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Chem 108 > ch 9 > Flashcards

ch 9 Flashcards

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1
Q

1.- 3. What is a solution (3 things)?

A
  1. homogenous mixture of 2 or more substances.
  2. forms when there is sufficients attraction between molecules of the solute and solvent.
  3. Have 2 components: Solvent (larger amount), and the solute (smaller amount).
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2
Q

1.-5. What are 5 facts about Solutes?

A
  1. may be liquid, gas, or solid.
  2. spread evenly through solution.
  3. mix w/ solvent so both solute and solvent have same state
  4. can’t be separated by filtration. Only evaporation
  5. not visible, but can give color to solution.
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3
Q
  1. T or F, water is a polar solvent? Why?
  2. How do solutions form?
  3. Explain “like dissolves like”, and how it pertains to solutions.
A
  1. T. Because of O-H bonds
  2. form when the solute–solvent interactions are large enough to overcome the solute–solute interactions and the solvent–solvent interactions.
  3. solutions will form when both solute and solvent have similar polarities. Ie: if both solute and solvent are polar, solutions will form. If solute and solvent are polar and non-polar, they won’t go into solutio (think oil and water).
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4
Q
  1. What is hydration?
  2. What is an electrolyte?
  3. What is a non-electrolyte?
  4. What is a strong electrolyte?
  5. What is a weak electrolyte?
A
  1. this is what happens when water molecules surround each ion and pull it into solution
  2. ions dissolved in water that can conduct electricity.
  3. a covalent substance that doesn’t separate into ions when dissolved. Rather dissolves as whole molecule. They don’t conduct electricity. Carbon compounds are an example.
  4. There is a 100% dissociation into ions NaCl is example. These are always ionic compounds. Strong electrical conduction. Represented by an arrow going one way.
  5. a compound that only partially dissolves into ions, and will go back and forth between dissociation and recombination. They are still ionic. Represented by two arrows
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5
Q
  1. What is solubility?
  2. Does temp affect the solubility of a solute? How?
  3. How do we express solubility mathematically?
  4. What is an unsaturated solution?
  5. What is a saturated solution
  6. What is a super-saturated solution?
A
  1. the maximum amount of solute that dissolves in a specific amount of solvent
  2. yes. Warmer temps increase solubility except with gasses in H2O. The it is the opposite case.
  3. grams of solute per 100 grams of H20 : g of solute/100g H20
  4. Contains less than the max amount of solute, and could dissolve more solute.
  5. contain max amount of solute. Any excess solvent will deposit on bottom
  6. A solution which is saturated at a high temp, and then cools
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6
Q
  1. What is Henry’s law?
  2. What is a soluble vs insoluble salt?
  3. What types of ions are soluble?
A
  1. Solubility of gas in a liquid is directly related to the pressure of that gas above the liquid. The more pressure, the more gas molecules dissolve in the liquid.
  2. Both are ionic compounds, yet soluble salts dissolve in water. Insoluble salts have ionic bonds too strong for H20 to dissolve.
  3. Li, Na, K, NH4, NO3, C2H3O2 (acetate).
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7
Q
  1. What is the concentration of a solution? How do we express this ration?
  2. -5. What are the 4 ways we can express concentration mathematically?
  3. What must you be very careful of when calculating solution?
A
  1. The amount of solute dissolved in a certain amunt of solution. concentration of solution = amount of solute/amount of solution
  2. m/m mass to mass percent: mass of solute/mass of solution x 100%
  3. v/v volume to volume percent: v of solute/v of solution x 100%
  4. m/v percent: mass of solute/ mL of solution x 100%
  5. molarity concentration (M): M= moles of solute/Liters of solution
  6. Solution is a combined value of the solute and solvent. Sometimes you will receive this info separate, and must think to add it together for the total solution.
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8
Q
  1. What is dilution?

2. the concentrations and volumes of initial and diluted solutions are related by which equations (there are two):

A
  1. a solvent, usually water, is added to a solution, which increases its volume and decreases the concentration of the solution. Mass and moles of solvent stays the same.
  2. for % of concentration:
    C1V1=C2V2

for molarity: M1V1=M2V2

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9
Q
  1. Describe the properties of a solution (as opposed to colloids ect).
  2. Describe colloids:
  3. Describe suspensions:
A
  1. Transparent, don’t separate, have small particles (like ions or molecules) that can’t be filtered and pass thru semipermeable membranes.
  2. have medium-sized particles, can’t be filtered, but can be separated by a semipermeable membrane. Ie: dust, smoke, marshmallow, blood plasma
  3. Heterogeneous mixtures. Large particles that settle. Can be filtered and must be stirred for suspension. Ie: oj, blood platelets
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10
Q

1-3 What are the 3 main points in osmosis?

  1. osmotic pressure is…….
A
  1. water flows from areas of lower to higher solute concentration.
  2. the level of the solution with the higher solute concentration rises
  3. the concentrations of the two solutions equalize with time
  4. equal to the pressure that would prevent the flow of additional water into the more concentrated solution and
    greater as the number of dissolved particles in the solution increases
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11
Q
  1. What happens in reverse osmosis?
A
  1. a pressure greater than the osmotic pressure is applied to a solution forcing it through a purification membrane.
    The flow of water is reversed leaving behind the molecules and ions in solution.
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12
Q
  1. What is an isotonic solution?

2. What are is considered an isotonic solution of glucose and NaCl?

A
  1. exerts the same osmotic pressure as body fluids such as red blood cells (RBCs)
  2. of 5.0% (m/v) glucose or 0.90% (m/v) NaCl is a typical isotonic solution
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13
Q
  1. What is a hypotonic solution?

2. What happens to cells in a hypotonic solution?

A
  1. has a lower solute concentration than RBCs.
    Means water flows into cells by osmosis.
  2. they will swell and possible burst hemolysis.
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14
Q
  1. What is a hypertonic solution?

2. What happens to cells in a hypertonic solution?

A
  1. has a higher solute concentration than RBCs. Means water flows out of cells.
  2. causes crenation: RBCs shrink in size
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15
Q
  1. What 3 things happen in dialysis?
A
  1. Solvent and small solute particles pass through an artificial membrane.
  2. Large particles are retained inside.
  3. Waste particles such as urea from blood are removed
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Chem 108 (10 decks)

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