MISC 02 - Midterm Quiz Flashcards by Juan Carlos Cornelio

A physician wishes to administer 1,200,000 units of penicillin G potassium every 4 hours. If 1 unit of penG potassium (MW=372) is 0.6 micrograms, how many mEq of potassium will the patient receive in a 24-hour period?

a. 11.61 mEq
b. 15.50 mEq
c. 93.02 mEq
d. 180 mEq
e. 1,080 mEq

a. 11.61 mEq

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A drug solution was prepared by adding 32.10 g of FeSO4 (MW 151.91) to enough water to make 500 mL of solution. The density of this solution is 1.0376. You solved for the following concentration expressions (1) the molarity; (II) the molality; (III) the mole fraction of FeSO4; (IV) the mole-fraction of water, and (V) the percent by weight of FeSO. Based on your answers, which of the following is correct?

I. The molality of the solution is 0.4342 m.
II. The molarity of the solution is 0.4226 M.
III. The mole fraction of water is 0.9922.
IV. The mole fraction of ferrous sulfate is 0.0076.
V. The equivalent weight of solute is 75.96.
VI. The percentage by weight of ferrous sulfate is 6.19 %.

a. I, II, III and IV
b. I, II, V, VI
c. III, IV, V, VI
d. I, II, III, V
e. All of the answers are correct

a. I, II, III, and IV

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Calculate the vapor pressure of solution when 0.5 mole of sucrose is added to 1000 g of water at 20°C. The vapor pressure of water at 20°C is 17.54 mmHg.

a. 0.16 mmHg
b. 2.81 mmHg
c. 17.38 mmHg
d. 17.70 mmHg
e. 108.63 mmHg

c. 17.38 mmHg

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A 0.2510 m aqueous solution of a drug gave a boiling point elevation of 0.113°C. Calculate the approximate molal elevation constant for the solvent.

a. 0.0284 °C/mole
b. 0.3640 °C/mole
c. 2.2212 °C/mole
d. 0.4502 °C/mole
e. 0.138 °C/mole

d. 0.4502 °C/mole

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What is the freezing point depression of a 1.3-m solution of NaCl, a strong electrolyte, in water?

a. 2.42°C
b. 4.35°C
c. 0°C
d. -2.42°C
e. -4.35°C

b. 4.35°C

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One gram of sucrose, molecular weight 342, is dissolved in 100 mL of solution at 25°C. What is the osmotic pressure of the solution?

a. 0.0029 atm
b. 0.0709 atm
c. 0.2428 atm
d. 0.2923 atm
e. 0.7094 atm

e. 0.7094 atm

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The freezing point of a molal solution of a nonelectrolyte is -1.86°C. What is the freezing point of a 0.1% solution of zinc chloride (MW 136), dissociating 80%? Assume that the volume of the molal solution is approximately 1 liter.

a. -0.04°C
b. 0°C
c. 1.04°C
d. 2.09°C
e. None of the choices

a. -0.04°C

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If 1500 g of a solution contains 75 g of a drug substance, what is the % (w/w) of the solution?

a. 5.00%
b. 4.76%
c. 5.26%
d. 11.25%
e. None of the above

a. 5.00%

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A solution contains 10 mg % of Ca2+ ions (AW 40). How many milliosmoles are represented in 1 liter of the solution?

a. 2.5 mOsmol
b. 5 mOsmol
c. 20 mOsmol
d. 40 mOsmol
e. 50 mOsmol

b. 5 mOsmol

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Calculate the molar concentration (Molarity) of 15.0 g NaOH in 225 mL of solution. (MW of NaOH is 40.0g)

a. 2.65 M
b. 1.67 M
c. 0.84 M
d. 0.375 M
e. None of the above

b. 1.67 M

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Calculate the approximate E value for a new drug (MW 187) with an Liso value of 2.5.

a. 0.23
b. 0.31
c. 2.75
d. 4.4
e. 10.9

a. 0.23

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The Liso of a new drug is 0.23. Based on this, how many grams of dextrose (MW 180) should be used in compounding the following prescription?

New drug - 0.5%
Dextrose - q.s.
Rose water ad - 50 mL
Make isoton. sol

a. 0.0575 g
b. 0.3925 g
c. 0.325 g
d. 0.18 g
e. 2.1805 g

d. 0.18 g

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A certain compound has a vapor pressure of 120 mmHg at 210 K and 14 mmHg at 150 K. Calculate the heat of vaporization of the compound.

a. 9,379.28 J/mol
b. 15,311.32 J/mol
c. 22,700.10 J/mol
d. 26,156.20 J/mol
e. None of the above

a. 9,379.28 J/mol

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Arrange the following in order of decreasing solubility in ammonia: CH2Cl2, CH4, H2O

a. CH2C > CH4 > H2O
b. CH4 > H2O > CH2Cl2
c. H2O > CH2Cl2 > CH4
d. CH2Cl2 > CH4 > H2O

c. H2O > CH2Cl2 > CH4

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This is defined as a mixture of two or more components that form a homogenous molecular dispersion, in other words, a one-phase system, the composition of which can vary over a wide range.

a. True solution
b. Saturated solution
c. Unsaturated solution
d. Supersaturated solution
e. All of the above

a. True solution

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Which of the following is/are true about electrolytes?

