14. Basic Chemistry: Acids and Bases

Consider separate aqueous solutions of HCl and H₂SO₄ with the same concentrations in terms of molarity. You wish to neutralize an aqueous solution of NaOH. For which acid solution would you need to add more volume (in mL) to neutralize the base?

• The HCl solution.

• The H₂SO₄ solution.

• You need to know the acid concentrations to answer this question.

• You need to know the volume and concentration of the NaOH solution to answer this question.

• c and d

Choose the answer that best completes the following statement. When 100.0 mL of water is added to 100.0 mL of 1.00 M HCl, ....

• the pH decreases because the solution is diluted.

• the pH does not change because water is neutral.

• the pH is doubled because the volume is now doubled.

• the pH increases because the concentration of H decreases.

• the solution is completely neutralized.

Which of the following/s do not represent a conjugate acid–base pair?

• HClO₄, ClO₄^-

• NH₄⁺, NH₃

• NH₃, NH₂^-

• H₂O, O^2-

• HClO, HClO₂

According to Bronsted-Lowry, what is the definition of an base?

• A substance that donates a hydrogen (H⁺) ion.

• A substance that donates a hydroxide (OH^-) ion.

• A substance that accepts a hydrogen (H⁺) ion.

• A substance that accepts a hydroxide (OH^-) ion.

• None of correct definition.

What is being donated/accepted between conjugate acid-base pairs?

• A hydrogen (H⁺) ion.

• A hydroxide (OH^-) ion.

• Water.

• An electron.

• A proton.

Cabbage juice changes color in the presence of other chemicals, and the color it changes depends on the other chemical's pH. We can classify cabbage juice as ....

• Reactant.

• Acid.

• Base.

• Indicator.

• Product.

The difference between a strong acid and a weak acid is that a strong acid ......

• has a lower pH.

• dissociates completely.

• has a higher pH.

• donates H⁺ ion.

• has a higher concentration.

Which of these statements is/are true regarding a 1.0 M solution of a strong acid HA?

• [A^-] > [H⁺].

• The pH is 0.00.

• [H⁺] = 1.0 M.

• [HA] = 1.0 M.

• There is no correct answer.

Which of these statements is/are true regarding a 0.10 M solution of a weak acid HA?

• The pH is more than 1.00.

• [H+] >> [A-]

• [H+] = [A-]

• The pH is less than one

• None of the above.

A buffer solutions consist of a weak acid and a salt of its ........