Question 1

What laboratory apparatus is depicted in the first image, and what is its primary use in acid-base titrations?

Accepted Answer

A burette, used to accurately deliver variable volumes of titrant during a titration.

Question 2

In a titration experiment, what is the function of the apparatus shown in the second image?

Accepted Answer

It is an Erlenmeyer flask, used to contain the analyte solution being titrated.

Question 3

Refer to the third image. What does the equivalence point on the titration curve represent?

Accepted Answer

The point at which the amount of acid equals the amount of base, resulting in complete neutralization.

Question 4

In the titration curve shown in the fourth image, what is the approximate pH at the equivalence point for the titration of a strong acid with a strong base?

Accepted Answer

pH = 7

Question 5

In the fifth image, what is the volume of 1.0 M HCl added at the equivalence point during the titration of 50.0 mL of 1.0 M NaOH?

Accepted Answer

$$50.00\ \mathrm{mL}$$

Question 6

A student mixes $$50.0\ \mathrm{mL} of$$ $$0.100\ \mathrm{M}\ \mathrm{HCl}$$ with $$10.0\ \mathrm{mL} of$$ $$0.100\ \mathrm{M}\ \mathrm{NaOH}. $$What is the limiting reactant, and what is the resulting pH?

Accepted Answer

NaOH is the limiting reactant; the solution is acidic with $$\mathrm{pH} \u003c 7.$$

Question 7

Calculate the pH after mixing $$50.0\ \mathrm{mL} of$$ $$0.100\ \mathrm{M}\ \mathrm{HCl}$$ with $$60.0\ \mathrm{mL} of$$ $$0.100\ \mathrm{M}\ \mathrm{NaOH}.$$

Accepted Answer

$$\mathrm{pH} = 12.0$$

Question 8

During a titration, why does the pH change most rapidly near the equivalence point?

Accepted Answer

Because the concentrations of acid and base are nearly equal, causing a sharp change in $$[\mathrm{H}^+] or$$ $$[\mathrm{OH}^-].$$

Question 9

A titration is performed by adding $$0.100\ \mathrm{M}\ \mathrm{NaOH} to$$ $$200.0\ \mathrm{mL} of $$dilute $$\mathrm{HNO}_3. If$$ $$25.0\ \mathrm{mL} of $$NaOH is required to reach the equivalence point, what is the molarity of the $$\mathrm{HNO}_3$$ solution?

Accepted Answer

$$0.0125\ \mathrm{M}$$

Question 10

Which of the following best describes the shape of the pH curve for the titration of a strong acid with a strong base?

Accepted Answer

A gradual increase in pH followed by a sharp rise at the equivalence point, then leveling off at high pH.

Question 11

If $$100.0\ \mathrm{mL} of$$ $$0.500\ \mathrm{M}\ \mathrm{NaOH} is $$titrated with $$1.00\ \mathrm{M}\ \mathrm{HCl}$$, what is the equivalence point volume of HCl added?

Accepted Answer

$$50.0\ \mathrm{mL}$$

Question 12

Which equation correctly relates the moles of acid and base at the equivalence point in a titration of a monoprotic strong acid with a strong base?

Accepted Answer

$$M_1$$ $$V_1$$ = $$M_2$$ $$V_2$$

Question 13

A titration curve for a strong acid-strong base titration is plotted. What does the first derivative of the curve represent?

Accepted Answer

The rate of change of pH with respect to the volume of titrant added.

Question 14

Why is it important to use a burette (as shown in the first image) rather than a beaker to deliver titrant during a titration?

Accepted Answer

A burette allows for precise measurement and controlled addition of titrant.

Question 15

During a titration, a student overshoots the equivalence point by adding too much titrant. How will this affect the calculated concentration of the analyte?

Accepted Answer

The calculated concentration will be too low because excess titrant is counted.

Acid-Base Titration and Limiting Reactant Situations in General Chemistry

스터디 가이드 - 연습 문제

학습 가이드 - 플래시카드