Deck 8: Solutions, Colloids and Membranes

Question 1

A vial contains 5 mL of 1% aqueous lidocaine, a dental anesthetic. In this solution,

A) both lidocaine and water are solutes.
B) both lidocaine and water are solvents.
C) lidocaine is the solute and water is the solvent.
D) lidocaine is the solvent and water is solute.
E) there are no solutes nor solvents in this solution.

Answer 1

lidocaine is the solute and water is the solvent.

Question 2

A solute dissolving in a solvent is a _______ because _______.

A) physical change; covalent bonds are broken in the process
B) chemical change; covalent bonds are broken in the process
C) chemical change; ionic attractions are broken in the process
D) physical change; covalent bonds are not broken in the process
E) chemical change; covalent bonds are not broken in the process

Answer 2

physical change; covalent bonds are not broken in the process

Question 3

A wine label states that it is 12 proof, meaning that it contains 6% ethanol. According to this information,

A) ethanol is a solute in wine and water is the solvent.
B) ethanol is a solvent in wine and water is the solute.
C) ethanol and water are both solvents in wine.
D) ethanol and water are both solutes in wine.
E) wine does not contain any solutes.

Answer 3

ethanol is a solute in wine and water is the solvent.

Question 4

Which of the following is a heterogeneous mixture?

A) vinegar
B) oil and vinegar salad dressing
C) lemonade
D) bronze
E) air

Question 5

The chart below illustrates the composition of air. According to this chart,

A) nitrogen and oxygen are solutes, while argon and carbon dioxide are solvents.
B) carbon dioxide is the only solute in air.
C) oxygen, argon, and carbon dioxide are solutes, while nitrogen is the solvent.
D) nitrogen is the solute, while oxygen, argon, and carbon dioxide are all solvents.
E) nitrogen, oxygen, argon, and carbon dioxide are all solutes in air.

Question 6

Table sugar is a

A) solution.
B) solvent.
C) element.
D) molecule.
E) suspension .

Question 7

In a solution, the component present in a larger amount is called the

A) solvent.
B) solute.
C) medium.
D) colloid.
E) solution.

Question 8

There are many mixtures in the body. The most common ______ for these mixtures is water.

A) solvent
B) solute
C) medium
D) colloid
E) solution

Question 9

Glucose in the blood is a

A) solution.
B) solvent.
C) homogenous mixture.
D) colloidal dispersion.
E) suspension.

Question 10

A _______ has components that are evenly distributed throughout the mixture.

A) homogenous mixture
B) heterogeneous mixture
C) pure compound
D) solute
E) solvent

Question 11

Which of the following is NOT a cause of renal failure?

A) diabetes
B) heart attack
C) low blood pressure
D) severe dehydration
E) infection

Question 12

Pepto-Bismol, the liquid pink antacid that must be shaken thoroughly before administering, is a

A) solution.
B) solvent.
C) homogenous mixture.
D) colloidal dispersion.
E) suspension.

Question 13

An example of this type of mixture is red blood cells in whole blood.

A) homogenous mixture
B) suspension
C) colloidal dispersion
D) solution
E) solvent

Question 14

Is gasoline, which is nonpolar, miscible with water?

A) Yes, because they are both liquids
B) Yes, because they have similar polarities
C) No, because they are both liquids
D) No, because they have similar polarities
E) No, because they do not have similar polarities

Question 15

We can predict whether or not a solute dissolves in a solvent with the rule "like dissolves like." This rule means that

A) a solute with the same diameter as the solvent will dissolve.
B) a solute with the same phase as the solvent will dissolve.
C) a solvent with the same polarity as the solvent will dissolve.
D) a solute with the same mass as the solvent will dissolve.
E) a solute contains some of the same elements as the solvent it will dissolve.

Question 16

A _______ settles after mixing and contains visible particles.

A) solution
B) solvent
C) homogenous mixture
D) colloidal dispersion
E) suspension

Question 17

???A typical ______ contains aggregates of atoms, molecules or ions. It can also contain large molecules distributed throughout the medium.

A) solution
B) solvent
C) mixture
D) colloidal dispersion
E) suspension

Question 18

In a colloidal dispersion, the major component is called the

A) solvent.
B) solute.
C) medium.
D) colloid.
E) solution.

Question 19

Is ethanol, a polar organic molecule that can hydrogen bond, miscible with water?

