Using Titration to Determine the Identity of an Unknown Acid 5. An unknown acid is titrated with NaOH to obtain the following titration curve. pH 14 12 10 8 6 4. 2 0 0 25 50 75 Volume of NaOH (mL) 100 a. Label the equivalence point and half-equivalence point on this curve. b. Determine the pK₂ of the unknown acid. Explain how you got your answer.

12.0 10.0 8.0 pH 6.0 4.0 C 2.0 0.0 D 0 5 10 15 20 25 30 mL of 0.1 M NaOH The graph above shows the titration curves of four monoprotic acids of varying strengths. All of the acids start out at 0.1 M concentration and 25.0 mL volume. Choose all of the correct statements about these titration curves from the cholces below. The titration curve labelled "D" is generated by the strongest acid in the series. In the curves shown above the stronger the acid the less NaOH required for neutralization. The stronger the acid the more important is the pKa of the Indicator used for titration. The Ka of the acid which generates curve "C" is about 103 The weaker the acid the lower the pH of the neutralization point. The acid which generates curve "D" has the highest neutralization-point pH in the series.

A solution of 25.0 mL 0.200 M CH3COOH solution is titrated with 0.200 M KOHsolution.a. Calculate the pH when 10.0 mL of KOH is added.b. Calculate the pH of the solution at the equivalence point.Ka for CH3COOH = 1.8x10-5; Kb for CH3COO- = 5.6x10-10.

A The graph shows the titration curves of a strong acid and a weak acid. Estimate the pk, of the weak acid from its titration curve V 14 12 10 pH 12086420 Volume of strong base (ml) 1st attempt Write the estimated pK, to one decimal place 1 OF 8 QUESTIONS COMPLETED 82 W S # 3 Z X E 80 FI D $ 4 C R F K5 V 4 FS T G A 6 B S Y 27 & H 8 U N 8 00 DHI 14 M 9 K TV O hi See Periodic Table O L SUBMIT ANSWER P ** FIL

In this experiment, the color change from pink/violet to colorless during the titration is caused by: Group of answer choices a.change from MnO4– to Mn2+ b.change from Fe2+ to Fe3+ c.change from H+ to H2O d.the addition of an indicator.

Acetic acid has a Ka of 1.8 x 10-5. Three acetifc acid/acetate buffer solutions, A, B, and C, were made using varying concentrations:   A. [acetic acid] ten times greater than [acetate] B. [acetate] ten times greater than [acetic acid], and C. [acetate] = [acetic acid].   Match each buffer solution to the expected pH:   a) pH = 3.74 b) pH = 4.74 c) pH = 5.74

The following titration curve depicts the titration of a weak base with a strong acid. 10 PH 2987654321 ++ Which of the following values best approximates the pKb value of the weak base? a. 9.8 b. 8.4 c. 7 d. 4.2