- الرساله ؛ اسئلة عن ملزمة الستيت

- الرساله ؛ 1. What distinguishes intramolecular forces from intermolecular forces?
A. Intramolecular forces act between molecules, while intermolecular forces act within a molecule.
B. Intramolecular forces act within a molecule, while intermolecular forces act between molecules.
C. Both act only within a molecule.
D. Both act only between molecules.
Answer: B


2. Which of the following is an intermolecular force?
A. Covalent bonds
B. Ionic bonds
C. Van der Waals forces
D. Sigma bonds
Answer: C


3. Which intermolecular force is responsible for hydrogen bonding?
A. Dipole-dipole interaction
B. Ion-dipole interaction
C. London dispersion forces
D. Induced dipole forces
Answer: A


4. Which of the following is the weakest intermolecular force?
A. Hydrogen bonding
B. Ion-dipole interaction
C. Van der Waals forces
D. Ionic bonds
Answer: C


5. What causes repulsion between two molecules when they get too close?
A. Electrostatic attraction
B. Overlapping electron clouds
C. Dipole-dipole forces
D. Formation of ionic bonds
Answer: B


6. What does Boyle's law state?
A. Pressure is proportional to volume at constant temperature.
B. Pressure is inversely proportional to volume at constant temperature.
C. Temperature is proportional to volume at constant pressure.
D. Temperature is inversely proportional to volume at constant pressure.
Answer: B


7. What is the ideal gas equation?
A. PV = nRT
B. P = nRT/V
C. V = nRT/P
D. All of the above
Answer: D


8. What assumption is incorrect for an ideal gas?
A. Molecules have negligible volume.
B. Molecules do not attract or repel each other.
C. Molecules have elastic collisions.
D. Molecules have strong intermolecular forces.
Answer: D


9. What is the critical temperature of water?
A. 374°C
B. 100°C
C. 218°C
D. 5.2°C
Answer: A


10. Which gas law explains the proportionality of temperature and volume?
A. Boyle’s Law
B. Charles’s Law
C. Avogadro’s Law
D. Dalton’s Law
Answer: B


11. What happens when a liquid reaches its boiling point?
A. Vapor pressure equals atmospheric pressure.
B. Vapor pressure exceeds atmospheric pressure.
C. Atmospheric pressure exceeds vapor pressure.
D. Temperature drops suddenly.
Answer: A


12. What is the latent heat of fusion for water?
A. 540 cal/g
B. 80 cal/g
C. 478 cal/g
D. 374 cal/g
Answer: B


13. What is the critical pressure of water?
A. 218 atm
B. 100 atm
C. 5 atm
D. 374 atm
Answer: A


14. What happens to liquids with higher molecular weight hydrocarbons?
A. They have higher boiling points.
B. They have lower boiling points.
C. Boiling point remains constant.
D. Boiling point decreases rapidly.
Answer: A


15. Why does ethanol have a higher boiling point than hydrocarbons of similar molecular weight?
A. It has a higher molecular weight.
B. It forms hydrogen bonds.
C. It forms ionic bonds.
D. It has lower vapor pressure.
Answer: B


16. Which structure does NaCl have?
A. Cubic
B. Tetragonal
C. Monoclinic
D. Hexagonal
Answer: A


17. What is polymorphism?
A. Different molecular weights of the same compound
B. Different crystalline forms of the same compound
C. Different solubilities of compounds
D. Different melting points of unrelated compounds
Answer: B


18. Why are amorphous solids more soluble than crystalline solids?
A. They are denser.
B. They have random molecular arrangements.
C. They have higher melting points.
D. They have lower thermal conductivity.
Answer: B


19. Which method is used to differentiate between polymorphs?
A. X-ray diffraction
B. UV spectroscopy
C. IR spectroscopy
D. Mass spectrometry
Answer: A


20. What describes the liquid crystalline state?
A. It is purely liquid.
B. It is intermediate between liquid and solid states.
C. It is purely solid.
D. It is an amorphous phase.
Answer: B

- الرساله ؛ Mcq للملزمه الثانيه

- الرساله ؛ 1. What is the first law of thermodynamics?
A. Energy can be created or destroyed.
B. Energy is always conserved.
C. Entropy of the universe always increases.
D. Energy can only exist in the form of heat.
Answer: B