A) Yes, because they are both liquids
B) Yes, because they have similar polarities
C) No, because they are both liquids
D) No, because they have similar polarities
E) No, because they do not have similar polarities

Question 20

The purpose of the kidneys is to

A) oxidize drugs.
B) store cholesterol.
C) digest food.
D) remove waste products from blood.
E) store urine.

Question 21

Which of the following usually occurs when a molecule dissolves in water?

A) The covalent bonds in the molecule break.
B) The covalent bonds in water break.
C) Covalent bonds between the molecule and water form.
D) Covalent bonds between several of the molecules form.
E) Hydrogen bonds form between the molecule and water.

Question 22

When sodium chloride dissolves in water, it forms _______ with water molecules.

A) hydrogen bonds
B) ionic bonds
C) dipole-dipole interactions
D) covalent bonds
E) ion-dipole interactions

Question 23

Which of the following substances are NOT physiologically important?

A) CO₂
B) Na⁺
C) glucose
D) HCO₃ ^-
E) All of the above are physiologically important substances.

Question 24

Which of the following is NOT an electrolyte?

A) Na⁺
B) HCO₃ ^-
C) Mg²⁺
D) HOCH₂CH₃
E) All of the above are electrolytes.

Question 25

Capsaicin is responsible for the heat of peppers. It is common practice to fry capsaicin in oil prior to eating. Which part of the capsaicin molecule forms intermolecular attractive force with oil, a nonpolar solvent?

A) a
B) b
C) c
D) d
E) All of these interact with oil.

Question 26

When MgCl₂ dissolves in water, it produces Mg²⁺ and Cl^- ions. Which statement best describes the interaction between Cl ^- and water?

A) Chloride anions are attracted to the partial negative charge of oxygen.
B) Chloride anions are attracted to the partial positive charge of oxygen.
C) Chloride anions are attracted to the partial negative charge of hydrogen.
D) Chloride anions are attracted to the partial positive charge of hydrogen.
E) Chloride anions are not attracted to any part of water.

Question 27

Which pair of solvents is NOT miscible?

A) hexane and water
B) water and methanol
C) methanol and ethanol
D) hexane and butane
E) ethylene glycol (HOCH₂CH₂OH) and ethanol

Question 28

Which of the following pictures best represents ethanol dissolved in water? Note that dashed lines represent hydrogen bonds.

A)
B)
C)
D)
E)

Question 29

How does an electrolyte differ from a nonelectrolyte?

A) Electrolytes are smaller than nonelectrolytes.
B) Electrolytes dissolve in water, while nonelectrolytes are insoluble in water.
C) Electrolytes are less polar than nonelectrolytes.
D) Electrolytes produce ions in solution while nonelectrolytes do not.
E) Electrolytes are more reactive than nonelectrolytes.

Question 30

How many ions of each type are produced when Na₃PO₄ is dissolved in aqueous solution?

A) 1 Na₃PO₄
B) 3 Na⁺, 1 P⁺, 4 O^{2 -}
C) 3 Na⁺, 4 PO₄^{3 -}
D) 3 Na⁺, 1 PO₄^{3 -}
E) 1 Na⁺, 1 PO₄ ^-

Question 31

Which figure best represents the dissolution of MgCl₂ in water?

A)
B)
C)
D)
E)

Question 32

Ethanol dissolving in water is an example of a

A) physical change, because each molecule retains its structural integral and no bonds are broken.
B) chemical change because all bonds to ethanol are broken.
C) chemical change because new bonds form between the hydrogens.
D) physical change because ethanol only loses one hydrogen to water.
E) chemical change because ethanol has a charge in solution.

Question 33

Sugar is stirred into cold iced tea and only some dissolves. The rest remains a solid. This solution is

A) miscible.
B) immiscible.
C) soluble.
D) insoluble.
E) saturated.

Question 34

Which of the following factors affect the solubility of an ionic compound in a solvent?

A) the identity of the ions
B) the strength of the electrostatic interactions between the ions
C) the temperature of the solvent
D) the identity of the solvent
E) All of these are factors in solubility.

Question 35

Is the solution of MgCl₂ in water an electrolyte?

A) Yes, because when MgCl₂ dissolves, it forms ions
B) Yes, because the MgCl₂ undergoes a chemical change in solution
C) Yes, because MgCl₂ and water react with each other
D) No, because MgCl₂ does not form ions
E) No, because MgCl₂ in water does not conduct electricity

Question 36

Which of the following solutes is most soluble in hexane?

