A2 PH - DEFINING ACIDS ] Flashcards

1
Q

The Brnnsted-Lowry description of acidity

A

An acid is a molecule which donates a proton and a base accept the base

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2
Q

Monoprotic Acid

A

donates one proton

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3
Q

Diprotic acid

A

donates 2 protons

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4
Q

Water can act as

A

a base and a acid

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5
Q

H3O +

A

H30 + is called the oxon ium ion, but the names hydronium ion and

hydroxonium ion are also used.

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6
Q

Why is H+ Called a proton

A

it has lost a electron, therefore this means that it only has a proton in the nucleus as no neutrons are present

since there is no electrons they can never give electrons only accept electrons

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7
Q

Water is slightly ionised:

A

This means it existed as this in equilibrium
H20(l) .- H+(aq) + oH-(aq)

It can also be written in the form

H20(l) + H20(1) …- H 30•(aq} + OH-(aq)

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8
Q

Kw

A

The equilibrium constant, Kw, is called the dissociation constant or ionization constant of water.

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9
Q

In pure water what is The Kw constant

A

1.00x10-7 M.

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10
Q

More kw

A

Kw is called the ionic product of water and at 298k it is equal to
1.0 x 10-14 mol 2 dm-6 • Each H20 that dissociates (splits up) gives rise
to one H+ and one oH- so. in pure water, a t 298 K :

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11
Q

why is water always at a constant

A

Because equilibrium lies to the left a lot there is a small value of ions so water is at a constant

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12
Q

at 298k water

A

it is 1 x 10-14

what is the Ph value since dissociation is one to one
h+ is 1 x10-7
so Ph is 7 in pure water - our interpretation of neutral

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13
Q

at 373k water

A

it has a Ph of 6.14
it appears acidic
the charges balance out so it is neutral Ph
the neutral point has changed.

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14
Q

What does a proton exist as

A

the proton does not exist in itself but rather it interacts with water to form H30+

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