Chemistry 8,9,10,11

A flask contains two compartments (A and B) with equal volumes of solution separated by a semipermeable membrane. Which diagram represents the final level of the liquids if A is initially a 10% (w/v) glucose solution and B is initially a 20% (w/v) glucose solution? A Picture B Picture C Picture

A

A particular wine contains 11.2% (v/v) ethanol. What volume of ethanol is in a 750.-mL bottle of this wine? A 84.0 mL ethanol B 0.840 mL ethanol C 6.70 mL ethanol D 14.9 mL ethanol

A

An unknown amount of water is added to 75 mL of a 3.5 M aqueous glucose solution. What can be said about the concentration of the resulting solution? A The concentration of the resultant glucose solution will be less than 3.5 M. B The concentration of the resultant glucose solution will be greater than 3.5 M. C The concentration of the resultant glucose solution will remain the same because the amount of glucose has not changed. D It is impossible to say anything about the concentration of the resultant glucose solution because the amount of added water has not been provided.

A

An unknown amount of water is added to 75 mL of a 3.5 M aqueous glucose solution. What can be said about the concentration of the resulting solution? A The concentration of the resultant glucose solution will be less than 3.5 M. B The concentration of the resultant glucose solution will be greater than 3.5 M. C The concentration of the resultant glucose solution will remain the same because the amount of glucose has not changed. D It is impossible to say anything about the concentration of the resultant glucose solution because the amount of added water has not been provided. References

A

Henry's law states that the solubility of a gas in a liquid is proportional to the A partial pressure of the gas above the liquid. B temperature of the liquid. C temperature of the gas above the liquid. D molecular weight of the gas above the liquid.

A

How many milliliters of a 5.25% (w/v) HCl solution must be used to prepare 250 mL of a 0.175% (w/v) HCl solution? A 8.3 mL HCl solution B 7,500 mL HCl solution C 230 mL HCl solution D 240 mL HCl solution E 8.6 mL HCl solution

A

Magnesium hydroxide can be made by the reaction shown below. If a chemist requires 0.725 moles of NaOH for this reaction, what volume of a 1.50 M NaOH solution is needed to provide this amount? A MgCl2(aq) + 2 NaOH(aq) → Mg(OH)2(s) + 2 NaCl(aq) B 0.483 L of a 1.50 M NaOH solution C 0.967 L of a 1.50 M NaOH solution D 1.09 L of a 1.50 M NaOH solution E 967 mL of a 1.50 M NaOH solution

A

The maximum level of lead allowed in drinking water is 15 mg/kg. What is this concentration in units of parts per million? rev: 10_28_2017_QC_CS-107432 A 15 ppm B 1.5 × 10-2 ppm C 1.5 × 104 ppm D 3.1 ppm

A

The pH of a lime is 1.90. What is the [H3O+]? A 1.3 × 10-2 M H3O+ B 1.3 × 1012 M H3O+ C 7.9 × 101 M H3O+ D 7.9 × 10-13 M H3O+ E 1.9 M H3O+

A

Which of the following statements concerning a solution is NOT true? A A solution is a heterogeneous mixture of two or more pure substances. B A solution is composed of a solvent and one or more solutes; the solute(s) dissolve in the solvent. C A solution has its components uniformly distributed. D A solution is likely to form when the solute(s) and the solvent have similar polarities.

A

Which pair of compounds will form a solution? A Benzene (C6H6) and hexane (C6H14) B Na2SO4 and benzene (C6H6) C NaCl and hexane (C6H14) D H2O and CCl4 E More than one of the combinations above will form solutions.

A

Which solution contains the smallest number of moles of sucrose (C12H22O11, molar mass = 342.30 g/mol)? A 2,000 mL of a 5.0 × 10-5% (w/v) sucrose solution B 2,000 mL of a 5.0 ppm sucrose solution C 20 mL of a 5.0 M sucrose solution D All of the solutions contain the same number of moles of sucrose.

