8. Ka of the acid equalsa)10-pKab)-log (pKa)c)-pKad)pKa 8a. pH at the half equivalence point of an acid-base titration equalsa)Ka of the acidb)pKa of the acidc)Kb of the based)pKb of the base ### Titration Curve ExplanationThis graph represents a titration curve, depicting the change in pH as a base is added to an acidic solution. The x-axis denotes the volume of base added, measured in milliliters (mL), ranging from 0 to 50 mL. The y-axis represents the pH level, ranging from 0 to 12.#### Key Features of the Graph:1. **Initial pH Level:** - At the beginning of the titration (0 mL), the pH is approximately 2, indicating a strongly acidic solution.2. **Buffering Region:** - As the base is incrementally added, the pH gradually increases. There is a relatively flat region between approximately 0 and 20 mL of base, illustrating the buffering capacity of the solution.3. **Equivalence Point:** - The drastic inflection point occurs between 20 and 30 mL. This steep portion of the graph signifies the equivalence point, where the amount of acid equals the amount of base, rapidly shifting from pH 4 to around pH 10.4. **Post-equivalence Region:** - Beyond the equivalence point, the addition of more base results in a gentler increase in pH, leveling off around pH 12 after approximately 40 mL of base has been added.This titration curve is typical for a strong acid-strong base titration, providing insight into the acid-base neutralization process and the solution's buffering capacity.

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Answered: Ka of the acid equals

Science

Chemistry

Ka of the acid equals

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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in the titration of 50.0 mL 0.0200 M weak acid HA using 0.0150 M NaOH, what is the solution pH at the equivalence point? (pKa of the weak acid HA is 5.50)
6
What is the pKa of the weak acid from the titration in the titration curve below?
TUAL Chemistry 20 Che pH Titration Curve for titrating 62.0 mL of Nitric Acid with 0.763 mol/L Aqueous Potassium Hydroxide A PH 15 SHR2109 14 13 11 176O 8 5 3 2 1 5 10 15 20 25 30 35 Volume of titrant added (mL) a. The volume of titrant used to reach the equivalence point for the titration is b. The pH at the equivalence point for the tittation is c. An appropriate indicator to use is ISTON ID the endpoint of the reaction the indicator colour would be d. The concentration of the nitric acid solution analyzed in this titration is calculated to be the correct number of significant digits) mL. (Record your 3-digit answer) (Record your 1-digit answer) At the start of the titration, the indicator colour would be and at mol/L. (Record your answer with
Kk.94.
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Based on the figure, which indicator would be appropriate to indicate the equivalence point of the titration of 0.15M HBr with 0.15M NaOH? (Select one.) Crystal violet Cresol red Thymol blue Erythrosin B 2,4-Dinitrophenol Bromphenol blue Methyl orange Bromcresol green Methyl red Eriochrome* Black T Bromcresol purple Alizarin Bromthymol blue Phenol red m-Nitrophenol o-Cresolphthalein Phenolphthalein Thymolphthalein Alizarin yellow R *Trademark Ciba-Geigy 0 1 2 3 4 -5 6 pH HH 7 8 9 10 10 11 12 13
You carry out the titration of a week diprotic solid with .25 M NaOH until surpassing the second equivalence point. The equivalence points are easy to see at 12 mL and 24 mL. You realize you forgot to write down the mass of your unknown and you do not want to start over. Using the pKa values, you decide the identity of your unknown is Ascorbic acid(molar mass: 176.12 g/mol; pKa1: 4.1; pKa2: 11.79). How many grams of Ascorbic acid did you start with?
Dilute solutions of the same weak acid (pKą = 4.5) ranging in concentration from 2 × 10-6 M to 2 × 10-2 M (0.002 to 20 mM) are titrated with a strong base that is five times more concentrated than the acid. At low concentrations of a weak acid, how does the concentration of the acid affect the shape of the titration curve? The higher the concentration of the acid, the sharper the inflection at the equivalence point. The lower the concentration of the acid, the sharper the inflection at the equivalence point. The shape of the titration curve is the same, regardless of the acid's concentration. The shape of the titration curve depends only on the pKa of the acid, not its concentration.
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
2.5 20.00 mL of 0.0750 M benzoic acid ( C6H5COOH) is titrated with 0.0250 M NaOH. Ka benzoic acid = 6.5 x 10-5 A.What is the pH of the solution after the addition of 10.00 mL NaOH? B.What is the concentration of benzoic acid after the addition of 40.00 mL NaOH?
16. Calculate the pH at the equivalence point in the titration of 25 mL of 0.10 M formic acid with a 0.1 M NaOH solution (given that pka of formic acid = 3.74). A. 4.74 B. 8.74 C. 8.37 D. 6.06 17. When a 0.20 M solution of acetic acid is neutralized with 0.20 M NaOH in 0.50 L of water, the pH of the. resulting solution will be (given that pKa for CH3COOH = 4.74) A. 12.67 B. 7.87 C. 8.87 D. 7.00 18. Calculate the equivalent weight of Na2CO3 when it is titrated against HCI in the presence of phenolphthalein. A. 106 B. 53 C. 26.5 D. 212