Properties of Acids and Bases Review

Monoprotic acids are

• Antacids

• Conjugate bases

• Acids that are only used once

• Acids that can donate one hydrogen ion per molecule

The conjugate base of HSO4-

• 
• 
• SO4-

• HSO4

pH 6 is less acidic than pH 2 by

• 4 times

• 4000 times

• 1000 times

• 10000 times

Ammonia and amines are considered to be weak bases. This means that they

• have pH values in the range of 6-8

• react very slowly to neutralise acids

• have relatively low solubilities in water

• partially ionise when in aqueous solution

Which of the following is amphiprotic?

• 
• 
• 
• O-

Two aqueous solutions of bases, X and Y, both with concentrations of 0.5M have pH values of 8 and 10, respectively. Which of the following statements is true about the solutions X and Y.

• X is a stronger base than Y

• X contains 100 times more undissociated molecules than Y

• The solution of X will conduct electricity better than the solution of Y

• The solution of Y contains a higher concentration of OH- ions than that of X

If C2H5OH is a very weak Bronsted-Lowry acid, what is true about the ion C2H5O-

• It is a good proton donor

• It is a strong Bronsted-Lowry base

• It is a stronger Bronsted-Lowry acid than C2H5OH

• In an aqueous solution, it will be present in higher concentrations at equilibrium than C2H5OH

A 2.0M solution of an acid has a pH of 3.5. Which of the following statements is true?

• The acid is weak and dilute

• The acid is strong and dilute

• The acid is weak and concentrated

• The acid is strong and concentrated

A solution is made from CH3COOH with a concentration of 0.5M and CH3COONa with a concentration of 0.10M. This solution would

• not be able to function as a buffer solution

• be able to buffer added acid better than added base

• be able to buffer added base better than added acid

• be able to buffer added acid and added base equally well

A solution is equimolar in NaHSO4 and Na2SO4. Addition of strong acid to this solution will result in

• precipitation of Na2SO4

• precipitation of NaHSO4

• reaction of SO4 2- to form HSO4-

• reaction of HSO4- to form SO4 2-