Acids and Bases (Physical) Flashcards

1
Q

Define Bronsted-Lowry acid
Define Bronsted-Lowry base
Define the reaction between the two.

A
  • acid: proton donor
  • base: proton acceptor
  • reaction: reaction involving the transfer of a proton.
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2
Q

Define:
- Monoprotic acid
- Diprotic acid
- Triprotic acid

A
  • mono- acid that releases one H+ ion per molecule.
  • do- acid that releases two H+ ions per molecule.
  • tri- acid that releases three H+ ions per molecule.
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3
Q

Give the definition of pH.

A

-log[H+]

(2d.p)

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4
Q

Equation to find the concentration of H+ ions in a solution once another solution is added.

A

[H+] in original solution x (old volume / new total volume)

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5
Q

Describe where Kw comes from.
What is the usual value for Kw at 298K?

A

Kw = Kc x [H2O]

  • During; H2O —(reversible symbol)-> OH- + H+ reaction there is so much water that [H2O] is seen as a constant value, while [H+] and [H2O] are variables.
  • As; Kc = ( [H+] x [OH-] ) / [H2O], therefore; Kc x [H2O] = [H+] x [OH-] and Kw = Kc x [H2O]
  • This means; Kw = [H+] x [OH-]

Kw = 1 x 10^-14 mol^2dm^-6

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6
Q

What is the effect of temperature on the pH and neutrality of water in terms of Kw?

A

H2O —(reversible symbol)-> OH- + H+ (—> exothermic)

  • As temperature increases, equilibrium shifts right to endothermic direction to oppose increase.
  • Therefore [H+] and [OH-] increase, Kw increases and pH decreases.
  • However water still neutral as [H+] = [OH-]
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7
Q

Give the definition of neutral

A

[H+] = [OH-]

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8
Q
A
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