A) pentane, CH₃CH₂CH₂CH₂CH₃
B) NaCl
C) KCl
D) methanol, CH₃OH
E) acetic acid, CH₃COOH

Question 37

An electrolyte is a substance that

A) dissolves in water.
B) does not dissolve in water.
C) hydrogen bonds with water.
D) produces ions when dissolved in water.
E) is an excellent resistor.

Question 38

Which of the following does NOT occur when an electrolyte dissolves in water?

A) A chemical change occurs.
B) The positive and negative ions separate from each other.
C) The positive ions interact with the oxygen of water.
D) The negative ions interact with the hydrogen of water.
E) The resulting solution conducts electricity.

Question 39

Which of the following describes the dissolution of MgCl₂ in water?

A) MgCl₂ → Mg⁺ + Cl₂ ^-
B) MgCl₂ → Mg²⁺ + Cl₂^{2 -}
C) MgCl₂ → Mg⁺ + Cl ^- + Cl
D) MgCl₂ → Mg²⁺ + 2Cl ^-
E) MgCl₂ → Mg⁺ + Cl ^-

Question 40

Why do kidney stones form?

A) Calcium salt levels in the kidneys reach saturated levels and precipitate.
B) Magnesium levels in the kidneys reach saturated levels and precipitate.
C) Organic toxins build up in the kidney and precipitate.
D) Chloride ions reach saturated levels in the kidney and precipitate.
E) All of the above ions and molecules contribute to the formation of kidney stones.

Question 41

According to the following table, are Jane Doe's blood test values within normal limits?

A) Yes.
B) No, glucose is too concentrated.
C) No, glucose is too dilute.
D) No, chloride is too concentrated.
E) No, chloride is too dilute.

Question 42

Jane Doe's blood test showed that her iron is 125 mg/dL. How many g/L is 125 mg/dL?

A) 12,500 g/L
B) 1.25 g/L
C) 0.00125 g/L
D) 125 g/L
E) 1250 g/L

Question 43

How many grams of dextrose are in 100 mL of D₅W (5.0% dextrose)?

A) 50 g
B) 5.0 g
C) 0.50 g
D) 0.050 g
E) 0.0050 g

Question 44

The permissible level of arsenic in drinking water is 10 ppb in the United States. What is the maximum mass of arsenic, in grams, allowable in 1 L of drinking water?

A) 10 g
B) 1.0 * 10^-6 g
C) 1.0 *10⁶ g
D) 1.0 * 10^-5 g
E) No amount of arsenic is allowable in drinking water.

Question 45

A 1% epinephrine solution is delivered by inhalation to treat asthma. This concentration is equivalent to

A) 1 g epinephrine dissolved in 100 mL of water.
B) 0.001 g epinephrine dissolved in 1 L of water.
C) 1 mg epinephrine dissolved in 100 mL of water.
D) 0.001 mg epinephrine dissolved in 1 L of water.
E) 1 μg epinephrine dissolved in 100 mL of water.

Question 46

Jane Doe has a blood glucose level of 92 mg/dL. How many grams of glucose does she have in 1 L of her blood?

A) 0.00092 g
B) 0.0092 g
C) 0.092 g
D) 0.92 g
E) 9.2 g

Question 47

Which container would be the best for preparing 1 L of a 10 g NaCl/L solution? In other words, which container will give the most accurate and precise measure of a large volume?

A) volumetric flask
B) beaker
C) graduated cylinder
D) Erlenmeyer flask
E) syringe

Question 48

How many moles of magnesium chloride (MgCl₂) are in 1.31 L of 0.38 M MgCl₂?

A) 0.498 moles
B) 0.50 moles
C) 1.49 moles
D) 1.5 moles
E) 0.29 moles

Question 49

According to a blood test, a patient has a blood iron value of 125 μg/dL. This value means that

A) the sample of blood contains 125 μg of iron.
B) the patient's body contains 125 μg of iron.
C) the mass of iron in the patient's blood is 125 μg.
D) for every deciliter of body volume, the patient contains 125 μg.
E) one deciliter of the patient's blood contains 125 μg of iron.

Question 50

What type(s) of unit(s) are represented on this table?

