12P- Acids And Bases Flashcards

1
Q

Definition of an acid

A

Proton donator

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2
Q

Definition of a base

A

Proton acceptor

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3
Q

What happens at an acid base equilibrium

A

The transfer of protons

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4
Q

Why is the pH scale logarithmic

A

pH scale measures H+ ion conc
In an aqueous solution H+ conc can cover a large range

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5
Q

Equation to calculate pH

A

-log[H+]

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6
Q

Equation to calculate H+ conc

A

[H+]= 1x 10^-pH

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7
Q

How many decimal places is pH given to

A

2 dp ALWAYS

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8
Q

How to calculate pH of a strong acid when given its conc

A

Monoprotic acid, same [H+] in moles/conc
Diprotic acid, double [H+] in moles/conc

Sub this value into pH= -log[H+]

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9
Q

What happens when water is ionised

A

Disassociates slightly

H2O(l) <—> H+(aq) + OH-(aq)

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10
Q

How is Kw derived and what the equation

A

From equilibrium constant Kc

Kc= [H+][OH-]/ [H2O]
Kc[H2O]= [H+][OH-]
H2O is much larger than the conc of any of the ions, assume it’s value is constant, make LHS equal to Kw

Kw= [H+][OH-]

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11
Q

What effects the value of Kw

A

Temperature

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12
Q

How to is Kw to calculate the pH of a strong base from its conc

A

Value of Kw at specific temp should be given
Sub [OH-] into Kw eq, to find [H+]
Sub [H+] into pH eq

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13
Q

Definition of weak acids and weak bases

A

They disassociate slightly in aqueous solutions

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14
Q

What’s Ka and form an equation

A

Disassociation constant for a weak acid

HA(aq)—> H+(aq) + A-(aq)
Ka= [H+][A-]/[HA]

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15
Q

Equation for pKa

A

pKa= -log10(Ka)

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16
Q

What’s the value of Kw at room temp

A

1x10^-14 mol^2 dm^-6