A

Which solution has the lowest pH? A 1.3 × 10-8 M -OH B 1.0 × 10-7 M -OH C 5.1 × 10-2 M -OH D 3.9 × 10-8 M -OH E 2.3 × 10-3 M -OH

A

Which species can act as a Brønsted-Lowry base? A CO32- B HBr C H2CO3 D NH4+

A

Which substance is a colloid? A mayonnaise B a dental filling C mint chocolate chip ice cream D gasoline

A

A hypotonic solution has _____ osmotic pressure than/as body fluids. A a higher B a lower C the same

B

A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v) NaCl in water. What volume of the saline solution must be administered to the patient in order to deliver 7.7 g of NaCl? A 8.4 mL of saline solution B 840 mL of saline solution C 7.1 mL of saline solution D 140 mL of saline solution

B

A sample of seawater contains 1.3 g of calcium ions in 3,100 kg of solution. What is the calcium ion concentration of this solution in units of ppm? A 4.2 × 10-4 ppm Ca2+ ions B 0.42 ppm Ca2+ ions C 420 ppm Ca2+ ions D 4.0 ppm Ca2+ ions E 4.0 × 103 ppm Ca2+ ions

B

A sample of urine has a pH of 8.2. Which statement describing the urine sample is NOT true? A The urine sample is basic. B The urine sample has a hydronium ion concentration greater than that of a neutral solution. C The urine sample has a hydroxide ion concentration greater than its hydronium ion concentration. D The urine sample has a hydroxide ion concentration greater than 1.0 × 10-7.

B

A sample of water from the Chesapeake Bay has [H3O+]=3.1 × 10-9 M. Which statement below accurately describes this water sample? A The pH of the water sample is 7.5. B The water sample is a basic solution. C The water sample doesn't contain any hydroxide ions. D The water sample has a higher concentration of hydronium ions than pure water does.

B

How many grams of glucose (C6H12O6) are contained in 555 mL of a 1.77 M glucose solution? A 0.982 g C6H12O6 B 177 g C6H12O6 C 0.555 g C6H12O6 D 0.177 g C6H12O6

B

If cells are placed in a hypertonic solution, A water diffuses out of the cells and the cells shrink in a process called hemolysis. B water diffuses out of the cells and the cells shrink in a process called crenation. C water diffuses into the cells and the cells swell and eventually burst in a process called hemolysis. D water diffuses into the cells and the cells swell and eventually burst in a process called crenation.

B

In the acid-base reaction: F-(aq) + HNO3(aq) Picture HF(aq) + NO3-(aq) A F- is the acid and its conjugate base is HF, and HNO3 is the base and its conjugate acid is NO3-(aq). B HNO3 is the acid and its conjugate base is NO3-(aq), and F- is the base and its conjugate acid is HF. C F- is the acid and its conjugate base is NO3-(aq), and HNO3 is the base and its conjugate acid is HF. D HNO3 is the acid and its conjugate base is HF, and F- is the base and its conjugate acid is NO3-(aq).

B

The attraction of an ion with a dipole in a molecule is called A a dipole-dipole interaction. B an ion-dipole interaction. C hydrogen bonding. D London dispersion forces. E van der Waals forces.

B

The pH of normal blood is 7.4. The pH of a diabetic's blood was determined to be 6.4. Which comparison of these two blood samples is accurate? A The diabetic's blood has a lower [H3O+] than normal blood. B The diabetic's blood is more acidic than normal blood. C Normal blood has a lower [OH-] than the diabetic's blood. D Normal blood has a higher [H3O+] than the diabetic's blood.

B

What interactions are responsible for holding dissolved Cl- ions in an aqueous solution? A ion-ion attractions between K+ and Cl- ions B ion-dipole attractions between Cl- ions and the hydrogen atoms of water C ion-dipole attractions between Cl- ions and the oxygen atom of water D hydrogen bonding between the Cl- ions and water

B

What is the concentration of a solution formed by diluting 25.0 mL of a 3.2 M NaCl solution to 135.0 mL? A 17 M NaCl B 0.59 M NaCl C 0.50 M NaCl D 2.7 M NaCl

B

What is the molarity of a 11.5% (w/v) glucose (C6H12O6, molar mass 180.16 g/mol) solution? A 0.0638 M B 0.638 M C 1.15 M D 1.76 M

B

Which acid has the strongest conjugate base? A Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10-2) B Hydrocyanic acid HCN (Ka = 4.9 × 10-10) C Hydrofluoric acid HF (Ka = 7.2 × 10-4) D Ammonium ion NH4+ (Ka = 5.6 × 10-10)

B

Which acid is the weakest? A Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10-2) B Hydrocyanic acid HCN (Ka = 4.9 × 10-10) C Hydrofluoric acid HF (Ka = 7.2 × 10-4) D Ammonium ion NH4+ (Ka = 5.6 × 10-10)

B

Which diagram properly depicts the dissolved species present in an aqueous solution of KOH? (water molecules are not shown) A Picture B Picture C Picture D Picture

B

Which ion is the strongest base? A Br- B F- C I- D NO3-

B

Which ionic compound is not soluble in water? A NaCl B AgCl C (NH4)2SO4 D Ca(CH3CO2)2

B

Which is not an example of a solution? A a dental filling B chicken noodle soup C gasoline D tap water

B

Which of the following statements concerning solution concentration is NOT true? A An unsaturated solution contains less than the maximum amount of solute that can be dissolved in the solvent. B A saturated solution contains more than 100 g of dissolved solute. C A solution can be made less concentrated by adding additional solvent. D The number of moles of solute present in exactly one liter of solution is referred to as the solution's molarity.

