Lecture 10_190626

Question 1

Le Chatelier’s principle

Answer 1

aA + bB ↔ cC + dD

Keq = [Ceq]^c * [Deq]^d / [Aeq]^a * [Beq]^b

CO2 + H2O ↔ H+ + HCO3

Keq = ([H+eq] * [HCO3- eq]) / ([H2Oeq] * [CO2 eq])

M + W ↔ MW

Keq = [MWeq] / ([Meq] * [Weq])

Question 2

pH

Answer 2

= -log[H+]

Question 3

Dissociation of Water

Answer 3

H2O ↔ H+ + OH

Keq = [H+] * [OH-] / [H2O]

[H+] * [OH-] = [H2O] * Keq
= 55.5M * 1.8 X 10–16 M (@25deg) = 1.0 X 10-14M^2

[H+] = [OH-], so [H+]^2 = 1.0 X 10-14M^2

[H+] = square root 1.0 X 10-14M^2

For pure water, [H+] = [OH-] = 1.0 X 10–7 M

pH = -log[1.0 X 10–7] = 7 for pure water (neutral) @ 25°C

Question 4

Acid

Answer 4

molecule that donates an H+ in solution

“HA” ↔ H+ + A
Examples, HCl, H2SO4, H3PO4, CH3COOH

Question 5

Strong acid

Answer 5

is any acid that ionizes completely in solutions. This means it gives off the greatest number of hydrogen ions or protons when placed in a solution. Ions are charged particles.

7 strong acids
hydrochloric acid. HCL.
hydrobromic acid. HBr.
Hydroiodic acid. HI.
Nitric acid. HNO3.
Perchloric acid. HClO4.
Sulfuric acid. H2SO4.
Chloric acid. HClO3.

Question 6

Weak acid

Answer 6

is an acid that is partially dissociated into its ions in an aqueous solution or water.

Question 7

Conjugate acid

Answer 7

H+ + B ↔ “HB+”

Question 8

Strong and Weak bases

Answer 8

a strong base is a base that is 100% ionized in solution. If it is less than 100% ionized in solution, it is a weak base.

Question 9

Strong and Weak bases

Answer 9

a strong base is a base that is 100% ionized in solution. If it is less than 100% ionized in solution, it is a weak base.

LiOH - lithium hydroxide
NaOH - sodium hydroxide
KOH - potassium hydroxide
RbOH - rubidium hydroxide
CsOH - cesium hydroxide
*Ca(OH)2 - calcium hydroxide
*Sr(OH)2 - strontium hydroxide
*Ba(OH)2 - barium hydroxide

Question 10

Dissociation of a weak Acid

Answer 10

HA ↔ H+ + A

Keq = [H+] * [A-] / [HA] = Ka

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

-log[H+] = -log(Ka * [HA] / [A-])

pH = – log(Ka) – log([HA] / [A-])

pH = – log(Ka) + log([A-] / [HA])

pKa = -log[Ka]

Question 11

Henderson-Hasselbalch equation

Answer 11

pH = pKa + log([A-] / [HA])

Question 12

Calc pH

Answer 12

HCO3?

CO2?

Question 13

SLIDES 7-12

Answer 13

Know these concepts!!!

Question 14

Acid-base regulation

Answer 14

CO2 + H2O → H2CO3 → H+ + HCO3- → H2CO3 → H2O + CO2

CO2 + H2O → H2CO3 = cellular respiration (tissue)
Carbonic Acide Anhydrase
H+ increase
HCO3- increase
pH decrease

H+ + HCO3- = renal & gi

H2CO3 → H2O + CO2 = exhalation (lungs)
H+ decrease
HCO3- decrease
pH increase

Question 15

Acid-base regulation

Answer 15

CO2 + H2O → H2CO3 → H+ + HCO3- → H2CO3 → H2O + CO2

CO2 + H2O → H2CO3 = cellular respiration (tissue)
Carbonic Acide Anhydrase
H+ increase
HCO3- increase
pH decrease

blood = H+ + HCO3- = renal & gi

H2CO3 → H2O + CO2 = exhalation (lungs)
H+ decrease
HCO3- decrease
pH increase

Question 16

Acid-base regulation and the Davenport diagram

Answer 16

CO2 + H2O → H+ + HCO3-

???pH = 6.1 + log([HCO3-] / [0.03 * PCO2])???

SLIDE 14, 19-21, 27!!!

Question 17

Buffering of hydrogen with hemoglobin and carbon dioxide (CO2) transport.

Answer 17

SLIDE 15!!!

Question 18

Integration of pH Control Mechanisms

Answer 18

SLIDE 16!!!

Question 19

Renal excretion of acid

Answer 19

SLIDE 17!!!

Question 20

Respiratory acidosis

Answer 20

↑CO2 = ↓pH, ↑HCO3-

Renal compensation = ↑HCO3

Result = ↑CO2, ↑↑HCO3, ~pH

Question 21

Metabolic acidosis

Answer 21

↓HCO3 or ↑H+ = ↓pH, ↓HCO3-

Respiratory compensation = ↓CO2

Result = ↓HCO3-, ↓CO2, ~pH

Question 22

Respiratory alkalosis

Answer 22

↓CO2 = ↑pH, ↓HCO3-

Renal compensation = ↓HCO3

Result = ↓↓HCO3-, ↓CO2, ~pH

Question 23

Metabolic alkalosis

Answer 23

↑HCO3 or ↓H+ = ↑pH, ↑HCO3-

Respiratory compensation = ↑CO2

Result = ↑CO2, ↑HCO3, ~pH

Question 24

Respiratory acidosis with compensation

Answer 24

SLIDE 23!!!

Question 25

Respiratory alkalosis with compensation

Answer 25

SLIDE 24!!!

Question 26

Metabolic acidosis with compensation and correction

Answer 26

Anion gap = (Na+ - (Cl- + HCO3-))
High AG → addition of acid 
*Cl- decrease or ?gap increase?
Normal AG → loss of base
*HCO3- decrease = ?gap decrease? or Cl- increase

SLIDE 25!!!

Question 27

Metabolic alkalosis with compensation and correction

Answer 27

SLIDE 26!!!

Question 28

Hypochloremic metabolic alkalosis

Answer 28

SLIDE 28!!!

Question 29

9 Conditions of van Slyke

Answer 29

SLIDE 29!!!

Question 30

Acute respiratory acidosis

Answer 30

= ↑CO2 = ↓pH, ↑HCO3-

BE = Normal

Question 31

Chronic respiratory acidosis

Answer 31

= ↑CO2 = ~pH, ↑↑HCO3-

BE = Positive (> +2)

Question 32

Acute metabolic acidosis

Answer 32

= ↓HCO3 or ↑H+ = ↓pH, ↓HCO3-

BE = Negative (< -2)

Question 33

Chronic metabolic acidosis

Answer 33

= ↓HCO3 or ↑H+ = ~pH, ↓HCO3-, ↓CO2

BE = Negative (< -2)

Question 34

Acute respiratory alkalosis

Answer 34

= ↓CO2 = ↑pH, ↓HCO3-

BE = Normal

Question 35

Chronic respiratory alkalosis

Answer 35

= ↓CO2 = ~pH, ↓↓HCO3-

BE = Negative (< -2)

Question 36

Acute metabolic alkalosis

Answer 36

= ↑HCO3 or ↓H+ = ↑pH, ↑HCO3-

BE = Positive (> +2)

Question 37

Chronic metabolic alkalosis

Answer 37

= ↑HCO3 or ↓H+ = ~pH, ↑HCO3-, ↑CO2

BE = Positive (> +2)