2. What is internal energy composed of?
A. Only kinetic energy
B. Only potential energy
C. Both kinetic and potential energy
D. Heat energy only
Answer: C


3. Which thermodynamic process occurs without any heat transfer?
A. Isothermal
B. Adiabatic
C. Isobaric
D. Isochoric
Answer: B


4.What is the correct equation for work done in a system against constant pressure?
A. W = P * ΔV
B. W = -P * ΔV
C. W = Q - P * ΔV
D. W = ΔH - ΔE
Answer: B


5. In a reversible isothermal expansion of an ideal gas, the maximum work done is given by:
A. W = -nRT * ln(V2/V1)
B. W = nRT * ln(P2/P1)
C. W = nRT * (V2/V1)
D. W = -P * ΔV
Answer: A


6. What defines an isolated system in thermodynamics?
A. Exchanges only heat with surroundings
B. Exchanges only work with surroundings
C. Exchanges neither heat nor work with surroundings
D. Exchanges heat and work with surroundings
Answer: C


7. What is enthalpy ()?
A. The heat content of a system at constant pressure
B. The heat required to increase kinetic energy only
C. The potential energy of a system
D. The entropy of a system
Answer: A


8. Which of the following reactions is endothermic?
A. Heat is evolved during the reaction
B. Heat is absorbed during the reaction
C. No heat transfer occurs during the reaction
D. The reaction is irreversible
Answer: B


9. The enthalpy of fusion () refers to:
A. The heat required to vaporize a liquid
B. The heat absorbed by a solid when melting
C. The heat released during freezing
D. The heat required to break chemical bonds
Answer: B


10. What is Hess's Law?
A. The heat of a reaction is independent of the pathway.
B. The entropy change is zero for reversible reactions.
C. Heat always flows from hot to cold.
D. The Gibbs free energy must be negative for spontaneous processes.
Answer: A


11. Entropy () measures:
A. Heat content of a system
B. Randomness or disorder of a system
C. The potential energy of a system
D. The stability of a chemical reaction
Answer: B


12. What is the condition for a process to be spontaneous?
A. ΔG > 0
B. ΔG = 0
C. ΔG < 0
D. ΔH > ΔS
Answer: C


13. Which equation represents Gibbs free energy?
A. ΔG = ΔH + TΔS
B. ΔG = ΔH - TΔS
C. ΔG = TΔS - ΔH
D. ΔG = ΔE - TΔH
Answer: B


14. At absolute zero (0 K), the entropy of a perfect crystalline substance is:
A. Maximum
B. Minimum but not zero
C. Zero
D. Undefined
Answer: C


15. What does a positive  indicate about a process?
A. The process is spontaneous.
B. The process is non-spontaneous.
C. The process is at equilibrium.
D. The process releases heat.
Answer: B


16. What does the second law of thermodynamics state?
A. Energy is always conserved.
B. Entropy of the universe always increases in spontaneous processes.
C. The entropy of a perfect crystal is zero at absolute zero.
D. Work done by a system equals heat supplied.
Answer: B


17. Which process is irreversible?
A. Heat transfer from hot to cold
B. Expansion of gas in vacuum
C. Compression of gas in equilibrium
D. A thermodynamic cycle at constant pressure
Answer: A


18. What does the third law of thermodynamics imply about supercooled liquids?
A. Their entropy is zero at 0 K.
B. Their entropy is not zero at 0 K.
C. They have no enthalpy at 0 K.
D. Their Gibbs free energy is maximum at 0 K.
Answer: B


19. In which process does entropy decrease?
A. Melting of ice
B. Freezing of water
C. Expansion of gas
D. Dissolution of salt in water
Answer: B


20. What role does Gibbs free energy () play in pharmaceutical systems?
A. Predicts solubility
B. Indicates stability of preparations
C. Determines ionization of drugs
D. All of the above
Answer: D

- الرساله ؛ هاي للملزمه الثالثة

Lec 6 :

1. According to the Arrhenius Theory, how is an acid defined?
- A) A substance that liberates hydrogen ions in aqueous media.
- B) A substance that supplies hydroxyl ions on dissociation in aqueous media.
- C) A substance that donates protons.
- D) A substance that accepts protons.

