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Chemistry Exam GR 11 > Unit 4: Solutions and Solubility > Flashcards

Unit 4: Solutions and Solubility Flashcards

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1
Q

What is a real life example of Quantitive Analysis?

A

A breathalyzer; measures concentration of alcohol in exhaled air.

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2
Q

What is the formula for meauring concentration?

A

C= N/V

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3
Q

Dilute

A

A small quantity of solute per unit volume of solution.

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4
Q

Concentrated

A

A large quntity of solute per unit volume of solution.

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5
Q

How can the wrong concentration be fatal? What happens when it’s too low?

A

Red blood cells can swell and burst (hemoglobic crisis). Cells are deprived of nutrients and oxygen.

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6
Q

When a label indicates “V/V” what does this mean?

A

V/V indicated 2 liquids that are being mixed together.

The first V represents the solute dissolved in the solution.

The second V represents the final volume of the solution.

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7
Q

What is the equation for calculating a V/V percentage?

A

Csolution = vsolute/vsolution X100%

*Your answer should be in units % V/V*

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8
Q

When you use W/V instead of V/V?

A

When there is a mass involved in the question.

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9
Q

What is the equation for calculating a W/V percentage?

A

Csolution= m solute/vsolution X100%

*Your answer should be in units % W/V*

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10
Q

Molar Concentration

A

The concentration of a solution expressed as moles of solute per unit volume of solution. (mol/L)

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11
Q

Dilution

A

The process of decreasing the concentration of a solution by adding more solvent. This doesn’t change the quantity of solute, only it’s concentration.

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12
Q

What is the equation for finding the concentration of a diluted solution?

A

CiVi=CfVf

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13
Q

What are the 2 equations for finding ppm?

A

1) 1ppm= 1g / 1000L
2) 1ppm = 1mg/L

*Choose based on the units in your problem*

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14
Q

What was the Arrhenius Acid Theory?

A

Acids are compounds that contain hydrogen and can dissolve in water to release hydrogen into solution. The hydrogen gives up its electron to the other element in the solution.

Example: HCl

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15
Q

What was the Arrhenius Base Theory?

A

Substances that dissolve in water to release hydroxide ions into solution.

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16
Q

Neutralization

A

When a base an an acid are mixed together to produce water and a salt. The H (relesed by acids) and OH (released by bases) ions join to create the water.

17
Q

What are 2 properties of bases and 4 properties of their solutions?

A

Bases:

  • Water soluable
  • Electrolytes

Base Solutions:

  • Taste bitter
  • Slippery
  • Turn red litmus blue
  • Neutralize acidic solutions
18
Q

What are 2 properties of acids and 5 properties of their solutions?

A

Acids:

  • Water soluable
  • Electrolytes

Acid Solutions:

  • Taste sour
  • Not slippery
  • Turn blue litmus red
  • Neutralize basic solutions
  • React with active metal to produce hydorgen gas
19
Q

Strong Acids and Bases

A

An acid or base that dissociates completely into ions in water. They are also strong electrolytes.

Exmaples: HCl (acid) and NaOH (base)

20
Q

Weak Acids and Bases

A

An acid or base that dissociated or ionizes very slightly in water. They are also weak electolytes.

*Most acids and bases are weak*

Examples: CH3OOH (acid) and NH3 (base)

21
Q

Strong/Weak vs. Concentrated vs. Dilute

Why should we not confuse these terms?

A

Strong and Weak: How well the ions seperate

Concerntrated and Dilute: How watered down a solution is

It is possible to have a dilute solution of a strong acid or a concentrated solution of a weak acid.

22
Q

What factor determines the strength of an acid or base?

A

How well the ions seperate.

23
Q

What is Autoionization?

A

Sometimes the collisions between molecules transfer a hydrogen ion from one molecule to another. In pure water this rarely happens.

24
Q

What happens when water molecules gain and loose hydrogen?

A

Loose: OH-

Gain: H3O+

In neutral solutions the ratio of gaining and loosing hydrogen is equal*

25
Q

What equation is used to determine the concentration/ PH of hydrogen ions when given the PH/Concentration?

A

(H+) = 10 -PH

Example:

(Determining Concentration)

A solution has a PH of 6 and (H+) = 10 -6 mol/L

1 X 10-6 mol/ L

OR

(Determining PH)

A solution has a concentration of 10-3 mol/L

PH=3

26
Q

What are the classifications on the PH scale?

A

PH less than 7= Acidic

PH equal to 7= Neutral

PH greater than 7= Basic (Alkaline)

27
Q

What are the products when acids react with the following:

a) Active Metals
b) Carbonates
c) Bases

A

a) Salt and Hydrogen Gas
b) Salt, Carbon Dioxide Gas, and Water
c) Salt and Water

28
Q

Titration

A

The presice adddition of a solution in a buret into a measured volume of a sample solution.

29
Q

Titrant

A

The solution in a buret during titration. The concentration of this solution is accurately know. It is called standard solution.

30
Q

Sample

A

The solution being analized in a titration.

31
Q

Acid-Base Indicator

A

Signals the end of the titration by sharply and permanently changing colour when the equivalence point is reached.

Example: Phenolphthalein

32
Q

Endpoint

A

A change is physical appearance that indicated a complete reaction.

33
Q

Saturated Solution

A

A solution that cannot dissolve more solute.

34
Q

Unsaturated Solution

A

A solution that could dissolve more solute.

35
Q

Supersaturated Solution

A

A solution that contains more dissolved solute than a saturated solution at the same temperature.

36
Q

What are the 3 ways temperature can affect solubility?

A

1) Solbility decreases with an increase in temperature
2) Molecules in a gas state have more kinetic energy than those in a iquid state
3) Heating a solution provides more energy to the gas molecules and they escape from the liquid (Ex: Flat Pop)

37
Q

What are the 3 ways pressure affects solubility?

A

1) Pressure is the force per unit area
2) Pressure has a very little effect on the solubility of a liquid or solid but a signifcant difference on gas
3) The solubility of a gas in a liquid is proportional to the pressure of that gas above the liquid but is not affected by the pressure of any other gas

38
Q

What are the factors that affect the rate of dissolving?

A

1) Temperature
2) Agittation or Mixing
3) Surface Area

Chemistry Exam GR 11 (6 decks)

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