Lecture 10_190626 Flashcards
Le Chatelier’s principle
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])
pH
= -log[H+]
Dissociation of Water
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
Acid
molecule that donates an H+ in solution
“HA” ↔ H+ + A
Examples, HCl, H2SO4, H3PO4, CH3COOH
Strong acid
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.
Weak acid
is an acid that is partially dissociated into its ions in an aqueous solution or water.
Conjugate acid
H+ + B ↔ “HB+”
Strong and Weak bases
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.
Strong and Weak bases
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
Dissociation of a weak Acid
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]
Henderson-Hasselbalch equation
pH = pKa + log([A-] / [HA])
Calc pH
HCO3?
CO2?
SLIDES 7-12
Know these concepts!!!
Acid-base regulation
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
Acid-base regulation
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
Acid-base regulation and the Davenport diagram
CO2 + H2O → H+ + HCO3-
???pH = 6.1 + log([HCO3-] / [0.03 * PCO2])???
SLIDE 14, 19-21, 27!!!
Buffering of hydrogen with hemoglobin and carbon dioxide (CO2) transport.
SLIDE 15!!!
Integration of pH Control Mechanisms
SLIDE 16!!!
Renal excretion of acid
SLIDE 17!!!
Respiratory acidosis
↑CO2 = ↓pH, ↑HCO3-
Renal compensation = ↑HCO3
Result = ↑CO2, ↑↑HCO3, ~pH
Metabolic acidosis
↓HCO3 or ↑H+ = ↓pH, ↓HCO3-
Respiratory compensation = ↓CO2
Result = ↓HCO3-, ↓CO2, ~pH
Respiratory alkalosis
↓CO2 = ↑pH, ↓HCO3-
Renal compensation = ↓HCO3
Result = ↓↓HCO3-, ↓CO2, ~pH
Metabolic alkalosis
↑HCO3 or ↓H+ = ↑pH, ↑HCO3-
Respiratory compensation = ↑CO2
Result = ↑CO2, ↑HCO3, ~pH
Respiratory acidosis with compensation
SLIDE 23!!!
