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Physical chemistry. > 3.1.12 Acids and bases > Flashcards

3.1.12 Acids and bases Flashcards

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1
Q

Bronsted-Lowery Acid:

A

Dontate protons.

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2
Q

Bronsted-Lowery Base:

A

Accept protons.

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3
Q

What ion causes a solution to be acidic?

A

H+ ions or H3O+

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4
Q

What causes a solution to be alkaline?

A

OH- (hydroxide ion)

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5
Q

EQUATION pH

A

pH = -log10[H+]

[H+] = hydrogen ion concentration.

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6
Q

Strong acid:

A

fully dissociates in water
HX -> H+ + X-

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7
Q

Examples of strong acids:

A

HCl, H2SO4, H3PO4

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8
Q

Examples of weak bases:

A

CH3COOH, any organic acid.

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9
Q

What is the concentration of hydrogen ions in a monoprotic strong acid?

A

It will be the same concentration as the acid.

0.1moldm3 HCl the pH will be -log10[0.1] = 1.00

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10
Q

EQUATION: Find [H+] from pH

A

[H+] = 1 x 10 ^ -pH

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11
Q

EXAMPLE: STRONG ACID calculate the concentration of HCl with pH of 1.35.

A

[H+] = 1 x 10^-1.35
0.045 moldm-3

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12
Q

What is the relationship between pH and concentration of H+?

A

lower pH = high concentration of H+

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13
Q

If two solutions have a difference of 1, what is the difference in [H+]?

A

factor of 10.

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14
Q

Why is pure water neutral?

A

[H+(aq)] = [OH-(aq)]

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15
Q

EQUATION Kw

A

Kw= 1 x 10-14 (at 25 * C)

Kw = [H+(aq)]^2

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16
Q

Example 2: Calculate the pH of water at 50ºC given that Kw = 5.476 x 10-14 mol2 dm-6 at 50ºC

A

[H+(aq) ] = √ Kw = √ 5.476 x 10-14 =2.34 x 10-7 mol dm-3

pH = - log 2.34 x 10-7 = 6.63

It is still neutral though as [H+(aq) ] = [OH-(aq)]

17
Q

What is the effect of temperature on the pH of pure water?

A

At different temperatures to 25 * C the pH of pure water changes.

Dissociation of water is endothermic so increasing the temperature = equilibrium would move to the right giving a bigger concentration of H+ ions and lower pH.

18
Q

How can you calculate pH from Kw?

A

Kw = 1.00 x 10-14

[H+]^2 = Kw
[H+] =

Physical chemistry. (13 decks)

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