Lab 1: homeostasis

how to measure pH of a solution

amount of hydrogen ions within that solution

pH of 7

neutral; H+ and OH- are equal

pH below 7

acid; more H+ ions than OH-

pH above 7

basic (alkaline); more OH- than H+

carbonic acid

one of the most important and frequently occurring

how is carbonic acid formed

when carbon dioxide (a waste produce of cellular respiration) reacts with water (in cells, blood, and fluid surrounding cells)

carbonic acid

weak acid

formula for carbonic acid formation

CO2 + H2O → H2CO3 → H + HCO3

homeostasis

the maintenance of a stable internal environment

acidosis

blood pH below 7.35

alkalosis

blood pH above 7.45

respiratory acidosis

insufficient exhalation of CO2

metabolic acidosis causes

ketoacidosis, losing too much bicarbonate, severe diarrhea, lactic acid, anaerobic respiration

ketoacidosis

the breakdown of fatty acids produces acidic ketone bodies, which lower the blood pH

respiratory alkalosis

too much CO2 is exhaled and the amount of carbonic acid decreases

metabolic alkalosis

caused by a drop in pH that is not associated with CO2 levels

metabolic alkalosis causes

excessive vomiting

buffer

resists changes in the pH of a solution by binding the ions produced by strong acids and bases

proteins that are good buffers

albumin and hemoglobin

strong acid formula

H + CL + Na + HCO → H2CO3 + Na + Cl

strong acid formula words

Hydrochloric acid + Sodium bicarbonate yields Carbonic acid and Sodium Chloride

strong base formula

Na + OH + H2CO3 → Na + HCO3 + H2O

strong base formula words

Sodium hydroxide + carbonic acid yields sodium bicarbonate and water

what happens when a strong acid is added to a solution

hydrogen ions are taken out of the solution by the buffer, preventing a drop in pH; sodium bicarbonate dissociates into sodium and bicarbonate ions. bicarbonate combines with hydrogen from the hydrochloric acid to form carbonic acid, a weak acid.

what happens when a strong base is added to a solution

hydroxide ions are taken out of solution by another component of the buffer. carbonic acid dissociates into hydrogen and bicarbonate ions. hydrogen ions combine with hydroxide ions from the sodium hydroxide to form water

sodium bicarbonate-carbonic acid buffer system

resists a pH change by removing either the hydrogen or hydroxide ions

sodium bicarbonate by itself will buffer

acids

carbonic acid by itself will buffer

bases

did the pH of the water change when acid was added

yes, it for more acidic as the HCL got added

did the pH of the water change when a base was added

yes, it got more alkaline as the NaOH was added

did the pH of the buffer solution change when an acid was added

there was no change

did the pH of the buffer solution change when a base was added

yes, it got slightly more alkaline

explain why the time decreased to change the color of the solution after exercise

when you exercise, you breathe more rapidly, which produces more CO2 output, decreasing the time of color change

how does the body get rid of potentially dangerous high levels of CO2 that are produced during strenuous physical exercise

anaerobic respiration and lactic acid