B

Which solution has the highest pH? A 4.3 × 10-8 M -OH B 1.0 × 10-7 M -OH C 5.1 × 10-2 M H3O+ D 1.9 × 10-8 M -OH E 1.0 × 10-2 M H3O+

B

Which solution has the lowest boiling point? A A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water. B A solution formed by dissolving 0.75 mol of glucose (C6H12O6) in 1.00 kg of water. C A solution formed by dissolving 0.75 mol of Ca(NO3)2 in 1.00 kg of water. D A solution formed by dissolving 0.75 mol of Na3PO4 in 1.00 kg of water. E All of the solutions described have the same boiling point.

B

Which species can act as a Brønsted-Lowry acid? A CO32- B HBr C Br2 D LiOH

B

Which species is the conjugate acid of HCO3-? A CO32- B H2CO3 C CO2 D H2O

B

Which term correctly describes the medical condition in which the pH of blood is greater than 7.45, and therefore the blood is more basic than normal? A respiratory alkalosis B alkalosis C respiratory acidosis D acidosis

B

A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v) NaCl in water. How many grams of NaCl are contained in 575 mL of this solution? A 53 g NaCl B 529 g NaCl C 5.3 g NaCl D 0.016 g NaCl E 1.6 g NaCl

C

A solution is made by dissolving 3.88 g of NaCl in enough water to make 67.8 mL of solution. What is the concentration of sodium chloride in units of weight/volume percent? A 5.41% (w/v) NaCl B 94.3% (w/v) NaCl C 5.72% (w/v) NaCl D 0.0572% (w/v) NaCl

C

A solution is made by mixing 569 mL of water and 238 mL ethanol. What is the concentration of ethanol in units of volume/volume percent? A 41.8% (v/v) ethanol B 0.418% (v/v) ethanol C 29.5% (v/v) ethanol D 0.295% (v/v) ethanol E 70.5% (v/v) ethanol

C

How many milliliters of 0.653 M NaOH are needed to neutralize 25.0 mL of a 1.02 M HBr solution? The neutralization reaction is: NaOH(aq) + HBr(aq) → H2O(l) + NaBr(aq) A 16.0 mL NaOH B 25.5 mL NaOH C 39.1 mL NaOH D 16.3 mL NaOH

C

Normal gastric juice has a pH of about 2. Assuming that normal gastric juice is primarily aqueous HCl, what is the concentration of HCl in the stomach? A 2 M HCl B 1.0 × 102 M HCl C 0.01 M HCl D 0.14 M HCl

C

What is the conjugate base of the hydronium ion, H3O+? A OH- B H2O- C H2O D H3O+ has no conjugate base

C

What is the maximum volume of a 0.788 M CaCl2 solution that can be prepared using 85.3 g CaCl2? A 1.00 L B 0.769 L C 0.975 L D 67.2 L

C

What is the molarity of a solution made by dissolving 3.09 moles of NaCl in 1.50 L of solution? A 4.64 M NaCl B 4.85 M NaCl C 2.06 M NaCl D 0.673 M NaCl

C

What is the molarity of a solution made by dissolving 36.29 g of NaCl in 2.30 L of solution? A 15.78 M NaCl B 0.0634 M NaCl C 0.270 M NaCl D 2.70 M NaCl

C

What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (Ka = 1.8 × 10-5)? A 4.74 B 7.00 C 4.57 D 4.92

C

What is the pH of a cleaning solution with a [H3O+] = 7.4 × 10-9 M H3O+? A 5.9 B 7.13 C 8.13 D 5.87

C

What is the pH of a peach with a [-OH] = 3.2 × 10-11 M -OH? A 11.32 B 10.49 D 3.51 E 3.2

C

Which buffer solution has the lowest pH (HF has Ka = 7.2 × 10-4)? A 0.10 M HF and 0.10 M NaF B 0.20 M HF and 0.20 M NaF C 0.20 M HF and 0.10 M NaF D 0.10 M HF and 0.20 M NaF E All of the buffer solutions described have the same pH.

