1.11: Colligative Properties
- Page ID
- 38591
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 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)