Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
43 Cards in this Set
- Front
- Back
|
Metabolic processes result in production of large amounts of what? |
Carbonic acid, sulfuric acid, phosphoric acid |
|
|
An acid is a proton..? |
donor Donates H+ to solution |
|
|
A base is a proton..? |
acceptor Accepts H+ from a solution |
|
|
What is a strong acid and what are some examples? |
Dissociates quickly in solution, releasing H+
Ex: HCl, HNO3, H2SO4 |
|
|
What is a strong base and what are some examples? |
Reacts very quickly with H+ removing it from solution Ex: OH- (reacts with H+ to form H2O) |
|
|
What type of acids are involved in acid-base balance? |
weak acids and bases *weak acid only partially dissociates (H2CO3) *weak base does not fully ionize in solution (HCO3) |
|
|
What are protons (H+ ions) normally bound by to H2O? |
electrostatic interaction |
|
|
What is acidity related with? |
H+ concentration |
|
|
Why are there significantly less of H+ ions compared to electrolytes? |
Because H+ ions are highly reactive and proteins in the body have many dissociable groups so alterations in charge or configuration can alter protein structure and function |
|
|
What should be kept constant for enzyme function and cellular structure? |
H+ concentration of body fluids |
|
|
What is the definition of pH? |
negative base 10 logarithm of the H+ ion concentration pH=-log10[H+] |
|
|
What determines the pH of body fluids? |
H+ ion concentration |
|
|
What is the normal extracellular fluid [H+]? |
40nEq/L (7.398-->blood pH) |
|
|
In pure water what are the amounts of H+ and OH-? |
There are the same amount of each, making the pH neutral (7) |
|
|
What is the inverse relationship between pH and [H+]? |
the greater the [H+], the lower the pH (acidemia) the lower the [H+], the higher the pH (alkalemia) |
|
|
What is acidemia? |
decrease in ECF pH below normal limits H+ ion conc. is above normal limits |
|
|
What is acidosis? |
the processes that cause net accumulation of acid in the body usually caused by disease |
|
|
What is alkalemia? |
increase in ECF pH above normal limits H+ ion conc. is below normal limits |
|
|
What is alkalosis? |
the processes that cause net accumulation of alkali in the body usually caused by diease |
|
|
An animal can have alkalosis without alkalemia? |
True |
|
|
What does pH and [H+] look like on a graph together? |
they vary exponentially, not linearly (curved line) |
|
|
What is the law of mass action? |
The velocity of a reaction is proportional to the product of the concentrations of the reactants. |
|
|
What are the two opposing reactions of the law of mass action and what is their velocity? |
HA---> H+ + A- H+ = A- ---> HA V1=K1[HA] V2 =K2[H+][A-] ** velocity is written based on the left side of the equation |
|
|
What happens to the rates of the opposing reactions when they are at equilibrium? |
They exactly counterbalance one another and their velocities are equal |
|
|
What is the Ka (dissociation constant)? |
The concentration of the acid relative to its dissociation ions |
|
|
What is pKa? |
the negative logarithm of the dissociation constant of a weak acid OR the pH at which an acid is half dissociated, existing equal proportions of acid and conjugate base |
|
|
What is the Henderson-Hasselbach equation? |
Defines the determinants of normal pH regulation and acid-base balance in ECF Also provides insight into the physiological control of acid and base composition of the ECF pH=pka + log (base/acid) |
|
|
What is a buffer? |
a compound that can accept or donate protons (H+ ions) and minimize a change in pH |
|
|
Where are blood buffers and what do they do? |
Present in the blood and are the first line of defense to prevent major changes in pH |
|
|
What happens when a strong acid is added to a buffer solution containing a weak acid and its conjugate base? |
the dissociated H+ from the strong acid are donated to the base and the change in pH is minimized |
|
|
Is it necessary to measure all components of every buffering system and why? |
No, because if one system is known, changes in other systems can be predicted |
|
|
What is the Isohydric principle? |
Multiple buffers in the same solution are always in equilibrium |
|
|
What is an example of serious deviations of pH disrupting cell metabolism? |
Some enzymes could reduce 90% activity with a change in pH by only 0.1 units |
|
|
What are the 3 systems that regulate H+ ion conc. and pH in body fluids? |
Chemical buffer systems (manage imbalance) Lungs Kidneys **Lungs and kidneys try to correct the pH by adjustments in ventilation or changes in renal function |
|
|
What does the HH equation look like using lung and kidney function? |
pH = pka + log [renal function/ventilation] [base/acid] [HCO3/PCO2] |
|
|
What do blood buffers do to the H+ ion? |
Keep them in control until balance is restored ***they dont add or remove H+ |
|
|
What are the 3 types of buffer systems? |
Proteins (hemoglobin, proteins---intracellular) Bicarbonate buffer system Phosphate buffer system |
|
|
What are the most plentiful buffers in the body and where are they important for? |
Proteins Intracellular acid-base balance |
|
|
Why are proteins buffers? |
Because they have a large number of acidic and basic groups Ex: imidazole ring of histidine residues, amino-terminal groups |
|
|
Why is hemoglobin a buffer? |
Important blood buffer together with bicarbonate buffer system readily available in the blood Has large number of acidic and basic groups |
|
|
How can hydrogen ions be accommodated by hemoglobin? |
by basic carboxyl groups: R-COO- + H+ <--> RCOOH by Imidazole groups of histidine: bond with iron on the heme groups |
|
|
What happens when arterial blood enters the tissue capillaries? |
oxygen leaves hemoglobin deoxyhemoglobin is an excellent buffer for the H+ produced when CO2 is added to the blood |
|
|
When both metabolic and respiratory levels are elevated what is happening? |
There is a metabolic alkalosis with compensatory respiratory acidosis (lungs are helping in alkalosis to increase the PCO2) |