Answers: A, B

2. What does the Brönsted–Lowry theory state about acids and bases?
- A) An acid is a substance capable of donating a proton.
- B) A base is a substance capable of accepting a proton.
- C) Acids are always positively charged.
- D) Bases can only be negatively charged substances.

Answers: A, B

3. Which of the following statements regarding the strength of acids and bases is true?
- A) HCl is a strong acid in all solvents.
- B) Acetic acid can behave as a strong acid in certain solvents.
- C) The strength of an acid is dependent on solvent properties.
- D) The strength of a base does not vary with the solvent.

Answers: B, C

4. What types of solvents are classified under amphiprotic solvents?
- A) Water
- B) Acetone
- C) Alcohols
- D) Hydrocarbons

Answers: A, C

5. In the Lewis theory, how is an acid defined?
- A) A substance that donates a proton.
- B) A molecule or ion that accepts an electron pair.
- C) A substance that provides a pair of unshared electrons.
- D) A neutral molecule that can act as a base.

Answers: B, C

6. What is true about polyprotic electrolytes?
- A) They can donate only one proton.
- B) Diprotic acids ionize in two stages.
- C) Triprotic acids ionize in three stages.
- D) They are always strong acids.

Answers: B, C

7. What factors influence the ionic strength of a solution?
- A) Total ion concentration.
- B) The charge of the ions present.
- C) Temperature of the solution.
- D) The volume of the solvent.

Answers: A, B

8. What is the Sörensen's pH scale used for?
- A) Measuring the concentration of hydroxyl ions.
- B) Quantifying the degree of acidity and alkalinity of a solution.
- C) Defining the molecular structure of acids and bases.
- D) Classifying different types of solvents.

Answers: B

9. Which of the following describes ampholytes?
- A) Compounds that can act as both acids and bases.
- B) Compounds that only donate protons.
- C) Compounds that accept protons only.
- D) Compounds that are always neutral.

Answer: A

10. What is the neutral pH value at room temperature?
- A) 0
- B) 7
- C) 14
- D) 6.15

Answer: B

11. In the context of acid-base reactions, what occurs during protolysis?
- A) An acid reacts with a base to form a new acid and a new base.
- B) Protons are transferred between different molecules.
- C) Strong acids dissociate completely in water.
- D) Weak acids do not participate in reactions.

Answers: A, B

12. Which of the following statements is true regarding monoprotic and polyprotic electrolytes?
- A) Monoprotic electrolytes can donate multiple protons.
- B) Polyprotic acids can donate two or more protons.
- C) Diprotic acids ionize in only one stage.
- D) Monoprotic acids have a simpler ionization process.

Answers: B, D

13. What is the effect of ionic strength on a solution?
- A) It affects the solubility of ionic compounds.
- B) It influences the activity coefficients of ions.
- C) It changes the pH of the solution.
- D) It has no significant effect on chemical reactions.

Answers: A, B

14. Which of the following are examples of Lewis acids?
- A) Boron trifluoride
- B) Aluminum chloride
- C) Acetic acid
- D) Hydrochloric acid

Answers: A, B

15. What happens at the isoelectric point (IEP) of a molecule?
- A) The molecule has maximum solubility.
- B) The net charge of the molecule is zero.
- C) The molecule donates protons only.
- D) The molecule exists only in its neutral form.

Answers: B, A

Lec 7 :

1. What is the primary function of a buffer solution?**
- A) To change the pH of a solution
- B) To resist changes in pH upon the addition of acids or bases
- C) To increase the temperature of a solution
- D) To dissolve salts

Answer: B

2. Which equation is commonly used to describe buffer systems?**
- A) Henderson-Hasselbalch equation
- B) Nernst equation
- C) Arrhenius equation
- D) Van 't Hoff equation

Answer: A

3. What is the consequence of adding a strong acid or base to a non-buffered solution?**
- A) The pH remains unchanged
- B) The pH changes significantly
- C) The solution becomes isotonic
- D) The solution becomes cloudy

Answer: B

4. Why are buffer solutions typically not prepared from weak bases and their salts?
- A) They are too expensive
- B) They are not effective at maintaining pH
- C) They have a higher pH range
- D) They are less stable than weak acids