I. Colligative properties of electrolyte solutions are higher than non-electrolytes
II. Strong and weak electrolytes are always assumed to be 80% dissociated.
III. An electrolyte solution such as vinegar conducts heat and electricity.

a. I and II
b. II and III
c. I and III
d. I, II, and III

d. I, II, and III

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Which of the following is NOT a factor which influences the rate of reaction?

a. Presence of catalysts
b. Concentration
c. Temperature
d. None of the choices

d. None of the choices

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If the dissolution of an ionic solid in water is exothermic, then it can be concluded that

a. △H for the solution process is positive
b. The solution process takes up heat
c. The lattice energy exceeds the hydration energy
d. The solubility of the ionic solid is independent of temperature
e. The solubility of the ionic solid decreases with increasing temperature

e. The solubility of the ionic solid decreases with increasing temperature

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Ionized solutes will readily partition into the non-aqueous phase. The partition coefficient is usually defined as the ratio of solubility in the aqueous phase to that in the non-aqueous phase.

a. Statement 1 is true, while 2 is false.
b. Statement 2 is true, while 1 is false.
c. Both statements are true
d. Both statements are false.

a. Statement 1 is true, while 2 is false.

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For solution to happen, the intermolecular forces between solute and solvent particles must be strong enough to compete with those between solute particles and those between solvent particles. When a solution is contained within a semipermeable membrane and separated from the solvent, the solvent will pass across the membrane into the solution.

a. Statement 1 is true, while 2 is false.
b. Statement 2 is true, while 1 is false.
c. Both statements are true
d. Both statements are false

c. Both statements are true

Imagine that you have created a solution of sugar and water in class. Your teacher has asked you to retrieve the sugar in its dry state. Which plan of action below should you choose?

a. Freeze the solution
b. Let the water evaporate
c. Do nothing because it is impossible to retrieve the sugar
d. Boil the solution and let it cool back down to room temperature
e. None of the choices

b. Let the water evaporate

The NaCl equivalent of ZnSO4 is 0.16. This means that:

a. 1.0 g of NaCl represents 0.16 g ZnSO4
b. 0.16 g NaCl is equivalent to 1 g ZnSO4
c. 0.16 g NaCl is equivalent to 0.16 g ZnSO4
d. None of the choices

b. 0.16 g of NaCl is equivalent to 1 g ZnSO4

Which substance is classified as a weak electrolyte?

I. Urea
II. Ephedrine
III. Sodium chloride
IV. sucrose

a. I, II, and IV
b. I and II
c. II only
d. I and IV only
e. I, II, III, and IV

c. II only

How will you describe the solubility of a substance if 46 grams of solute dissolves in 360 mL of solvent?

a. Very soluble
b. Freely soluble
c. Soluble
d. Sparingly soluble
e. Slightly soluble

c. Soluble

Which of the following methods of adjusting tonicity is not based on E values? A. Cryoscopic method B. White-Vincent Method C. Sprowl's method d. NaCl equivalent method e. None of the above

A. Cryoscopic method

Arrange the following in order of decreasing vapor pressure: I. CH3OCH3 II. CH3CH2OH III. CH3CH2CH2CH3 IV. CH3CH2CH3 V. CHCI a. II > V > I > IV > III b. II > I > V > IV > III c. II > III > IV > I > V d. III > IV > I > V > II e. III > IV > V > I > II

d. III > IV > I > V > II

According to this law, at a definite temperature, the partial pressure component in a liquid mixture is equal to vapor pressure in the pure state multiplied by the mole fraction of the component in the solution. a. Le Chatelier's b. Dalton's law c. Raoult's law d. Nernst law e. Graham's law

c. Raoult's law

Which property is classified as colligative? a. Solubility of a solute b. Osmotic pressure c. Temperature of solution d. Hydrogen ion concentration e. All of the above

b. Osmotic pressure

A solution with more solute particles than inside a cell means that the solution is: a. Hypotonic to the cell b. Isotonic to the cell c. Hypertonic to the cell d. None of the above

c. Hypertonic to the cell

Under hypertonic conditions, the cell will: a. Remain the same b. Shrink c. Swell d. None of the above

b. Shrink

Which factor would not affect the solubility of sugar in water? a. Stir the water and sugar b. Add salt to the water c. Heat the water and sugar d. Grind the sugar to make it finer e. None of the above

e. None of the above

The boiling point elevation is defined as: a. Tᵇ - Tᵒᵇ b. Tᵇ + Tᵒᵇ c. Tᵒᵇ - Tᵇ d. Tᵇ x Tᵒᵇ

a. Tᵇ - Tᵒᵇ

The colligative properties of a solution are related to the: a. Number of ions in the solution b. Total number of solute particles in the solution c. Number of unionized molecules in the solution d. All of the above

b. Total number of solute particles in the solution

Decrease in solubility of non-electrolyte by the addition of an electrolyte results in: a. Separation b. Salting out c. Salting in d. Reduction

b. Salting out

This is a type of solution where solvent cannot hold anymore the excess number of solute in a solution at a given temperature. A. Unsaturated Solution B. Saturated Solution C. Supersaturated Solution D. Dilute Solution

