Recent content by jetsetter

Carbonic Acid (H2CO3) I believe.

We have to neutralize an H+ donating acid.

I also know that ultimately we will get something like this: Alkalinity = f1Ct + f2Ct + [OH-] - [H+] f1 and f2 need to be calculated in order to ascertain Ct.

I realize it is going to be something like this: Alkalinity = (1 eq/mol)([HCO3]) + (2 eq/mol)([CO3]) + (1 eq/mol)([OH]) - (1 eq/mol)([H]) The influence of the OH and H are minimal and easy to calculate. [H+] = 10^(-7.8), [OH-] = (10^(-7.8))/(1 x 10^(-14))

Well, alkalinity is the buffering capacity of the liquid. The resistance of the liquid to pH change. The greater the carbonate concentration the greater the buffering capacity.

Homework Statement If the pH of a natural water is 7.8 and the alkalinity was measured to be 125 meq/L, determine the following: -Alkalinity as mg/L CaCO3: Answer = 6250 mg/l CaCO3 -Approximate the total carbonate concentration CT, in moles per liter: Answer = 0.125 moles per liter...