Application of ph in daily life?

Answer 1

in our blood we have a buffer system

H2O(l) + CO2(g) <-----> H2CO3(aq)

H2CO3(aq) <---> HCO3-(aq) + H+(aq)

when a child playing is out in the field and suddenly hyperventilates, he/she is expelling more CO2(g) than he/she normally would. This would then decrease normal CO2(g) levels in the blood. Following Le Chatelier's principle the above reaction (2nd one) would then tend to shift to the left due to decrease in CO2(g) ==> which means the body would have to compensate by producing more H+(aq) ions. This then affects our body's pH...... our pH is becoming acidic and when not corrected.... would lead to acidosis.... which is fatal

remedy: to replenish CO2(g) one has to encourage the child to inhale and exhale in a paper bag covering his/her nose and mouth. What you are actually doing is increasing the CO2(g) intake so that the equilibrium now would balance out by shifting the system to its normal forward reaction.

Life and Death situation of pH in daily life (",)