C

Which compound is a weak acid? A HNO3 B HBr C CH3COOH D H2SO4

C

Which solution containing an equal number of moles of each of the substances is a buffer? A HCl and NaCl B HNO2 and HNO3 C CH3COOH and NaCH3COO D H2CO3 and CO32- E More than one of the solutions is a buffer.

C

Which solution has the greatest mass of solute? A 2.00 L of a 0.75 M NaCl solution B 2.00 L of a 0.75 M CaCl2 solution C 2.00 L of a 0.75 M Ca(NO3)2 solution D 2.00 L of a 0.75 M Na2CO3 solution E All of the solutions have the same mass of solute.

C

Which solution has the highest freezing point? A A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water. B A solution formed by dissolving 0.25 mol of KCl in 1.00 kg of water. C A solution formed by dissolving 0.75 mol of KCl in 4.00 kg of water. D A solution formed by dissolving 0.25 mol of KCl in 0.50 kg of water. E All of the solutions described have the same freezing point.

C

Which species is the conjugate base of NH3? A NH4+ B NH2 C NH2- D H2O E NH4OH

C

Which substance is a nonelectrolyte? A NaCl B (NH4)2SO4 C H2O2 D KOH

C

Which substance is a nonelectrolyte? A NaCl B (NH4)2SO4 C H2O2 D KOH

C

Ammonia, NH3, is an example of a A strong acid B strong base C weak acid D weak base

D

Nonpolar compounds are soluble in A ionic compounds. B electrolytes. C polar solvents. D nonpolar solvents.

D

The [-OH] in a sample of egg whites is 6.3 × 10-7 M. What is the [H3O+] in these egg whites? A 6.3 × 10-7 M H3O+ B 1.0 × 10-7 M H3O+ C 6.3 × 10-21 M H3O+ D 1.6 × 10-8 M H3O+ E 1.0 × 10-14 M H3O+

D

The [H3O+] in a cabernet sauvignon wine is 5.9 × 10-4 M. What is the [-OH] in this wine? A 5.9 × 10-4 M -OH B 1.0 × 10-7 M -OH C 5.9 × 10-18 M -OH D 1.7 × 10-11 M -OH E 1.0 × 10-14 M -OH

D

What is the molarity of a 25.0% (v/v) aqueous isopropyl alcohol solution? The density of isopropyl alcohol (C3H8O, molar mass 60.09 g/mol) is 0.786 g/mL. A 0.529 M B 1.18 M C 0.327 M D 3.27 M

D

What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution? A 0.0115 M KCl B 11.5 M KCl C 1.55 × 10-4 M KCl D 0.155 M KCl

D

What is the net ionic equation for the acid-base reaction of hydrobromic acid with sodium hydroxide? A NaOH(aq) + HBr(aq) → H2O(l) + NaBr(aq) B Na+(aq) + -OH(aq) + H+(aq) + Br-(aq) → H2O(l) + Na+(aq) + Br-(aq) C Na+(aq) + -OH(aq) + H+(aq) + Br-(aq) → H+(aq) + -OH(aq) + Na+(aq) + Br-(aq) D -OH(aq) + H+(aq) → H2O(l)

D

Which ionic compound is soluble in water? A PbBr2 B Fe(OH)3 C BaSO4 D Ca(NO3)2 E More than one of the ionic compounds is soluble in water.

D

Which salt forms a basic solution when dissolved in water? A KCl B NH4Br C LiNO3 D Na3PO4

D

Which salt forms a solution with a pH < 7 when dissolved in water? A RbI B NaCH3COO C LiNO2 D (NH4)2SO4

D

Which solution has the highest boiling point? A A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water. B A solution formed by dissolving 0.75 mol of glucose (C6H12O6) in 1.00 kg of water. C A solution formed by dissolving 0.75 mol of Ca(NO3)2 in 1.00 kg of water. D A solution formed by dissolving 0.75 mol of Na3PO4 in 1.00 kg of water. E All of the solutions described have the same boiling point.

D

Which species is a diprotic acid? A Mg(OH)2 B CH3COOH C H2 D H2CO3

D

An aqueous solution with a low pH is necessary for a certain industrial process. Which of the following solutions would have the lowest pH? A 2.0 M NaOH B 0.5 M HCl C 1.0 M acetic acid, CH3COOH D 0.15 M NaOH E 1.0 M HCl

E