Answer:** B

5. What is buffer capacity?**
- A) The ability of a buffer to dissolve salts
- B) The maximum amount of acid or base a buffer can neutralize while maintaining pH
- C) The rate at which a buffer solution can react
- D) The concentration of salt in a buffer solution

Answer: B

6. What pH range is typically maintained in human blood?**
- A) 6.0 - 6.5
- B) 7.0 - 7.5
- C) 7.35 - 7.45
- D) 8.0 - 8.5

Answer: C

7. Which of the following is a common biological buffer in erythrocytes?**
- A) Sodium chloride
- B) Phosphate buffer
- C) Sodium bicarbonate
- D) Hemoglobin/oxyhemoglobin

Answer: D

8. What effect does a low buffer capacity have on tissue irritation?**
- A) It increases irritation
- B) It has no effect
- C) It minimizes irritation
- D) It makes irritation unpredictable

Answer: C

9. At which pH does the undissociated form of weakly basic drugs predominantly exist?**
- A) Low pH (around 4)
- B) Physiological pH (around 7.4)
- C) High pH (around 9)
- D) Neutral pH (around 7)

Answer: B

10. What is the purpose of using isotonic solutions in pharmaceutical applications?**
- A) To increase the concentration of drugs
- B) To prevent discomfort and tissue swelling
- C) To change the pH of the solution
- D) To enhance drug absorption

Answer: B

11. What happens to the pH of a buffer solution when a small amount of strong acid is added?**
- A) The pH increases significantly
- B) The pH decreases slightly
- C) The pH remains unchanged
- D) The pH fluctuates wildly

Answer: B

12. Which of the following statements is true regarding pH indicators?**
- A) They are always colorless
- B) They change color based on the pH of the solution
- C) They can only be used in buffered solutions
- D) They are not affected by temperature

Answer: B

13. What effect does dilution have on buffer solutions?**
- A) It increases buffer capacity
- B) It can change the pH significantly
- C) It has no effect on pH
- D) It stabilizes the solution

Answer: B

14. In the context of buffer solutions, what does the term "dilution value" refer to?**
- A) The volume required to prepare a buffer
- B) The change in pH when the buffer is diluted to half strength
- C) The concentration of the buffer components
- D) The total volume of the buffer solution

Answer: B

15. Which buffer system is primarily responsible for maintaining blood pH?**
- A) Carbonic acid/bicarbonate
- B) Ammonium/amine
- C) Acetic acid/sodium acetate
- D) Phosphate buffer

Answer: A

16. What is the primary reason for adjusting the pH of drug solutions?**
- A) To enhance solubility
- B) To increase the color intensity
- C) To maintain a stable temperature
- D) To alter physical appearance

Answer: A

17. Which of the following factors does NOT affect buffer capacity?**
- A) The ratio of salt to acid concentration
- B) The temperature of the solution
- C) The individual concentrations of buffer components
- D) The presence of other compounds in solution

Answer: B

18. Why is it important to maintain the pH of urine within a specific range?**
- A) To prevent kidney damage
- B) To ensure proper drug absorption
- C) To regulate body temperature
- D) To maintain electrolyte balance

Answer: A

19. How does the presence of a buffer solution influence the solubility of an alkaloidal base?**
- A) It decreases solubility at low pH
- B) It stabilizes the base and prevents precipitation
- C) It increases the pH, leading to precipitation
- D) It has no effect on solubility

Answer: B

20. Which type of buffer is commonly used in ophthalmic solutions?**
- A) Strong acid buffers
- B) Weak acid buffers
- C) Strong base buffers
- D) Non-buffered solutions

Answer: B

Lec 4 : " Solution of Non-Electrolytes "


1. What are the main objectives of studying non-electrolyte solutions?
- A) Identification of colligative properties
- B) Understanding types of pharmaceutical solutions
- C) Determining molecular weight
- D) Calculating enzyme activity

Answer : A , B , C

2. Which of the following is a characteristic of a true solution?
- A) Contains dispersed particles
- B) Homogeneous mixture of substances
- C) Visible separation of phases
- D) Contains larger particles than colloidal dispersion

Answer : B

3. What defines an ideal solution?
- A) No heat is absorbed or evolved during mixing
- B) Changes in properties of components
- C) The solution has a different volume than the components
- D) Cohesive forces are greater than adhesive forces