B. Saturated Solution

The boiling point or temperature of a substance corresponds to the temperature at which the thermal energy of the molecules is sufficient to overcome the cohesive forces that hold its molecules together in the liquid state. Substances with stronger intermolecular attractive forces have lower boiling temperatures. a. Statement I is true while II is false b. Statement II is true while I is false c. Both statements are true d. Both statements are false

a. Statement I is true while II is false

Which of the following statements is FALSE regarding polar and non-polar covalent bonds? a. The physical properties of substances are also affected by their polarities. b. A covalent bond that has an equal sharing of electrons is called a nonpolar covalent bond. c. If there is no difference in the electronegativities of atoms, this means that a molecule is nonpolar. d. The polarity of a covalent bond can be judged by determining the difference in the electronegativities of the two atoms making the bond. e. None of the above

e. None of the above

Which of the following is/are example/s of intensive property? I. Temperature II. Pressure III. Specific gravity IV. Concentration V. color a. I, II, and III only b. I, II and V only c. I, II, III, and IV only d. I, II, III, and V only e. I, II, III, IV and V

e. I, II, III, IV and V

A student from physical pharmacy class has characterized the physical properties of water drinking fountain available in school. Upon determining the boiling point, there was an apparent difference between the actual and theoretical value. This means that: a. The water is impure. b. The water has microbial contamination. c. It is normal d. A and B e. A, B, and C

a. The water is impure.

If the volume of a container of gas is reduced, what will happen to the pressure inside the container? a. The pressure will increase b. The pressure will not change c. The pressure will decrease d. The pressure depends on the type of gas e. None of the above

a. The pressure will increase

The added factors a and b in the van der Waals constant in the relationship (P+) (V - nb) = nRT are factors that correct for deviations in the gas constant, R. a. The tendency of the gas molecules to ionize. b. The average velocities of the gas molecules. c. The pressure exerted by the gas molecules at constant temperature. d. The attractive forces and volume occupied by the gas molecules. e. All of the above

d. The attractive forces and volume occupied by the gas molecules.

What is the new pressure of 5.0 g sample of gas with a volume of 650 mL at 1.50 atm is expanded to 7.50 L at constant temperature? a. 6.67 torr b. 98.8 atm c. 1.91 psi d. 0.17 mm Hg e. None of the above

e. None of the above

Calculate the molecular weight of a gas if 0.53 gram of it occupies 59.7 mL at STP? a. 31.6 g/mol b. 40.0 g/mol c. 47.8 g/mol d. 143.1 g/mol e. 196.30 g/mol

e. 196.30 g/mol

The least number of intensive variables that must be fixed to describe the system completely. a. Number of phases b. Number of components c. Number of intermediates d. Number of degrees of freedom e. None of the above

d. Number of degrees of freedom

Which of the following is/are definition/s of a drug? I. It is a substance recognized in an official pharmacopoeia or formulary II. It is intended for the diagnosis, cure, mitigation, treatment, or prevention of disease. III. It is a chemical that affects the structure or function of the human body. IV. It is intended for use as a device or a component, part, or accessory of a device. a. I and II only b. I, II, and III only c. I, II, and IV only d. I, III, and IV only e. I, II, III, and IV

b. I, II, and III only

This is used for relating the effect of the least number of independent variables upon various phases that can exist in an equilibrium system containing a given number of components. a. Newton's Law b. Le Chatelier's principles c. Avogadro's principle d. Gibb's phase Rule e. Dalton's law

d. Gibb's phase Rule

Dialysis solutions are administered through what delivery system? a. Oral b. Rectal c. Topical d. Parenteral e. Respiratory

d. Parenteral

What do you call the physical properties of matter that depend on the arrangement on the number and kind of atoms within the molecule? a. Additive b. Colligative c. Constitutive d. Extensive

c. Constitutive

As a pharmacy student, your knowledge in physical pharmacy may be useful in: I. An understanding of the basic physical chemistry necessary for the drug design. II. Increasing the absorption of drug upon administration. III. The manufacture of medicines on both a small and a large scale. IV. The cultivation, avoidance, and elimination of microorganisms in medicines. A. I and II only B. II and III only C. I, II, and III only D. I, II, and IV only E. I, II, III, and IV

E. I, II, III, and IV