mixed witH₂ .0 L of 3.0×10 - 3 M HNO3.

A) 3.67 B) 3.74 C) 2.25 D) 3.16 E) 2.44 A) 3.67 B) 3.74 C) 2.25 D) 3.16 E) 2.44

Exam 16: Reactions Between Acids and Bases

In the titration of 25.0 mL of a solution of a weak acid HX with 0.250 M NaOH, the pH = 4.50 after the addition of 5.0 mL of the NaOH solution. The equivalence point occurs when 30.4 mL of the NaOH solution has been added. What is the ionization constant ( K _a) of HX?

(Multiple Choice)

4.8/5

(43)

Question 21

Carbonic acid is a diprotic acid with K _al = 4.3×10^{- 7} and K _a2 = 5.6×10^{- 11}. Estimate the pH of a solution of sodium hydrogen carbonate.

(Multiple Choice)

4.8/5

(49)

Question 22

Solutions are made by combining equal amounts of the following. Which is a buffer?

(Multiple Choice)

4.9/5

(46)

Question 23

Exhibit 16-1 Consider the equilibrium reaction below to answer the following question(s). HNO₂ + H₂ O H₃O + + NO₂ 1 - K a (HNO₂ ) = 4.5 10 - 4 -Refer to Exhibit 16-1. What is the concentration of nitrite ion, NO₂ - , present at equilibrium if 0.100 moles of HCl are added to 0.200 moles of HNO₂ to form one-liter of solution?

(Multiple Choice)

4.9/5

(32)

Question 24

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Ag₂S II. Mg₃(PO₄)₂ III. AgBr

(Multiple Choice)

4.9/5

(36)

Question 25

Oxalic acid is diprotic with p K _al = 1.23 and p K _a2 = 4.19. What is p K _b for the hydrogen oxalate ion?

(Multiple Choice)

4.8/5

(35)

Question 26

Which of the following titrations would produce a pH equal to 7.0 at the equivalence point? I. Titrating NH₃ with standard HCl (delivered from the burette) II. Titrating HCl with standard NaOH (delivered from the burette) III. Titrating CH₃COOH with standard NaOH (delivered from the burette)

(Multiple Choice)

4.8/5

(37)

Question 27

A 0.10 M solution of hydrazine (N₂H₄, K _b = 1.7×10^{- 6}) containing an unknown concentration of hydrazine hydrochloride (N₂H₅Cl) has a pH of 7.50. What is the concentration of N₂H₅Cl in the solution?

(Multiple Choice)

4.9/5

(41)

Question 28

Which of the following general combinations of substances form an acid-base buffer when added to water?

(Multiple Choice)

4.7/5

(47)

Question 29

Consider a buffer solution containing a weak acid, HX, and a salt of the weak acid's conjugate base, NaX. Under what conditions is the pH greater than the p K _a of the weak acid?

(Multiple Choice)

4.9/5

(32)

Question 30

A sample of acetic acid (approximately 0.001 M, K _a = 1.8×10^{- 5}) is titrated with 0.00993 M NaOH. What indicator should be used?

(Multiple Choice)

4.7/5

(41)

Question 31

Consider the two buffer solutions prepared below: Solution A: [HA] = 0.15 M and [A^-] = 0.25 M Solution B: [HA] = 1.50 M and [A^-] = 2.50 M Which statement below is true regarding the pH and buffering capacity of these two solutions?

(Multiple Choice)

4.9/5

(37)

Question 32

Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH₄Cl in 1.00 L of 0.15 M NH₃. K _b = 1.8×10^{- 5} for NH₃.

(Multiple Choice)

4.8/5

(45)

Question 33

What is the volume of 0.0175 M Ba(OH)₂ required to neutralize 10.0 mL of 0.0300 M HCl?

(Multiple Choice)

4.9/5

(33)

Question 34

A buffer was prepared such that the pH was 5.20. If the solution contains 0.400 moles of acetic acid (CH₃COOH) per liter, what is the concentration of the acetate ion (CH₃COO^-) in this solution? The p K _a for acetic acid is 4.74.

