Acids bases and buffers Flashcards

1
Q

what is a Bronsted Lowry acid ?

A

proton donor

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2
Q

what is a Bronsted Lowry base?

A

proton acceptor

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3
Q

Metal + acid

A

salt + hydrogen

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4
Q

metal oxide + acid

A

salt + water

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5
Q

metal hydroxide + acid

A

salt + water

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6
Q

metal carbonate + acid

A

salt + water + carbon dioxide

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7
Q

what is a conjugate pair?

A

a conjugate pair is linked by the transferring of a proton

  • conjugate acid is +
  • conjugate base is -
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8
Q

what is Kw?

A
  • ionic product of water

- Kw = [H+][OH-}

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9
Q

How to calculate the pH

A

pH = -log[H+]

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10
Q

How to calculate the [H+]

A

[H+] = 10^-pH

inverse of log

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11
Q

How to calculate pH of strong monobasic acids

A

[HA] = [H+]

use pH = -log[H+]

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12
Q

How to calculate pH of strong dibasic acids

A
[HA] = 2[H+]
pH = -log[H+ x2]
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13
Q

How to calculate pH of strong bases

A

[Base] = [OH-]

  • first find H+ using Kw/OH-
  • then find pH using -log[H+]
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14
Q

How to calculate the pH of a weak acid

A

Ka = [H+]^2 / [HA]

  • rearrange to find [H+] by doing square root of Ka*[HA]
  • calculate pH by doing -log[H+]
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15
Q

How to calculate pKa

A

pKa = -log(Ka)

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16
Q

how to calcualte Ka when you have pKa

A

Ka = 10^-pKa

17
Q

acid strength in pKa / Ka

A
  • high pH + low Ka = weaker acid

- low pH + high Ka = stronger acid

18
Q

Ka equation

A

Ka = [reactants] / [products]

19
Q

how to calculate H+ when you have Ka

A

[H+] = √Ka*[HA]