pH and Buffers

What is normal ratio of bicarbonate buffer in blood?

• 10:1

• 20:2

• 20:1

• 1:20

————- is known as the alkali reserve of blood.

At ————— pH amino acid exist as zwitter ion.

What is a buffer solution?

• A mixture of a weak acid and a strong base

• A mixture of a strong acid and a weak base

• A mixture of a weak acid and its conjugate base

• A mixture of a strong acid and its conjugate base

What is the buffering capacity of a solution?

• Its ability to resist changes in pH

• Its ability to neutralize strong acids

• Its ability to dissolve limestone

• Its ability to form carbonic acid

A buffer is defined as a combination of chemicals that

• ability to change a pH

• ability to prevent pH from decreasing

• ability to resist a pH increase

• minimizes the changes in the concentrations of H⁺ and OH^-

If some process releases acid [H⁺] into the blood, this equilibrium responds by shifting to the left as long as there is HCO₃^-present for the H⁺ to react with, thus removing the excess H⁺ions. What happens after the release of H⁺?

• pH never lowers

• pH is lowered and then immediately restored

• pH raises and then is restored

• ph lowers and remains low

If a process releases base into the blood, which would react with and lower the concentration of the H⁺, the equilibrium shifts to the right as long as there is H₂CO₃, thus replacing the lost H⁺ions. To protect against added base, what needs to be in relatively high amounts?

• HCO₃^-

• OH^-

• H⁺

• H₂CO₃

Which solution A and B of equal volume and concentration mixed together to form a buffer?

• Nitric acid and potassium hydroxide

• Nitric acid and potassium nitrate

• Propanoic acid and potassium hydroxide

• Propanoic acid and potassium propanoate

What is the pH of a neutral solution at 25°C?

• A) 0

• B) 7

• C) 14

• D) 1