chemistry chapter 17.3-4-5

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10⁻⁵.

13.48

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10⁻⁴.

2.99

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10⁻⁵.

4.75

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10⁻⁵.

4.754

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10⁻⁵.

9.075

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10⁻⁵. A) 2.83 B) 1.5 × 10⁻³ C) 4.82 D) 4.00 E) 1.0 × 10⁴

A

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO₂) and 0.290 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4.50 × 10⁻⁴. A) 3.487 B) 3.210 C) 13.86 D) 10.51 E) 4.562

A

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO₂) and 0.205 M in formic acid (HCO₂H). The Ka of formic acid is 1.77 × 10⁻⁴. A) 3.910 B) 3.587 C) 13.84 D) 10.10 E) 4.963

A

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 8.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M. A) 0.0979 B) 0.0930 C) 0.129 D) 0.123 E) 0.00976

A

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point? A) 21.2 B) 0.245 C) 3.92 D) 0.153 E) 29.5

A

The pH of a solution that contains 0.818 M acetic acid (Ka = 1.76 × 10⁻⁵) and 0.182 M sodium acetate is __________. A) 4.102 B) 5.407 C) 8.593 D) 8.370 E) 9.898

A

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10⁻⁸. A) 2.54 B) 11.47 C) 7.00 D) 7.51 E) 7.54

B

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺. When the concentration of F- exceeds __________ M, BaF₂ will precipitate. Neglect volume changes. For BaF₂, Ksp = 1.7 × 10⁻⁶. A) 5.9 × 10⁻⁵ B) 1.1 × 10⁻² C) 2.4 × 10⁻⁸ D) 2.7 × 10⁻³ E) 1.2 × 10⁻⁴

B

Calculate the pH of a solution prepared by dissolving 0.350 mol of benzoic acid (C₇H₅O₂H) and 0.250 mol of sodium benzoate (NaC₇H₅O₂) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10⁻⁵. A) 4.333 B) 4.041 C) 9.959 D) 9.667 E) 5.190

B

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO₂). The Ka of formic acid is 1.77 × 10⁻⁴. A) 37.8 B) 0.0937 C) 11.3 D) 1.06 × 10⁻³ E) 3.529

B

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂) and 0.278 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4.50 × 10⁻⁴. A) 55.6 B) 0.162 C) 15.5 D) 2.78 × 10⁻³ E) 3.448

B

The Kb of ammonia is 1.76 × 10⁻⁵. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 50.0 mL of 1.00 M ammonium nitrate is __________. A) 4.632 B) 9.246 C) 4.742 D) 9.372 E) none of the above

B

A 25.0 mL sample of 0.723 M HClO₄ is titrated with a 0.273 M KOH solution. The H₃O⁺ concentration after the addition of 60.0 mL of KOH is __________ M. A) 0.0181 B) 0.430 C) 0.0200 D) 0.273 E) none of the above

C

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 25.3 mL of base. The concentration of HCl is __________ M. A) 11.7 B) 0.00352 C) 0.141 D) 0.0352 E) 0.139

C

A solution is prepared by dissolving 0.23 mol of hydrofluoric acid and 0.27 mol of sodium fluoride in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the __________ present in the buffer solution. The Ka of hydrofluoric acid is 1.36 × 10⁻³. A) H₂O B) H₃O⁺ C) fluoride ion D) hydrofluoric acid E) This is a buffer solution: the pH does not change upon addition of acid or base.

C

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO₂H) and 0.230 mol of sodium formate (NaCO₂H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10⁻⁴. A) 2.099 B) 10.318 C) 3.682 D) 2.307 E) 3.952

C

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH₃ and 0.350 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10⁻⁵. A) 5.137 B) 4.367 C) 9.633 D) 8.781 E) 8.863

C

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10⁻⁴. A) 3.94 × 10⁻⁵ B) 0.0180 C) 2.84 D) 0.280 E) 12.2

C

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10⁻⁴. A) 1.12 × 10⁻⁴ B) 0.0450 C) 4.25 D) 0.342 E) 5.53

C

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The Ka of butanoic acid is 1.5 × 10⁻⁵. A) 4.90 B) 50.0 C) 41.6 D) 60.1 E) 4.65

C

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 26.6 mL of the base is added. The concentration of acetic acid in the sample was __________ M. A) 0.365 B) 0.175 C) 0.119 D) 0.186 E) none of the above

D

A 25.0-mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hydrazoic acid is 1.9 × 10⁻⁵. A) 4.45 B) 1.34 C) 3.03 D) 4.78 E) 4.66

D

A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the __________ present in the buffer solution. The Ka of hydrazoic acid is 1.9 × 10⁻⁵. A) H₂O B) H₃O⁺ C) azide D) hydrazoic acid E) This is a buffer solution: the pH does not change upon addition of acid or base.

D

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 4.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M. A) 0.0862 B) 0.0876 C) 0.0980 D) 0.0848 E) 0.00253

D

The Ka of acetic acid is 1.76 × 10⁻⁵. The pH of a buffer prepared by combining 45.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is __________. A) 1.705 B) 0.851 C) 3.406 D) 4.709 E) 2.383

D

The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 25.0 mL of 0.145 M HCl is __________. A) 1.314 B) 1.181 C) 0.00824 D) 12.819 E) 12.923

D

The pH of a solution prepared by mixing 55.0 mL of 0.183 M KOH and 30.0 mL of 0.145 M HC₂H₃O₂ is __________. A) 9.97 B) 7.74 C) 1.172 D) 12.828 E) none of the above

D

What is the molar solubility of silver sulfate (Ag₂SO₄) in water? The solubility-product constant for Ag₂SO₄ is 1.5 × 10⁻⁵ at 25°C. A) 1.9 × 10⁻³ B) 2.5 × 10-⁻² C) 5.5 × 10⁻³ D) 1.6 × 10⁻² E) 5.0 × 10⁻⁶

D

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10⁻⁴. A) 14.28 B) 10.43 C) 5.48 D) 3.57 E) 4.13

D

A 25.0 mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of hydrazoic acid is 4.50 × 10⁻⁴. A) 11.72 B) 9.28 C) 4.72 D) 7.00 E) 8.80

E

In which aqueous system is Pbl₂ least soluble? A) H₂O B) 0.5 M HI C) 0.2 M HI D) 1.0 M HNO₃ E) 0.8 M KI

E

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10⁻¹⁰ at 25°C. A) 9.0 × 10⁻¹¹ B) 3.6 × 10⁻¹⁰ C) 9.74 D) 1.9 × 10⁻⁵ E) 1.3 × 10⁻⁵

E

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO) and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10⁻⁸. A) 13.88 B) 6.46 C) 8.49 D) 7.30 E) 7.54

E

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

FALSE

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

FALSE

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

FALSE

__________ analysis determines only the presence or absence of a particular metal ion, whereas __________ analysis determines how much of a given substance is present.

Qualitative, quantitative

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

TRUE

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

TRUE

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of __________.

acid

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be __________.

amphoteric

An assembly of a metal ion and the Lewis bases bonded to it is called a __________.

complex ion.

In general, the solubility of a slightly soluble salt is __________ by the presence of a second solute that furnishes a common ion.

decreased