A) % mass/volume
B) mass/volume
C) moles/volume
D) equivalents/volume
E) both B and C

Question 51

The general equation for determining concentration is

A) concentration = amount of solvent/amount of solute.
B) concentration = amount of solute/amount of solution.
C) concentration = amount of solution/amount of solvent.
D) concentration = amount solute/amount of solvent.
E) concentration = amount of solvent/amount of solution.

Question 52

According to a blood test, a patient has a blood calcium concentration of 9.7 mg/dL. Express this concentration in mg/mL.

A) 970 mg/mL
B) 97 mg/mL
C) 9.7 mg/mL
D) 0.97 mg/mL
E) 0.097 mg/mL

Question 53

To make 1.0 L of a 10. g NaCl/L solution, 10. g of NaCl is weighed and poured into a volumetric flask. What is the next step?

A) The next step is to measure out 1.0 L of water, pour it into the container, and mix.
B) The next step is to fill the container up to the top of the flask.
C) The next step is to fill the container to the 1.0 L mark while swirling to mix.
D) The next step is to transfer the NaCl to a new flask.
E) None of these. The solute should always be added to the container after the solvent, not before.

Question 54

The concentration of an adrenalin chloride solution, used to treat acute allergic responses, is 15 mg in 30. mL. Express this concentration in mg/mL (mg per milliliter).

A) 0.50 mg/mL
B) 2.0 mg/ml
C) 5.0 mg/mL
D) 45 mg/mL
E) 450 mg/mL

Question 55

How many grams of NaCl are in 350 mL of normal saline (0.9% NaCl)?

A) 3150 g
B) 315 g
C) 31.5 g
D) 3.15 g
E) 0.315 g

Question 56

A solution is prepared by dissolving 1.5 g of NaCl in enough water to produce a total solution volume of 750 mL. What is the concentration of the solution in % m/v?

A) 0.20%
B) 2.0%
C) 0.0020%
D) 500%
E) 5.0%

Question 57

Drinking water from a well is discovered to have an arsenic concentration of 3.4 * 10^-4 g of arsenic per liter. Does this value exceed the permissible level of arsenic in drinking water of 10 ppb?

A) No, 3.4 * 10^-4 g is lower than the permissible value of 1.0 * 10^-5 g/L.
B) Yes, 3.4 * 10^-4 g is higher than the permissible value of 1.0 * 10^-5 g/L.
C) No, 3.4 *10^-4 g is lower than the permissible value of 1.0 *10^-3 g/L.
D) Yes, 3.4 * 10^-4 g is higher than the permissible value of 1.0 *10^-3 g/L.
E) It is not possible to determine the answer from the information given.

Question 58

A patient's blood test shows that his chloride level is 101 mmol/L. Convert this concentration to units of molarity.

A) 1010 M
B) 101 M
C) 10.1 M
D) 1.01 M
E) 0.101 M

Question 59

What volume of a 6.0% solution of ethanol contain 3.0 g of ethanol?

A) 5.0 mL
B) 6.0 mL
C) 10 mL
D) 30 mL
E) 50 mL

Question 60

Jane Doe's blood test showed that her iron is 125 mg/dL. You would like to convert the value into g/L. Which unit conversion converts 125 mg/dL into g/L?

A)
B)
C)
D)
E)

Question 61

Carbamazepine is an antiepileptic. A typical daily dose is 1.1

A) 0.22 mL
B) 5.5 mL
C) 22 mL
D) 220 mL
E) 5500 mL

Question 62

How many grams of glucose should be weighed out to make 1 liter of a rehydration solution that contains 75 mmol of glucose (the molar mass of glucose is 180 g)?

A) 14 g
B) 1.4 *10⁴ g
C) 0.42 g
D) 4.2*10 ^{- 3} g
E) 4.2*10 ^{- 4} g

Question 63

An order is given to administer 50. mg of furosemide, a diuretic, over the course of 2 hours by IV. If a 500. mL bag contains 200. mg of furosemide, what volume of solution does the patient need to receive over the course of two hours?

A) 0.50 mL
B) 50. mL
C) 130 mL
D) 20 mL
E) 500 mL

Question 64

Which of the following compounds passes most easily through the cell membrane?

A) Na⁺
B) glucose
C) sucrose
D) glycerol
E) O₂

Question 65

Cephadrine is one of many antibiotics that act by inhibiting bacterial cell wall synthesis. If a typical daily dosage is 660 mg, how many milliliters of 75 mg/mL suspension of cephadrine should be administered daily?

