In the blood buffer system, CO2 reacts with water: CO2(g) + H2O(l) H+(aq) + HCO3-(aq). During intense exercise, the concentration of dissolved CO2 increases. What is the immediate effect on this equilibrium and on blood pH?
More CO2 pushes the equilibrium towards the products.
Which mixture does NOT produce a buffer solution?
Check whether the acid and base are present in equal moles.
The pH of a solution remains almost unaffected on the addition of a few drops of an acid, alkali, or water; such a solution is known as:
This is the defining property of one particular solution type.
A buffer solution is made by mixing CH3COOH with CH3COONa. Which equation correctly shows how this buffer removes added OH-?
The weak acid component neutralises added OH-.
What is the pH of a buffer solution containing 0.20 mol dm-3 CH3COOH and 0.40 mol dm-3 CH3COONa? (Ka for CH3COOH = 1.8 x 10^-5 mol dm-3)
Use pH = pKa + log10([salt]/[acid]).
Which of the following would form a buffer solution?
A buffer needs a weak acid (or base) with its conjugate.
The buffer system in blood involves:
Think about dissolved carbon dioxide in blood.
A buffer solution contains H2PO4- and HPO4(2-). What happens when a small amount of acid (H+) is added?
The more basic component of the pair absorbs the added H+.
A buffer solution is prepared from a weak acid HA and its sodium salt NaA. When a small amount of potassium hydroxide (KOH) is added to this buffer, which equation correctly represents the reaction that removes the added OH-?
The weak acid reacts with the added hydroxide.