Answer : A

4. In a real solution, when cohesive forces are greater than adhesive forces, what type of deviation occurs?
- A) Negative deviation
- B) Positive deviation
- C) Ideal behavior
- D) No deviation

Answer : B

5. According to Raoult’s Law, the partial vapor pressure of a component in an ideal solution is given by:
- A) The vapor pressure of the pure component multiplied by its volume fraction
- B) The vapor pressure of the pure component multiplied by its mole fraction
- C) The total pressure of the solution
- D) The temperature of the solution

Answer : B

6. What happens to the boiling point of a solvent when a non-volatile solute is added?
- A) It decreases
- B) It remains the same
- C) It increases
- D) It fluctuates

Answer : C

7. What is the significance of Kb in the context of boiling point elevation?
- A) It is a constant specific to each solute
- B) It indicates vapor pressure
- C) It relates to the boiling point elevation per molal concentration
- D) It measures the solubility of the solute

Answer : C

8. Which statement is true about freezing point depression?
- A) The freezing point of a solution is higher than that of the pure solvent
- B) The freezing point of a solution is lower than that of the pure solvent
- C) It has no effect on the vapor pressure
- D) It occurs only in ideal solutions

Answer : B

9. What is osmotic pressure?
- A) The pressure required to boil a solution
- B) The pressure that must be applied to prevent solvent passage through a semipermeable membrane
- C) The pressure of vapor in equilibrium with the liquid
- D) The pressure created by heating a solution

Answer : B

10. What is unique about steam distillation?
- A) It can only be used for miscible liquids
- B) It purifies compounds at high temperatures
- C) It allows purification of organic compounds below their decomposition temperature
- D) It is ineffective for volatile oils

Answer : C

Lec 4 ...

11. Which of the following is an example of a colligative property?
- A) Density
- B) Vapor pressure lowering
- C) Color
- D) Refractive index

Answer : B

12. What type of solution is formed when two substances with similar properties are mixed?
- A) Ideal solution
- B) Colloidal dispersion
- C) Coarse dispersion
- D) Azeotropic mixture

Answer : A

13. Which of the following describes a negative deviation in a real solution?
- A) Benzene and ethanol
- B) Chloroform and acetone
- C) Carbon disulfide and acetone
- D) Ethanol and water

Answer : B

14. What effect does increasing the concentration of a non-volatile solute have on the vapor pressure of the solvent?
- A) Increases vapor pressure
- B) Decreases vapor pressure
- C) Has no effect
- D) Fluctuates vapor pressure

Answer : B

15. What is the triple point?
- A) The temperature at which a liquid boils
- B) The point at which solid, liquid, and vapor are in equilibrium
- C) The point at which a solution freezes
- D) The boiling point of an azeotropic solution

Answer : B

16. Which of the following statements is true about ideal gases and ideal solutions?
- A) Both behave perfectly under all conditions
- B) Both have no interactions between molecules
- C) Ideal gases have no volume, while ideal solutions do
- D) Ideal solutions can exist at all concentrations

Answer : C

17. What happens during osmosis?
- A) Solvent moves from a region of high solute concentration to low
- B) Solvent moves from a region of low solute concentration to high
- C) Solvent and solute mix uniformly
- D) No movement occurs

Answer : B

18. Which of the following compounds can act as a propellant in aerosol dispensers?
- A) Water
- B) Ethanol
- C) Trichloromonofluoromethane
- D) Sucrose

Answer : C

19. When does a solution exhibit boiling point elevation?
- A) When a non-volatile solute is added
- B) When a volatile solute is added
- C) When the solution is cooled
- D) When the solution is diluted

Answer : A

20. In terms of colligative properties, what is the relationship between the number of solute particles and the properties observed?
- A) Properties depend solely on the identity of the solute
- B) Properties depend on the concentration of solute particles
- C) Properties are unaffected by the solute
- D) Properties are consistently higher with more solute

Answer : B

هذا شامل للملزمة الرابعة

Lec 4 - Colligative properties :

Elevation of Boiling Point :

1. What is the normal boiling point?
- A) The temperature at which a liquid turns into a solid
- B) The temperature at which the vapor pressure equals the atmospheric pressure
- C) The temperature at which a solid dissolves in a solvent
- D) The temperature at which all liquids evaporate