(Multiple Choice)

4.9/5

(44)

Question 35

Calculate the pH of a solution formed when 1.5 L oF₄.5×10^{- 3} M HCl is mixed witH₂ .0 L of 3.0×10^{- 3} M HNO₃.

(Multiple Choice)

4.9/5

(44)

Question 36

Which of the following mixtures would not be suitable for preparing a buffer solution?

(Multiple Choice)

4.7/5

(42)

Question 37

A sample of 0.100 mole of acetic acid ( K _a = 1.8×10^{- 5}) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 25.0 mL of the base?

(Multiple Choice)

4.9/5

(38)

Question 38

Consider the titration of a weak acid with a strong base . Which statement below is true regarding the equivalence point in this titration?

(Multiple Choice)

4.8/5

(45)

Question 39

What volume of 0.200 M H₂ SO₄is required to neutralize 50.0 mL of 0.100 M NaOH? Assume the chemical equation is: H₂ SO₄(aq) + 2 NaOH (aq) Na₂ SO₄(aq) + 2 H₂ O ( )

(Multiple Choice)

4.8/5

(29)

Question 40

Showing 21 - 40 of 98

Exam 16: Reactions Between Acids and Bases

In the titration of 25.0 mL of a solution of a weak acid HX with 0.250 M NaOH, the pH = 4.50 after the addition of 5.0 mL of the NaOH solution. The equivalence point occurs when 30.4 mL of the NaOH solution has been added. What is the ionization constant ( K a) of HX?

Carbonic acid is a diprotic acid with K al = 4.3×10 - 7 and K a2 = 5.6×10 - 11. Estimate the pH of a solution of sodium hydrogen carbonate.

Solutions are made by combining equal amounts of the following. Which is a buffer?

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Ag2S II. Mg3(PO4)2 III. AgBr

Oxalic acid is diprotic with p K al = 1.23 and p K a2 = 4.19. What is p K b for the hydrogen oxalate ion?

Which of the following titrations would produce a pH equal to 7.0 at the equivalence point? I. Titrating NH3 with standard HCl (delivered from the burette) II. Titrating HCl with standard NaOH (delivered from the burette) III. Titrating CH3COOH with standard NaOH (delivered from the burette)

A 0.10 M solution of hydrazine (N2H4, K b = 1.7×10 - 6) containing an unknown concentration of hydrazine hydrochloride (N2H5Cl) has a pH of 7.50. What is the concentration of N2H5Cl in the solution?

Which of the following general combinations of substances form an acid-base buffer when added to water?

Consider a buffer solution containing a weak acid, HX, and a salt of the weak acid's conjugate base, NaX. Under what conditions is the pH greater than the p K a of the weak acid?

A sample of acetic acid (approximately 0.001 M, K a = 1.8×10 - 5) is titrated with 0.00993 M NaOH. What indicator should be used?

Consider the two buffer solutions prepared below: Solution A: [HA] = 0.15 M and [A - ] = 0.25 M Solution B: [HA] = 1.50 M and [A - ] = 2.50 M Which statement below is true regarding the pH and buffering capacity of these two solutions?

Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH4Cl in 1.00 L of 0.15 M NH3. K b = 1.8×10 - 5 for NH3.

What is the volume of 0.0175 M Ba(OH)2 required to neutralize 10.0 mL of 0.0300 M HCl?

A buffer was prepared such that the pH was 5.20. If the solution contains 0.400 moles of acetic acid (CH3COOH) per liter, what is the concentration of the acetate ion (CH3COO - ) in this solution? The p K a for acetic acid is 4.74.

Calculate the pH of a solution formed when 1.5 L oF4.5×10 - 3 M HCl is mixed witH₂ .0 L of 3.0×10 - 3 M HNO3.

Which of the following mixtures would not be suitable for preparing a buffer solution?