A) 660 mL
B) 75 mL
C) 0.0088 mL
D) 8.8 mL
E) 1.1 mL

Question 66

If the semipermeable membrane only allows the passage of water, what process will to occur?

A) nothing
B) mixing
C) dialysis
D) dilution
E) osmosis

Question 67

Which of the following statements describes one way in which osmosis and dialysis are similar?

A) Both involve the movement of molecules from low to high concentration.
B) Both involve the movement of molecules from high to low concentration.
C) Both involve the passage of a solute through a semipermeable membrane.
D) Both require an input of energy.
E) Osmosis and dialysis are in no way similar.

Question 68

Consider solutions A and B separated by a semipermeable membrane. Which diagram best illustrates what the volumes should look like after osmosis occurs?

A)a
B)b
C)c
D)d
E)e

Question 69

It is normal to have about 100 mM (mmol/L) of chloride (Cl ^- ) in the blood. How many meq is this?

A) 1 *10⁵ meq
B) 100 meq
C) 1 meq
D) 0.1 meq
E) 1*10 ^{- 5} meq

Question 70

If A contains 6% NaCl in water and B contains 3% NaCl in water, which of the following will occur?

A) Water will flow from A to B.
B) Water will flow from B to A.
C) NaCl will flow from A to B.
D) NaCl will flow from B to A.
E) Nothing will happen.

Question 71

In the following diagram, A is ______ and B is ______.

A) hypotonic; hypertonic
B) hypertonic; hypotonic
C) A and B are isotonic.
D) A and B are both hypotonic.
E) A and B are both hypertonic.

Question 72

A child is given 7.5 mL of a liquid pain reliever as a suspension containing 160 mg/5 mL of the pain reliever. How many milligrams of the pain reliever did the child receive?

A) 1200 mg
B) 21 mg
C) 107 mg
D) 1.5 mg
E) 240 mg

Question 73

A student adds 0.250 L of 200 mM buffer stock solution to a volumetric flask and dilutes the stock to 1.0 L. What is the final concentration of the solution?

A) 0.11 mmol
B) 110 mmol
C) 11 mmol
D) 50 mmol
E) 5.0 mmol

Question 74

An order is given to administer 100. mg of furosemide, a diuretic, over the course of 4 hours by IV. If a 500. mL bag contains 200. mg of furosemide, what flow rate, in mL per hour, should be administered to the patient?

A) 25 mg/hour
B) 25 mL/hour
C) 63 mL/hour
D) 10 mL/hour
E) 250 mL/hour

Question 75

Which of the following statements describes one way in which osmosis and dialysis are different?

A) Osmosis is the movement of molecules from low to high concentration and dialysis is the reverse.
B) Dialysis is the movement of molecules from low to high concentration and osmosis is the reverse.
C) Osmosis refers to the flow of solvent, whereas dialysis refers to the flow of small solutes.
D) Dialysis refers to the flow of solvent, whereas osmosis refers to the flow of small solutes.
E) In dialysis, colloids cannot cross the semipermeable membrane, but they can in osmosis.

Question 76

A biologist needs 500 mL of a 10 mM phosphate buffer. The stock solution of the buffer is 100 mM. How much stock solution should be used to make the 10 mM phosphate buffer?

A) 500 mL
B) 5000 mL
C) 50 mL
D) 5.0 mL
E) 0.5 mL

Question 77

If A contains 3 mmol NaCl and 3 mmol glucose, while B contains 6 mmol NaCl, which of the following will occur?

A) Water will flow from A to B.
B) Water will flow from B to A.
C) NaCl will flow from A to B.
D) NaCl will flow from B to A.
E) Nothing will happen.

Question 78

The cell membrane separates the interior of the cell from its surroundings, but it does allow the passage of some small molecules from regions of higher concentration to regions of lower concentration. This process is called

A) osmosis.
B) simple diffusion
C) dialysis.
D) dissolution.
E) active transport.

Question 79

Convert 0.015 M Ca²⁺ to equivalents of Ca²⁺.

A) 0.015 equivalents
B) 7.5 *10 ^{- 4} equivalents
C) 0.030 equivalents
D) 15 equivalents
E) 0.75 equivalents

Question 80

How many moles of glucose are in 0.82 L of a 0.13 M glucose solution?

A) 0.11 moles
B) 0.33 moles
C) 6.3 moles
D) 1.9 moles
E) 0.22 moles