Answer : B

2. What effect does the addition of a nonvolatile solute have on the boiling point of a solvent?
- A) It lowers the boiling point
- B) It raises the boiling point
- C) It has no effect
- D) It causes the solvent to freeze

Answer : B

3. What does the term \( \Delta T_b \) represent?
- A) The change in temperature during freezing
- B) The melting point depression
- C) The boiling point elevation
- D) The initial temperature of the solvent

Answer : C

4. What is the primary reason for the boiling point elevation when a solute is added to a solvent?
- A) Increased molecular weight of the solvent
- B) Reduced vapor pressure of the solvent
- C) Increased temperature of the solution
- D) Decreased surface tension

Answer : B

5. Which of the following solutions would exhibit the greatest boiling point elevation?
- A) 1 molal NaCl solution
- B) 1 molal glucose solution
- C) 0.5 molal NaCl solution
- D) 2 molal glucose solution

Answer : A

Depression of Freezing Point :

6. What is the normal freezing point of a pure substance?
- A) The temperature at which it boils
- B) The temperature at which solid and liquid phases are in equilibrium
- C) The temperature at which it evaporates
- D) The temperature at which it sublimates

Answer : B

7. How does the addition of a solute affect the freezing point of a solvent?
- A) It raises the freezing point
- B) It causes the solvent to poil
- C) It has no effect
- D) It lowers the freezing point

Answer : D

8. Which of the following is true regarding the relationship between solute concentration and freezing point depression?
- A) The freezing point decreases with increasing solute concentration
- B) The freezing point increases with increasing solute concentration
- C) There is no relationship
- D) The freezing point remains constant regardless of solute concentration

Answer : A

9. When a solute is added to a solvent, which of the following changes occurs?
- A) The solid phase becomes more stable
- B) The liquid phase solidifies at a higher temperature
- C) The solid phase dissolves at a lower temperature
- D) The liquid phase freezes at a higher temperature

Answer : C

10. What type of solute typically has a greater effect on freezing point depression?
- A) Non-electrolytes
- B) Electrolytes
- C) Solids
- D) Gases

Answer : B

11.What happens to the freezing point of a solution when a solute is dissolved in a solvent?

A) It increases
B) It decreases
C) It remains the same
D) It fluctuates

Answer: B

12. What is required for the temperature of a solution to drop to its freezing point?

A) The temperature must rise
B) The temperature must drop to a level lower than the solid solvent
C) The pressure must increase
D) The amount of solute must decrease

Answer: B

13. What is the primary result of the lowering of the freezing point?

A) Increased vapor pressure
B) Decreased vapor pressure
C) No change in vapor pressure
D) Instant evaporation

Answer: B

14. What does the value of Kf represent?

A) The boiling point elevation constant
B) The freezing point depression constant
C) The vapor pressure constant
D) The solubility constant

Answer: B

15. What is the value of Kf for water when using solutions of sucrose and glycerin?

A) 1.86 °C kg/mol
B) 2.00 °C kg/mol
C) 0.52 °C kg/mol
D) 3.14 °C kg/mol

Answer: A

Osmotic pressure :

16. What is osmotic pressure defined as?

A) The pressure required to allow solvent passage
B) The excess pressure needed to prevent solvent passage
C) The total pressure in a solution
D) The pressure exerted by solute molecules

Answer: B

17. What happens when a non-volatile solute is added to a solvent?

A) The vapor pressure of the solvent increases
B) The vapor pressure of the solvent decreases
C) The boiling point of the solution decreases
D) The freezing point of the solution decreases

Answer: B

18. What is the role of a semipermeable membrane in osmotic pressure?

A) It allows both solute and solvent to pass freely
B) It restricts the passage of solute while allowing solvent to pass
C) It prevents any movement of molecules
D) It enhances the pressure in the solution

Answer: B

19. What effect does increasing the concentration of a solute have on osmotic pressure?

A) It decreases osmotic pressure
B) It has no effect on osmotic pressure
C) It increases osmotic pressure
D) It stabilizes osmotic pressure

Answer: C

20. Which of the following factors is NOT considered when calculating osmotic pressure?

A) Temperature
B) Volume of the solution
C) Density of the solute
D) Number of solute particles

Answer: C

21. the osmotic pressure can be affected by which of the following?

