1.11: Colligative Properties
- Page ID
- 38591
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- A solution contains 75 mmol/L of NaCl and 100 mmol/L of glucose. What would be its freezing point?:
- -0.326°C
- -0.465°C
- -0.512°C
- -0.651°C
- -0.930°C
- A urine sample has a freezing point of -0.83°C. What is its osmolarity?:
- 224.1 mosmoles/L
- 224.1 osmoles/100 ml
- 446.1 mosmoles/L
- 446.1 osmoles/100 ml
- 892.4 osmoles/100 ml
- Choose the solution that has a freezing point closest to that a 300 milliosmolar solution of glucose:
- 100 millimolar ZnCl2
- 150 millimolar maltose
- 300 millimolar NaCl
- 100 millimolar ZnSO4
- 150 millimolar Ba(OH)2
- A mole of which of the following substances equals 1 osmole of the same substance?
- NaHCO3
- NaCl
- K2HPO4
- glucose
- Ba(OH)2
- The calculated osmolality of serum with Na = 139 mmol/L, Cl = 101 mmol/L, K = 4 mmol/L, glucose =1300 mg/L, and BUN = 140 mg/L,
- 256
- 270
- 280
- 290
- 300
Use the following Key to answer Questions 6-9:
- 1, 2 and 3 are correct
- 1 and 3 are correct
- 2 and 4 are correct
- only 4 is correct
- all are correct
- The measurement of osmolarity is based upon what principle(s)?:
- vapor pressure decrease
- viscosity
- freezing point depression
- specific gravity
- As the osmolality of a solution increases, which of the following occur(s)?:
- osmotic pressure increases
- vapor pressure decreases
- freezing point decreases
- boiling point decreases
- Osmotic pressure is:
- not measurable by how much the vapor pressure changes
- equal to number of solvent molecules times a factor
- measurable by how much it raises the freezing point of water
- proportional to concentration of solute particles
- The presence of unmeasured solutes in serum can be determined by:
- increased osmolality
- decreased osmolality
- measured osmolality significantly less than calculated osmolality
- measured osmolality significantly greater than the calculated osmolality
- Answer
-
- b (p. 267,269)
- c (p. 269)
- a (p. 267, 269)
- d (p. 267)
- d (p. 267)
- b (p. 269)
- a (p. 269)
- d (p. 267-269)
- d (p. 267)