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# College Acids and Bases Questions

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College Acids and Bases
College Acids and Bases
A solution with a pH value of 7 indicates a(n):
1. volatile solution
2. alkaline solution
3. neutral solution
4. acidic solution
College Acids and Bases
A substance that has a pH above 7.0 is considered to be a(n):
1. neutral solution
2. acid solution
3. alkali solution
4. reducing solution
College Acids and Bases
If the pH of a solution is decreased from 9 to 8, it means that the
1. concentration of H+ has decreased by a factor of 10
2. concentration of H+ has increased tenfold
3. concentration of OH- has increased tenfold
4. concentration of OH- has decreased by a factor of 10
5. concentration of H+ has increased by a factor of 100
College Acids and Bases
Which of the following describes a base, according to the Brønsted-Lowry theory?
1. resists changes in pH
2. releases hydrogen ions in a solution
3. accepts hydrogen ions in a solution
4. a single subunit that is repeated in a much larger molecule
5. a large molecule with many repeating subunits
College Acids and Bases
Which of the following describes a buffer?
1. resists changes in pH
2. releases hydrogen ions in a solution
3. accepts hydrogen ions in a solution
4. a single subunit that is repeated in a much larger molecule
5. a large molecule with many repeating subunits
College Acids and Bases
Which of the following are examples of electrolytes?
1. Sugars, Salts, and Starches
2. Sugars, Starches, and Fats
3. Acids, Bases, and Sugars
4. Acids, Bases, and Salts
College Acids and Bases
Which of the following titrations demonstrates the reaction of a strong acid with a strong base?
1. $CH_3COOH + LiOH$
2. $H_2SO_4 + KOH$
3. $CH_3OH + Ca(OH)_2$
4. $NH_3 + Al(OH)_3$
College Acids and Bases
How does the titration curve of a weak acid and a strong base differ from the titration curve of a strong acid and a strong base?
1. The pH value changes more readily in the titration curve of the strong acid and the strong base
2. The pH value changes equally for each of the titration curves
3. The pH value changes more readily in the titration curve of a weak acid and a strong base
4. The pH value changes only in the presence of a buffer
College Acids and Bases
Which of the following describes an acid, according to the Brønsted-Lowry Theory?
1. resists changes in pH
2. releases hydrogen ions in a solution
3. accepts hydrogen ions in a solution
4. a single subunit that is repeated in a much larger molecule
5. a large molecule with many repeating subunits
College Acids and Bases
Which of the following correctly defines a buffer?
1. A solution that resists changes in pH when an acid is added
2. A solution that resists changes in pH when a base is added
3. A solution that allows changes in pH when an acid or a base is added
4. A solution that resists changes in pH when an acid or a base is added
College Acids and Bases
Which of the following represents a viable buffer?
1. HCl and its salt
2. NaOH and its salt
3. Ammonia and its salt
4. None of the above
College Acids and Bases
Which of the following is an appropriate description of a back titration?
1. A base is titrated with an acid
2. A known excess of standard reagent is added to the solution and titrated
3. A weak base is titrated with an acid, and the solution is titrated with a strong base
4. None of the above
College Acids and Bases
Which of the following correctly represents the equation used to calculate the pH value of the buffer, based on the $K_a value$?
1. $pH=pK_a+{log} [[A^-]]/[[HA]]$
2. $pH=pK_a-{log} [[A^-]]/[[HA]]$
3. $pH=pK_a+{log} [[HA]]/[[A^-]]$
4. $pH=pK_a-{log} [[HA]]/[[A^-]]$
College Acids and Bases
Which acid-base pair from the following would most readily result in an equivalence point that occurs most closely at a pH value of 7?
1. $HCl"/"Ca(OH)_2$
2. $NaOH"/"CH_3COOH$
3. $NH_3"/"CH_3COOH$
4. Either (b) or (c)
College Acids and Bases
Which of the following equations represents the pH of the buffer?
1. $[HA]/[A^-]$
2. 1
3. $[HA], only$
4. $[A^-]/[HA]$
College Acids and Bases
College Acids and Bases
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