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Gr 12 Chemistry > Acid-Base Equilibria > Flashcards

Acid-Base Equilibria Flashcards

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1
Q

tastes sour and causes dyes to change colour

A

Acids

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2
Q

tastes bitter and feels soapy

A

Base

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3
Q

increases [H+] when dissolved in solution

A

Arrhenius Acid

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4
Q

increases [OH-] when dissolved in solution

A

Arrhenius Base

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5
Q

H+ donor; donates a proton

A

Bronsted-Lowry Acid

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6
Q

H+ acceptor; accepts a proton

A

Bronsted-Lowry Base

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7
Q

two formulas that differ by H+

A

Conjugate Acid-Base Pair

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8
Q

Conjugate ___ of a/an ___ has one fewer H+

A

base; acid

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9
Q

Conjugate ___ of a/an ___ has one more H+

A

acid; base

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10
Q

substance is one which can both donate and accept protons/hydrogen ions

A

Amphiprotic

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11
Q

substances has reactions as both acid and base

A

Amphoteric

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12
Q

All ____ substances are ____, but not all ____ substances are ____.

A

amphiprotic; amphoteric; amphoteric; amphiprotic

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13
Q

in water, few molecules act as bases and few act as acids

A

autoionization of water

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14
Q

Ion Product Constant (Kw)

A

Kw) = 1.0×10^(-14)

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15
Q

[H+] and [OH-] if a solution is neutral

A

[H+] = [OH-]

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16
Q

[H+] and [OH-] if a solution is acidic

A

[H+] > [OH-]

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17
Q

[H+] and [OH-] if a solution is basic

A

[H+] < [OH-]

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18
Q

formula for calculating pH

A

pH = -log[H+]

19
Q

formula for calculating [H+]

A

[H+] = 10^(-pH)

20
Q

formula for calculating pOH

A

pOH = -log[OH-]

21
Q

formula for calculating [OH-]

A

[OH-] = 10^(-pOH)

22
Q

relationship between pH and pOH

A

[H+][OH-] = 1.0×10^(-14)

pH + pOH = 14.00

23
Q

uses electrodes to indicate small changes in voltage to detect pH for accurate measurements

A

pH meter

24
Q

give less accurate, but quick measurements; compound that has one colour in its acid form and another in its basic form

A

indicators

25
Q

What are the common strong acids?

A

HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4

26
Q

donates only one proton

ex: HCl, HBr, HI, HNO3, HClO3, HClO4

A

monoprotic

27
Q

donates two protons

ex: H2SO4

A

diprotic

28
Q

What are the common strong bases?

A

KOH, NaOH, Ba(OH)2, CsOH, Sr(OH)2, LiOH

29
Q

strongest acid that can exist in an aqueous solution

A

H3O+

30
Q

strongest base that can exist in an aqueous solution

A

OH-

31
Q

formula for percent ionization

A

[H+]eq/[HA]initial × 100

32
Q

Relationship between KA and Kb

A

Ka × Kb = 1.0×10^(-14)

33
Q

shift in equilibrium causes by the addition of a compound having an ion in common with the dissolved substance

A

the common ion effect

34
Q

resist a change in pH when small amounts of a strong base or strong acid is added

A

buffer solutions

35
Q

Henderson-Hasselbalch Equation

A

pH = pKa + log([A-]/[HA])

[A-]/[HA] = antilog(pH-pKa)

*pKa = -log(Ka)

36
Q

technique used to determine the concentration of an unknown solution

A

Titration

37
Q

solution of a known concentration which is added to another solution whose concentration has to be determined

A

Titrant

38
Q

solution whose concentration has to be determined

A

Analyte or Titrand

39
Q

point at which the amount of titrant added is enough to completely neutralise analyte solution; moles of base is equal to the moles of acids and the solution only contains salt and water

A

equivalent point

40
Q

substance (weak acid or weak base) that is added to the analyte solution and changes colour at or near the equivalence point

A

indicator

41
Q

point at which indicator changes colour in an acid-base titration

A

end point

42
Q

equivalence point of strong acid and strong base titration

A

pH = 7

43
Q

equivalence point of weak acid and strong base

A

pH > 7

44
Q

equivalence point of strong acid and weak base titration

A

pH < 7

Gr 12 Chemistry (1 decks)

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