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Bioenergetics > Week 2 - Acid & Base Balance > Flashcards

Week 2 - Acid & Base Balance Flashcards

1
Q

Define an ionic bond

A

Complete transfer of e- between atoms.

Type of chemical bond generating 2 oppositely charged ions.

Very strong, difficult to break.

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2
Q

What happens in an ionic bond?

A

Metal loses e- to become a +ively charged CATION.

Nonmetal accepts e- to become a -ively charged ANION.

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3
Q

Bonds of salts + acids + bases

A

Salts – Ionic bonds

Acids + bases - Covalent bonds

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4
Q

Purpose of salts vs acids + bases

A

SALTS

  • Structural components
  • Electrolyte properties

ACIDS + BASES

  • Metabolic control
  • Homeostasis
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5
Q

What happens to both salts, acids + bases in water?

A

They dissociate

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6
Q

Which out of acids + bases are the proton donors + the proton acceptors?

A

Acids - proton donors

Bases - proton acceptors

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7
Q

What happens when acids dissociate in H20

A

They release H+.

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8
Q

What is the general formula of what happens to acids + give an example

A

Acid —> proton + anion (into solution).

HCL —> H+ + Cl-

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9
Q

Give 3 examples of acids in the human body

A

HCL (for digestion)

Carbonic acid (chemical buffering)

Citric acid (2nd stage of CHO breakdown).

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10
Q

Compare strong acids to weak acids

A

STRONG vs WEAK

Dissociate completely — Reach equilibrium

Irreversible — Reversible + conc. driven

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11
Q

Give an example of a strong acid

A

HCL

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12
Q

Give an example of a weak acid

A

Carbonic acid

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13
Q

What happens when bases dissociate in H20

A

Release OH-

hydroxyl group

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14
Q

Give the general equation for a base

A

Base —> Hydroxyl ion + cation

NaOH —> OH- + Na+

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15
Q

What can concentration be shown as?

A

Moles per litre

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16
Q

What is the potential of hydrogen (pH)?

A

Quantitive measure of the acidity or alkalinity of a solution.

17
Q

How is pH calculated

A

As a -ive logarithm to base 10 of H+ conc in a given solution.

-log(10)[H+]

18
Q

Define buffering

A

Chemical + physiological mechanisms that moderate changes in [H+]

19
Q

What pH does arterial blood have + what can it lead to if it ranges from those values?

A

7.35-7.45

Acidosis or alkalosis

20
Q

Properties of chemical buffers

A

Immediate response

Reversible

Catalysed by enzymes

21
Q

Properties of physiological buffers

A

2nd line of defence: Pulmonary/ventilatory + renal systems

22
Q

How long can renal buffering take

A

Hours to days

23
Q

Renal buffering

A

Renal tubules regulate acidity through complex chemical reactions that restore bicarbonate blood.

Only pathway to eliminate acids other than carbonic acid

Excretion of H+

Urine acidity or a alkalinity refletcs [H+].

24
Q

How long can ventilatory/pulmonary buffering take

A

Fast response – important during exercise

25
Q

Ventilatory/Pulmonary buffering

A

Changes CO2 conc.

⬆️ H+ stimulates the ventilatory control

⬆️ alveolar ventilation

⬆️ CO2 removal

26
Q

Equation for when carbonic acid donates a H+

A

H2CO3 —> H+ + HCO3-

27
Q

What is the role of a weak base

A

To mop up H+ so reaction becomes reversible.

28
Q

What are the possible variations in arterial blood?

A

PO2

PCO2

pH

Temp

29
Q

What is one of the factors that regulates ventilation?

A

Plasma pH

30
Q

What are the forms of metabolic alkalosis

A

Diuretics

Overactive adrenal gland

Loss of acids through stomach drainage

31
Q

What are the forms of respiratory alkalosis

A

Hyperventilation

32
Q

What are the forms of metabolic acidosis

A

Lactic acidosis

Build up of ketones

Kidney malfunction

Lung malfunction

Loss of bases through digestive tract

33
Q

What are the forms of respiratory acidosis

A

Hypoventilation

34
Q

What are the acid-base imbalances caused by intense exercise

A

Large temp disturbance

Low plasma pH = nausea, headache…

Bioenergetics (12 decks)

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