Chapter 21 Flashcards

1
Q

What is a buffer solution?

A

A buffer solution is a solution which resists changes in pH when small amounts of acids or alkalis are added. They are used to keep the pH almost constant.

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2
Q

What do buffer solutions consist of?

A

A buffer can consists of weak acid - conjugate base or weak base - conjugate acid

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3
Q

What does the weak acid do in a buffer solution?

A

Removes added alkali

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4
Q

What does the conjugate base do in a buffer solution?

A

Removes added acid

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5
Q

How does the ethanoic acid and sodium ethanoate buffer solution work?

A

Ethanoic acid is a weak acid and partially ionises in solution to form a relatively low concentration of ethanoate ions

Sodium ethanoate is a salt which fully ionises in solution

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6
Q

What happens when H+ ions are added to a buffer solution..? (acid)

A

Conjugate base removes the added acid.

The increased H+ reacts with the A- (conjugate base) and forms more HA until equilibrium is re-established. (equilibrium shifts to the left)

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7
Q

What happens when OH- ions are added to a buffer solution..? (alkali)

A

Weak acid removes added alkali

OH- reacts with H+ and forms water. More HA dissociates to restore some H+. So equilibrium shifts to the right.

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8
Q

How do you calculate the pH of a buffer solution?

A

H+ = Ka x [HA]/[A-]

The values of H+ and A- are no longer thought to be equal. (As A- is added as a component in the buffer solution)

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9
Q

What is the buffer system used to control blood pH?

A

The carbonic acid- hydrogen carbonate buffer system.
H2CO3 –> H+ + HCO3

Body cells produce CO2 during aerobic respiration
This CO2 will combine with water in blood to form a solution containing H+ ions
CO2 (g) + H2O (l) ⇌ H+ (aq) + HCO3- (aq)

This equilibrium between CO2 and HCO3- is extremely important
If the concentration of H+ ions is not regulated, the blood pH would drop and cause ‘acidosis’
Acidosis refers to a condition in which there is too much acid in the body fluids such as blood
This could cause body malfunctioning and eventually lead to coma

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10
Q

How does the carbonic acid- hydrogen carbonate buffer system react when OH- or H+ is added?

A

If H+ is added it reacts with the conjugate base HCO3- to form more HA (H2CO3) Equilibrium shifts to the left.

If OH- is added it reacts with H+ to form water. Then more H2CO3 dissociates to restore H+ and shifts equilibrium to the right.

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11
Q

What should the pH of blood be?

A

between 7.35 and 7.45

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12
Q

What shape is a pH curve?

A

A s shape.

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13
Q

What is the equivalence point of a titration?

A

The volume of one solution that exactly reacts with the volume of the other solution. It is the centre of the vertical section of the pH curve.

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14
Q

What is the end point of a titration?

A

The indicator contains equal amounts of the weak acid and conjugate base so the colour is in-between the two extremes.

eg methyl orange- HA is red, A- is yellow. End point is orange

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15
Q

How do you choose which indicator to use?

A

The indicator must have a colour change which coincides with the vertical section of the pH titration curve.

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15
Q

How do you choose which indicator to use?

A

The indicator must have a colour change which coincides with the vertical section of the pH titration curve.

16
Q

Example of strong acid?

A

HCL

17
Q

Example of strong base?

A

NaOH

18
Q

Example of weak acid?

A

CH3COOH

19
Q

Example of weak base?

A

NH3