2- Ahmed has done four types of titrations of 1M and 50 ml forboth acid and base (Conductometric Titration of Strong Acidwith Strong Base , Potentiometric Titration of Weak Acidwith Strong Base , Potentiometric Titration of Strong Acidwith Strong Base and Conductometric Titration of WeakAcid with Strong Base ). He plotted the results in curves asshown below. Match between the type of titration and his results3- Ahmed standardized NaOH (10 ml) with KHP( mass=1 g ,MW= 204 g/mol ). Calculate the concentration ofstandardized NaOH?4- Calculate pka for a weak acid titrated with strong baseusing the curve shown below?1412-10-86-4-2-0-10203040505- If the solute moved 3 cm in paper chromatography and R,was 0.5. How long in cm the solvent has moved? O 4G ll.Done Final exam_dde3a4008bef6ffbf3...sity2IDAcademic Year:me311Lion:10'of Na1- Name the glassware and the apparatuses that showing byyour instructor.A.В.С.D.2- Ahmed has done four types of titrations of 1M and 50 ml forboth acid and base (Conductometric Titration of Strong Acidwith Strong Base , Potentiometric Titration of Weak Acidwith Strong Base , Potentiometric Titration of Strong Acidwith Strong Base and Conductometric Titration of WeakAcid with Strong Base ). He plotted the results in curves asshown below. Match between the type of titration and his results3-stanJaOH (10 ml)KHP( mass= 1 g,MW= 204 g/mol ). Calculate the concentration ofstandardized NaOH?4- Calculate pka for a weak acid titrated with strong baseusing the curve shown below?125- If the solute moved 3 cm in naner chromatography and R,

1. Curve for Conductometric titration of strong acid Vs strong base : 2. Curve for Potentiometric…

2- Ahmed has done four types of titrations of 1M and 50 ml for both acid and base (Conductometric Titration of Strong Acid with Strong Base , Potentiometric Titration of Weak Acid with Strong Base , Potentiometric Titration of Strong Acid with Strong Base and Conductometric Titration of Weak Acid with Strong Base ). He plotted the results in curves as shown below. Match between the type of titration and his results

2- Ahmed has done four types of titrations of 1M and 50 ml for both acid and base (Conductometric Titration of Strong Acid with Strong Base , Potentiometric Titration of Weak Acid with Strong Base , Potentiometric Titration of Strong Acid with Strong Base and Conductometric Titration of Weak Acid with Strong Base ). He plotted the results in curves as shown below. Match between the type of titration and his results

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Lactic acid is a common by-product of cellular respiration and is often said to cause the burn associated with strenuous activity. A 25.0-mL sample of 0.100 M lactic acid (HC3H5O3, pKa = 3.86) is titrated with 0.100 M NaOH solution. Calculate the pH after the addition of 0.0 mL, 4.0 mL, 8.0 mL, 12.5 mL, 20.0 mL, 24.0 mL, 24.5 mL, 24.9 mL, 25.0 mL, 25.1 mL, 26.0 mL, 28.0 mL, and 30.0 mL of the NaOH. Plot the results of your calculations as pH versus milliliters of NaOH added.
A student is preparing to titrate 25.00 mL of 0.2 M NaOH. He has options to use among 3 weak monoprotic acid at same concentration, with different acid dissociation constants, WA1= 1 X 10-4, WA2= 1 X 10-5 , WA3= 1 X 10-8. Which is the best acid titrant you would recommend ?
1 Calculate the pH at the equivalence point in titrating 0.069 M solutions of each of the following with 0.056 M NaOH. (a) periodic acid (HIO4) pH = (b) ascorbic acid (HC6H7O6), Ka = 8e-05 pH = (c) hydrocyanic acid (HCN), Ka = 4.9e-10 pH
explain each of the following cases. a) when we treat 1 mol / liter of hydrochloric acid, the pH increases. There comes a cast that the pH reaches a certain value and does not change anymore. Why does this happen? b) Methyl orange can be used to determine the final titration point of nitric acid with ammonia solution, while phenophthalein is not used in this case. Why? c) pH of 10-8 mol / l HCl is not 8. Why?
A sample of 50.00 mL of 0.1000 M aqueous solution of chloroacetic acid, CH2ClCOOH (K1= 1.4 × 10-3), is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following stages in the titration, and plot thetitration curve: 0, 5.00, 25.00, 49.00, 49.90, 50.00, 50.10, and 55.00 mL NaOH.
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
Calculate the titration of 0.1 M 50 mL H3PO4 with 0.1 M NaOH as baseline, pre-end, endpoint, post-endpoint and plot the titration curve. (Ka1= 7x10-3, Ka2= 2.2x10-7 , Ka3= 4.5x10-13)
Calculate the pH at the equivalence point of 65 ml solution containing a weak acid, AH, for instance CH3COOH, titrated with 30 ml of a strong base, B OH, like KOH, with a concetration of 0.91 M. The acid dissociation constant, Ka , is 2.15e-7. pH ← please insert your value