A) Type of solute
B) Nature of the solvent
C) Temperature
D) Volume of the container

Answer: A,B,C

22. What principles are osmotic pressure and distillation processes based on? (Select all that apply)

A) Escaping tendencies of water
B) Vapor pressure lowering
C) Solvent-solute interactions
D) Temperature stability

Answer: A,B

23. what factors influence the relationship between vapor pressure and osmotic pressure?

A) Temperature
B) Solvent type
C) Volume of the solvent
D) Energy of the system

Answer: A

24.What occurs at equilibrium in the context of vapor pressure and osmotic pressure? (Select all that apply)

A) Free energy of the system is minimized
B) The escaping tendency of the solvent equals that of the air
C) The pressure in the system stabilizes
D) There is no movement of molecules

Answer: A,B

وهذا بس لل Colligative properties الي بالنهاية

- الرساله ؛ 1. What is an electrolyte solution?
A) A solution that does not conduct electricity
B) A solution containing ions that conduct electricity
C) A solution of non-ionized molecules
D) A solution without ions
Answer: B

2. According to Arrhenius theory, electrolytes dissociate into:
A) Molecules
B) Atoms
C) Ions
D) Electrons
Answer: C

3. Which of the following are examples of strong electrolytes?
A) Acetic acid and ammonia
B) HCl and NaOH
C) H2CO3 and NH4OH
D) Parabens and anesthetics
Answer: B

4. What happens to the specific conductance of a strong electrolyte solution as it is diluted?
A) It increases
B) It decreases
C) It remains constant
D) It fluctuates randomly
Answer: B

5. What is the equivalent conductance of a solution?
A) The ability of ions to resist current
B) The total resistance of the solution
C) The current-carrying capacity of ions after complete dissociation
D) The molar concentration of the solution
Answer: C

6. Which electrode in an electrolyte cell undergoes reduction?
A) Anode
B) Cathode
C) Both anode and cathode
D) None of the above
Answer: B

7. Why is platinum commonly used as an electrode in electrolytic cells?
A) It reacts with ions
B) It is non-reactive and ensures accurate reactions
C) It is cheap and widely available
D) It increases the temperature of the solution
Answer: B

8. What is the ionic strength (μ) of a solution used to measure?
A) The temperature of the solution
B) The activity coefficient of ions
C) The total number of ionic charges contributing to electrostatic forces
D) The molar concentration of ions
Answer: C

9. What is the formula for osmotic pressure for electrolyte solutions?
A) \pi = RT
B) \pi = iRTc
C) \pi = mRT
D) \pi = Kf m
Answer: B

10. Which of the following is true for the osmotic coefficient (g)?
A) It measures the resistance of ions in a solution
B) It is always equal to 1 for strong electrolytes
C) It provides a measure of the degree of dissociation of weak electrolytes
D) It remains constant for all types of solutions
Answer: C

11. What happens to the equivalent conductance of a strong electrolyte upon dilution?
A) It decreases
B) It increases
C) It remains constant
D) It depends on the type of electrolyte
Answer: B

12. Which of the following is a property of electrolyte solutions?
A) Non-conductive
B) Shows transference numbers
C) Unaffected by dilution
D) Contains only non-ionized compounds
Answer: B

13. What determines ion activity in solutions?
A) Concentration only
B) Ionic strength
C) Temperature only
D) Molecular weight
Answer: B

14. What is the difference between strong and weak electrolytes?
A) Strong electrolytes dissociate completely, while weak electrolytes dissociate partially
B) Strong electrolytes cannot dissociate, while weak electrolytes can
C) Strong electrolytes conduct current only when diluted
D) Weak electrolytes contain only positive ions
Answer: A

15. In the degree of dissociation equation (α), what does \Lambda_c represent?
A) Conductance at a specific concentration
B) Specific conductance of ions
C) Total conductance of the solution
D) Maximum possible conductance at infinite dilution
Answer: A

16. Why is platinum used in electrolytic cells?
A) To ensure reactions with ions
B) Because it is non-reactive
C) To reduce energy requirements for reactions
D) Both B and C
Answer: D

17. During electrolysis, what occurs at the cathode?
A) Oxidation reaction
B) Oxygen release
C) Reduction reaction
D) Hydroxyl ion formation
Answer: C

