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Chemistry 115 > Chapter 16 > Flashcards

Chapter 16 Flashcards

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1
Q

Buffer

A

A solution that resists pH changes when an acid or base is added

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2
Q

Neutralize added acid or base

A

Buffer solution

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3
Q

Acid buffer

A

Significant amount of weak acid and its conjugate base

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4
Q

Base buffer

A

Significant amount of weak base and its conjugate acid

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5
Q

Creating an acid buffer

A

Significant amounts of weak acid plus the conjugate base salt

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6
Q

Henderson-Hasselbalch equation

A

Calculating pH using Ka and initial acid/base concentrations

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7
Q

pH changes of a buffer solution

A

Use a before and after table with proper stoichiometry to find new acid/base concentrations, then the HH equation

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8
Q

Creating a base buffer

A

Weak base and its conjugate acid salt

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9
Q

Buffer effectiveness

A

Buffer have a limit in the amount of acid or base that they can neutralize

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10
Q

Buffer effectiveness factors

A

Relative amounts (1:1)
Absolute concentrations (larger)

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11
Q

Buffering capacity

A

The amount of acid or base that a buffer can neutralize

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12
Q

Buffering range

A

The pH range where the buffer is effective

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13
Q

Effective buffer range

A

pH varies from pKa by +/- 1

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14
Q

Effective buffer concentrations

A

Acid and base are within a factor of 10

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15
Q

When choosing which acid to make a buffer

A

chose the one with the pKa closest to the pH

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16
Q

Amount of avid or base that can be added to a buffer without destroying its effectiveness

A

Buffer capacity

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17
Q

Buffer capacity increases

A

With increasing concentration of the buffer components and as the acid base ratio approaches 1:1

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18
Q

Titration

A

Reaction where acid has neutralized base or vice versa

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19
Q

Titrant

A

In burette, added to analyze in flask

20
Q

Analyte

A

Solution in flask, titrant added to it

21
Q

Point where a titration is complete

A

Equivalence point

22
Q

Equivalence point

A

Mols of acid stoichiometrically matches the mols of base

23
Q

Ways to measure pH

A

pH metre or indicator

24
Q

Titration curve

A

pH versus volume of titrant added

25
Q

Inflection point on the titration curve

A

The equivalence point of the titration

26
Q

pH at equivalence point

A

Varies based on strength of acid or base added

27
Q

Strong acid-base titration curve

A

Rapid change in pH near equivalence point (10 pH units)

28
Q

pH calculations along the titration curve

A

Vary based on pint in titration and if the titrant is an acid or a base

29
Q

Polyprotic acid titration

A

Multiple equivalence points
Ka1 is higher then Ka2

30
Q

Volume of base in Polyprotic acid titration

A

Volume of base added from start to equivalence point 1 is the same as the volume between equivalence points

31
Q

What is an indicator

A

Weak organic acid dye
A buffer
Water soluble

32
Q

Flaws of an indicator

A

They are subjective, people see differently
Must go to end point (past equivalence, excess titrant)

33
Q

End point

A

Change in pH shown by an indicator, past the equivalence point

34
Q

Equivalence point

A

Mols of acid stoichiometrically matches mols of base

35
Q

When is the end point reached

A

An indicator has slightly and permanently changed colour

36
Q

pKa of indicator is equal to

A

pH at equivalence point

37
Q

Insoluble ionic compounds

A

Dissolve very little
Have Ksp

38
Q

Ksp

A

Solubility product constant
A type of Keq

39
Q

Solubility

A

Quantity of compound dissolved in a specific amount of liquid

40
Q

Solute

A

The compound or substance that is being dissolved

41
Q

Solvent

A

What is dissolving the solute
Often water

42
Q

Molar solubility

A

S
Molarity of dissolved solute in a saturated solution
Units: mol/L

43
Q

Relative solubility

A

Comparing Ksp’s of compounds
ONLY WHEN STOICHIOMETRY IS THE SAME

44
Q

Common ion solubility

A

Addition of soluble salt containing one of the ions of the insoluble salt deceased solubility

45
Q

Insoluble ionic hydroxide solubility

A

Higher pH leads to lower solubility
Lower pH leads to higher solubility

46
Q

Insoluble ionic weak acid anion solubility

A

Lower pH leads to higher solubility

Chemistry 115 (8 decks)

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