A sample of 0.100 mole of acetic acid ( K a = 1.8×10 - 5) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 25.0 mL of the base?

Consider the titration of a weak acid with a strong base . Which statement below is true regarding the equivalence point in this titration?

What volume of 0.200 M H₂ SO₄is required to neutralize 50.0 mL of 0.100 M NaOH? Assume the chemical equation is: H₂ SO₄(aq) + 2 NaOH (aq) Na2 SO₄(aq) + 2 H₂ O ( )

Introduction to Chemistry

Atoms, Molecules, and Ions

Equations, the Mole, and Chemical Formulas

Chemical Reactions in Solution

Thermochemistry

The Gaseous State

Electronic Structure

The Periodic Table: Structure and Trends

Chemical Bonds

Molecular Structure and Bonding Theories

Liquids and Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Solutions of Acids and Bases

Chemical Thermodynamics

Electrochemistry

Transition Metals, Coordination Chemistry and Metallurgy

The Chemistry of Hydrogen, Elements in Groups 3A Through 6A, and the Noble Gases

Nuclear Chemistry

Organic Chemistry and Biochemistry

Filters

In the titration of 25.0 mL of a solution of a weak acid HX with 0.250 M NaOH, the pH = 4.50 after the addition of 5.0 mL of the NaOH solution. The equivalence point occurs when 30.4 mL of the NaOH solution has been added. What is the ionization constant ( K _a) of HX?

Carbonic acid is a diprotic acid with K _al = 4.3×10^{- 7} and K _a2 = 5.6×10^{- 11}. Estimate the pH of a solution of sodium hydrogen carbonate.

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Ag₂S II. Mg₃(PO₄)₂ III. AgBr

Oxalic acid is diprotic with p K _al = 1.23 and p K _a2 = 4.19. What is p K _b for the hydrogen oxalate ion?

Which of the following titrations would produce a pH equal to 7.0 at the equivalence point? I. Titrating NH₃ with standard HCl (delivered from the burette) II. Titrating HCl with standard NaOH (delivered from the burette) III. Titrating CH₃COOH with standard NaOH (delivered from the burette)

A 0.10 M solution of hydrazine (N₂H₄, K _b = 1.7×10^{- 6}) containing an unknown concentration of hydrazine hydrochloride (N₂H₅Cl) has a pH of 7.50. What is the concentration of N₂H₅Cl in the solution?

Consider a buffer solution containing a weak acid, HX, and a salt of the weak acid's conjugate base, NaX. Under what conditions is the pH greater than the p K _a of the weak acid?

A sample of acetic acid (approximately 0.001 M, K _a = 1.8×10^{- 5}) is titrated with 0.00993 M NaOH. What indicator should be used?

Consider the two buffer solutions prepared below: Solution A: [HA] = 0.15 M and [A^-] = 0.25 M Solution B: [HA] = 1.50 M and [A^-] = 2.50 M Which statement below is true regarding the pH and buffering capacity of these two solutions?

Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH₄Cl in 1.00 L of 0.15 M NH₃. K _b = 1.8×10^{- 5} for NH₃.

What is the volume of 0.0175 M Ba(OH)₂ required to neutralize 10.0 mL of 0.0300 M HCl?

A buffer was prepared such that the pH was 5.20. If the solution contains 0.400 moles of acetic acid (CH₃COOH) per liter, what is the concentration of the acetate ion (CH₃COO^-) in this solution? The p K _a for acetic acid is 4.74.

Calculate the pH of a solution formed when 1.5 L oF₄.5×10^{- 3} M HCl is mixed witH₂ .0 L of 3.0×10^{- 3} M HNO₃.

A sample of 0.100 mole of acetic acid ( K _a = 1.8×10^{- 5}) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 25.0 mL of the base?

What volume of 0.200 M H₂ SO₄is required to neutralize 50.0 mL of 0.100 M NaOH? Assume the chemical equation is: H₂ SO₄(aq) + 2 NaOH (aq) Na₂ SO₄(aq) + 2 H₂ O ( )