WorksheetsCh. 15 Section 2 pH and Titrations
Total questions: 15
Worksheet time: 21mins
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
Check all the boxes that include equipment or materials that you would use during an acid-base titration.
gloves and safety glasses
evaporating dish and watch glass
buret and ring stand
unknown and known acid and base solutions
salt solution
If you are titrating with 1.0 M NaOH and the unknown solution is 1.0 M HCl, which would be true?
it is impossible to tell the volumes from this information
the volume of unknown HCl would be more than the volume of the NaOH
the volume of the NaOH used would be more than the volume of the unknown HCl
the volume of the unknown HCl would be equal to the volume of NaOH used
Which best explains an endpoint versus an equivalence point of a titration?
the end point of a titration is where the two solutions are present in chemically equal amounts; the equivalence point is the point where the indicator changes color
the equivalence point of a titration is the point where equal volumes of acid and bases have been added; the end point is when the indicator has been added
the equivalence point of a titration is where the two solutions are present in chemically equal amounts; the end point is the point where the indicator changes color
None of these are correct
An unknown solutions turns clear when tested with phenolphthalein. What is known from this information?
the solution is a base
the solution is an acid
the solution is neutral
the solution contains a salt and water
An unknown solution turns clear when tested with phenolphthalein. The solution turns orange when tested with methyl orange. What is most likely true?
the pH of the solution is 8.2
the pH of the solution is 2.0
the pH of the solution is 11
the pH of the solution is 4.0
