pH 14 12 10 8 6 4 2 0 0 10 Acid-Base Titration Curve equivalence point: VNaOHE half-equivalence point: VNaOH= pka= 20 30 ml NaOH pH= 40 pH= 50 Assignment and rubric: Use the proper graphing techniques to find the equivalence and half-equivalence points and determine the pKa and Ka of an unknown acid the exar.. CA 60 -Series1

pH 14 12 10 8 6 4 2 0 0 10 Acid-Base Titration Curve equivalence point: VNaOHE half-equivalence point: VNaOH= pka= 20 30 ml NaOH pH= 40 pH= 50 Assignment and rubric: Use the proper graphing techniques to find the equivalence and half-equivalence points and determine the pKa and Ka of an unknown acid the exar.. CA 60 -Series1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. PREV 1 2 4 NEXT Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. 3.0 x 10-6 %3D 5 RESET [0] [0.200] [0.0200] [0.100] [0.140] [0.175] [x] [2x] [0.200 + x] [0.200 - x] [0.0200 + x] [0.0200 - x] [0.100 + x] [0.100 - x] [0.140 + x] [0.140 - x] [0.175 + x] [0.175 - x] II
5. I found my initial equivalence point for titration. How do I calculate 1/4, 1/2 & 3/4 equivalence points?
Identify which point on the titration curve corresponds to the p.Ka for each of the titratable groups, and which point corresponds to the pl. Drag the appropriate labels to their respective targets. imidazole group pl -СООН group -NH3+ group Hd 14 12 10 8 6- 4H 2 0 2 Moles "OH added per mole histidine 3
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3
A Consider the pH titration curve above (pH vs volume in ml). The pk, of the weak base being titrated and the pH of the equivalence point are, respectively: 12 11 10 8 7 5 4 2 1 10 20 30 40 O 2.5 and 4.0 • 5.4 and 4.5 O 11.2 and 5.4 O 11.2 and 4.5 O 4.5 and 5.4 Based on the indicator information above, which of the following indicators could be used successfuly in the titration in Part A? (Select all correct responses. Indicator Colour (low pH – high pH) pK, methyl yellow red-yellow 3.1 methyl orange red-yellow 3.7 bromophenol blue yellow-blue 4.2 bromocresol green yellow-blue 4.7 methyl red pink-yellow 5.1 bromocresol purple bromothymol blue yellow-purple 6.3 yellow-blue 7.0 phenol red yellow-red 7.9 O phenol red cresol red yellow-red 8.3 O bromocresol purple thymol blue yellow-blue 8.9 O methyl yellow thymolphthalein colourless-blue 9.2 O bromothymol blue O thymol blue O thymolphthalein Part C Baseu on the table above, what colour is methyl orange at pH3? Submit Request Answer Part…
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
culate the pH during the titration gent. The Ka of acetic acid is 1.75x105. 801031 1801031/ A) 10.00 C) 191801031 of 50.00 191801031 191801031 19 E) 8.73 191801031 1 m of 0.100 M acetic acid with 0.1000 M sodium hydroxide at 25°C after the addition of 25.00 mL of 191801031 91801031 191801031 191801031 191801031 191801031 191801031 031 191801001 031 191801031 191801031 101801031 031 191801031 191801031 191801031 191801031 191801031 101801031 (91801031 101801031 191801031 191801031 191801031 191801031 191801031 191801031 191801031 19180103 191801031 101001031 191801031 191801031 181801031 191801031 181801004 391 191301051 19
10:49 1 4 7 +/- Question 6 of 10 In the titration of 69.0 mL of 0.400 M HCOOH with 0.150 M LIOH, how many mL of LiOH are required to reach the equivalence point? 2 5 8 mL 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
Consider how best to prepare one liter of a buffer solution with pH = 3.79 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams sodium salt of weak acid = grams sodium salt of conjugate base =
Which of the following indicators will be the most appropriate to be used for the titration of 15.0 mL 1.0 M H2CO3 with 1.0 M KOH titrant to the second equivalence point ? H2CO3: pKa, 6.35 ; pKaz : 10.33 Select one: O A. Methyl Red, pKa 5.1 O B. Phenol red, pka 7.9 OC. Phenopthalein, pka 9.3 O D. Bromthymol blue, pka 7.0 O E. Methyl Orange, pka 3.7
If the equivalence point of the titration is when the pH is 4, what indicators could you use? Acidic Basic T Indicator pH Range 2 3 4 5 6 7 8 9 10 11 12 13 14 Thymol Blue 1.2-2.8 and 8.0-9.2 Methyl Orange 3.0-4.4 Bromphenol Blue 3.0-46 Congo Red 3.0-5.0 Bromcresol Green 38-5.4 Methyl Red 4.4-6.2 Bromthymol Blue 60-7.6 Phenol Red 6.8-8.4 Which one would you use if the pH is 6?
The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. 14 pH 12 10 8 6 4 2 0 L 05 (1) The pH curve represents the titration of a weak acid with a weak base. (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown list. L J 1 10 15 20 25 30 35 40 45 50 mL of 0.1 M base added Malachite green Thymol blue Methyl orange Bromocresol green Methyl red Bromothymol blue Cresol red Phenolphthalein Thymolphthalein Alizarin yellow 0.2 pH 0 1.2 1 1.8 2 2.8 3.2 4.4 3 3.8 5.4 4 4.8 6.0 5 6.0 6 8.0 7.6 7.0 8.2 8 8.8 9.6 9 10.0 94 10.6 10.1 12.0 10 11 12 13 14