Ch. 15 Section 2 pH and Titrations

An acid-base titration always involves the

• addition of a strong acid

• addition of a strong base

• controlled addition of a standard solution

• addition of metal ions.

An acid-base titration is carried out by monitoring

• temperature

• pH

• density

• pressure

When titrating a strong acid with a strong base, the equivalence point

• will be below a pH of 7.0

• will be at a pH of 7.0

• will be a pH above 7.0

• will be either above or below a pH of 7.0

What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?

• .0.200 M

• 0.320 M

• 0.280 M

• 0.500 M

What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of 0.0904 M HNO3?

• 0.230 M

• 0.460 M

• .0.355 M

• 0.620 M

What is the molarity of an H₂SO₄ solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution whose concentration is 0.333 M?

• .0.116 M

• 0.465 M

• .0.232 M

• 0.880 M

During an acid-base titration, a rapid change in pH

• occurs when the first addition of the standard solution is made

• occurs at several points during the titration

• occurs when the amounts of H₃O⁺ ions and OH^- ions are nearly equal

• should not occur

An indicator, congo red, has a transition range of pH 3.0 –5.0. It would be a good indicator for titrating a

• strong acid and a strong base

• weak acid and a strong base

• strong acid and a weak base

• weak acid and a weak base

When titrating a weak acid with a strong base, the equivalence point

• will be below a pH of 7.0

• will be at a pH of 7.0

• will be above a pH of 7.0

• cannot be determined by pH

What can be used to determine pH solutions due to the color changes?

• -log [H₃O⁺] (calculations with a calculator)

• indicators

• balanced chemical reactions

• pH meters