A buffered solution containing dissolved aniline, C, H, NH₂, and aniline hydrochloride, C,H, NH, Cl, has a pH of 5.60. A. Determine the concentration of C, H, NH; in the solution if the concentration of C, H, NH, is 0.275 M. The pK, of aniline is 9.13. [C HẠNH;] = B. Calculate the change in pH of the solution, ApH, if 0.363 g NaOH is added to the buffer for a final volume of 1.95 L. Assume that any contribution of NaOH to the volume is negligible. ApH = M

A buffered solution containing dissolved aniline, C, H, NH₂, and aniline hydrochloride, C,H, NH, Cl, has a pH of 5.60. A. Determine the concentration of C, H, NH; in the solution if the concentration of C, H, NH, is 0.275 M. The pK, of aniline is 9.13. [C HẠNH;] = B. Calculate the change in pH of the solution, ApH, if 0.363 g NaOH is added to the buffer for a final volume of 1.95 L. Assume that any contribution of NaOH to the volume is negligible. ApH = M

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...

See similar textbooks

Similar questions

Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7
Calculate the pH of each of the following solutions a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5 b. 0.10 M sodium propanoate, NaCH3CH2COO. c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate
2. Which one of the following is a buffer solution? a. 0.40 M HCN and 0.10 KCN b. 0.20 M СH;COОН c. 1.0 M HNO3 and 1.0 M NANO3 d. 0.10 M KCN с. e. 0.50 M HCl and 0.10 NaCl Why? (Be specific! Also explain why the other 4 choices are NOT buffer solutions.)
10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40. Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid. A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.
A n analytical chemist is titrating 198.9 mL of a 0.2300 M solution of diethylamine ((C,H,) NH) with a 0.1500 M solution of HNO3. The p K, of diethylamine b. is 2.89. Calculate the pH of the base solution after the chemist has added 357.1 mL of the HNO, solution to it. 3 Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.
se or conjugate base. 12 2. A 50.0mL sample of an acid HA, of unknown molarity is titrated with 0.1000 M KOH. The pH of the resulting solution is measure with a pH meter and graphed below. Select the letter that corresponds to the following. Some letters may be used more than once. Some may not be used at all. 10+ a. the equivalence point: R 9 b. the half equivalence point: Q 8+ c. where [KOH] is greatest: 7+ P I of d. where [H+] is greatest: T e. where [HA]=[A-]: 5+ 4 f. where [A-] is the predominate species: 3+ 2 SO a. What is pH after 10.0mL of 0.15M NaOH solution has been added to 25.0 mL of 0.12M HF solution? Ka = 6.8 x 10-4. b. After adding NaOH, is the resulting solution a buffer solution? Explain. 3. Complete the following calculations. (P) (Q) 84 3 ST PR
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. 1 2 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH2(aq) H*(aq) H2NNH;*(aq) + Before (mol) Change (mol) After (mol) 5 RESET 0.200 0.100 +x 0.200 + x 0.200 - x -x 0.100 + x 0.100 - x 1.00 x 103 -1.00 x 10-3 2.00 x 10-3 -2.00 x 10-3 6.00 x 103 -6.00 x 10-3 7.00 x 10-3 -7.00 x 103 8.00 x 103 -8.00 x 103
6. