The Significance of pH๐Ÿงช Flashcards

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1
Q

Where are Buffers important?

A

In living systems

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2
Q

State 2 functions of buffers in the body?

A

-Maintain pH of the body within normal pH ranges
-Ensure enzymes and other cellular processes function optimally

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3
Q

What are the normal pH values of the following substances in the body?

Blood?
Urine?
Gastric Fluid?
Saliva?

A

Blood- 7.4
Urine- 6.0 (range 4.4-8.0)
Gastric Fluid- 2.0
Saliva- 6.2- 7.2

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4
Q

Name the two major inorganic buffers in the body and their function

A

Phosphate- Buffer Reserve in Skeleton
Bicarbonate- Major Buffer in Human Body

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5
Q

Name an organic buffer in the body

A

Macromolecules i.e. amino acid side chais in proteins- can also act as buffers

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6
Q

Name an organic buffer in the body

A

Macromolecules i.e. amino acid side chais in proteins- can also act as buffers

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7
Q

Many molecules in biological Systems are what?
And what are their ionic properties Influenced by?

A

Many molecules in biological systems are weak acids and/or weak bases

Their ionic properties are influenced by their hydrogen ion concentration [H+]

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8
Q

How would you calculate the pH of a STRONG ACID?

A

pH= -log[H+]

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9
Q

What happens when acids dissociate?

A

They release [H+] ions

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10
Q

What is an acid?

A

A substance that will dissociate in water to produce [H+] ions

-PROTON DONATOR

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11
Q

What is a base?

A

A substance which in water tends to combine with [H+] ions

-PROTON ACCEPTOR

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12
Q

Write an equation to demonstrate the dissociation of acids

A

A <โ€”โ€”โ€“> H+ + B-
acid conjugate base

In water;

HA + H20 โ€”โ€”โ€”> H30+ + A-
acid water con. acid con.base

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13
Q

A โ€”โ€”โ€”> H+ + B-

This equilibrium reaction always involves what?

A

A conjugate acid-base pair, comprising a hydrogen ion (acid) donor and an acceptor (base)

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14
Q

For the dissociation constant of an acid, how is the forward reaction balanced?

A

By the reverse reaction

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15
Q

A <โ€”โ€”โ€“> H+ + B-
Describe the concentrations of A, H+ and B- when an equilibrium is established?

A

The ratio of the concentrations of H+ and B- to A is constant when an equilibrium is established

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16
Q

What equation is used to calculate the acid dissociation constant?

A

For A <โ€”โ€”โ€“> H+ + B-

Ka= [H+][B-]
โ€”โ€”โ€”โ€”
[A]

17
Q

A <โ€”โ€”โ€“> H+ + B-

Describe what happens to the value of K as the strength of the acid increases

A

As the strength of the acid increases, the higher the degree of dissociation so the value of K increases as the reaction is pushed to the right, producing more conjugate base

18
Q

What is the Henderson- Hasselbalch Equation?

A
19
Q

How would you calculate pKa if given the value of Ka

A

pKa = -logKa

20
Q

Describe the relationship between acid strength and Ka

A

Directly Proportional
-As the strength of the acid increases so does the value of Ka
-The larger the value of Ka the smaller the pH

21
Q

Describe the relationship between acid strength and pKa

A

-Inversely Proportional
-As the strength of the acid increases the value of pKa decreases
-The larger the value of pKa the higher the pH

22
Q

What are indicators?

A

Weak acids or bases which have a distinct colour difference between their ionised form (In-) and their unionised form (HIn).

e.g. HIn- colourless
In- - red

23
Q

The degree of dissociation and pH of indicators are related by what equation?

A

pH= pKa + log [In-]
โ€”โ€”
[HIn]

24
Q

Why is very little indicator added to solutions?

A

So that the pH of the solution is unaffected

25
Q

How is the ratio of [In-]/[HIn] determined?

A

By the pH

26
Q

What determines the colour of the indicator?

A

The ratio of [In-]/[HIn]

27
Q

How can you measure the pH of a solution based on the colour of the indicator solution?

A

When either the ionised, or unionised form of the indicator is coloured, the depth of colour for the given amount of indicator can be used to measure pH

28
Q

What is an electrical method of measuring pH?

A

-pH meter

29
Q

Describe what a pH meter is

A

-Measurement made using a glass electrode
-Glass electrode- thin walled glass bulb containing a platinum electrode immersed in 1M Hal

30
Q

What do buffer solutions do?

A

Resist changes in pH when acid or base is added

31
Q

What do buffer solutions consist of?

A

A conjugate acid-base pair of either a weak acid or weak base

32
Q

Buffering systems in the body play a vital role in what?

A

Maintaining pH homeostasis

33
Q

What does buffering in the oral cavity limit?

A

pH changes caused by acid production by plaque bacteria

34
Q

Using the Henderson Hasselbalch Equation;

pH = pKa- log [Acid]
โ€”โ€”โ€“
[Base]
When is optimum buffering capacity?

A

-It can be shown that buffering is most effective when [Acid]= [Base]

  • [A]=[B] so log(1)=0 hence pH=pKa

-Buffers operate optimally at their pKa ie when HALF DISSOCIATED (as [A]=[B])

-At optimum buffering capacity pH=pKa

35
Q

Describe how plaque bacteria results in dental caries

A

-Plaque Bacteria ferment dietary carbohydrates to produce acid
-This causes plaque pH to fall
-Leading to increased solubility of Dental Enamel
-Which if not reversed leads to Dental Caries

36
Q

Describe how Saliva prevents Dental Caries

A

-Saliva acts as a buffer and neutralises the acid produced by plaque bacteria and thereby prevents dental caries (if buffering is adequate)

37
Q

Where is bicarbonate an important buffer?

A

Extremely important buffer in body fluids such as blood

38
Q

What proteins does saliva contain?

A

Unusual Proteins that are histadine rich and are known as histatins; these too are important buffers in saliva

39
Q

What is Histadine?

A

An amino acid which is very good at acting as a buffer