18. What causes a decrease in specific conductance upon dilution?
A) Increase in the number of ions per unit volume
B) Decrease in the number of ions per unit volume
C) Increase in interaction between ions
D) Formation of stronger ionic bonds
Answer: B

19. Which of the following is a weak electrolyte?
A) HCl
B) H2CO3
C) NaOH
D) H2SO4
Answer: B

20. What is the formula for calculating osmotic pressure of electrolyte solutions?
A) \pi = RT
B) \pi = iRTc
C) \pi = Kf m
D) \pi = mcRT
Answer: B

21. How does the activity coefficient change in dilute solutions?
A) It increases
B) It decreases

- الرساله ؛ C) It remains constant
D) It depends on the type of ion
Answer: A

22. What happens in highly diluted solutions of strong electrolytes?
A) Ion pairs form
B) Complete dissociation occurs
C) Overall conductance decreases
D) Oxidation of cations occurs
Answer: B

23. Why does the curve for acetic acid rise sharply compared to strong electrolytes?
A) Increased dissociation upon dilution
B) Decreased dissociation of strong electrolytes
C) Reduction in the number of active ions
D) Formation of new ions
Answer: A

24. What is the definition of osmolality?
A) Number of ions in 1 liter of water
B) Number of molecules in 1 liter of water
C) Number of molecules in 1 kg of water
D) Concentration of electrolytes in 1 kg of water
Answer: C

25. Which of the following does not affect ionic strength?
A) Number of ions in the solution
B) Ion charges
C) Ion concentration
D) Temperature
Answer: D

26. What factors affect Van’t Hoff factor (i)?
A) Temperature only
B) Type of electrolyte and degree of dissociation
C) Molar concentration only
D) Molecular weight of the solvent
Answer: B

- الرساله ؛ الخامسة

Physical pharmacy :
Mcq Lec 2
+ Mcq Lec 2
Mcq Lec 3
Mcq Lec 4
Mcq Colligative properties Lec 4
Mcq Lec 5
Mcq Lec 6
Mcq Lec 7

أسئلة الفاينل - الجهاز التنفسي :

١- أكثر شكل يتنقل فيه O2 بالدم
٢- وظيفة السيرفكتانت
٣- وظيفة الpleural fluid
٤- سؤال على dissociation curve
٥- سبب دخول -cl لخلية الدم الحمراء (الجواب ياخذ مكان -hco3)
٦- اول جزء يصير بي تبادل غازي (الجواب respiratory bronchioles)
٧- سؤال متعلق بالزفير ما اتذكره ( الجواب واضح اذا تعرف ان عملية الزفير passive )
٨- وظائف الجهاز التنفس بإستثناء (الجواب تنظيم الدم او نقله)
٩- جابت ضغط O2 , CO2 بالشرايين فجوابها 95 , 40
١٠- جابت سؤال عن شيفت رايت (زياده ph نقصانco2 نقصان2-3BPG زياده درجه حراره)
١١- اكو سؤال مال
كل الاختيارات ادناه تمثل conducting airways exept
جان من ضمن الخيارات ال (alveoli) هو الجواب الصحيح
١٢- العوامل الي تحددdiffusion خلال Respiratory membrane انو تكون عمليه الانتشار inervesly عكسيه: الجواب ) thickness of the membrane

#Physiology

أسئلة المِد - فيزياوية :

١- تعريف ال Colligative
٢- شروط ال Ideal solution
٣- شروط Raoult's low
٤- سؤال بال Real solution of Raoult's low يمتى يصير ال Maximum pressure (من يصير عدنه Positive )
٥- مسألة عن ال Steam distillation مال Immiscible
(ينطي درجتين والدرجة الجديدة أقل منهم اثنينهم)
٦- العوامل الي تأثر على Kp
٧- مسألة عن ال Tf
٨- اذا ال Freezing point double so the Molecular weight..... شنو راح يصير بيه
٩- عن ال Curves مال vapor pressure lowering in vapor pressure curve for solution lies below that the pure solvent , temp. mut be ....
١٠- شنو الجزيئات الي راح تعبر خلال ال U shape tube ؟ ( الجواب : Solvent only )

أسئلة الفاينل - فيزياوية :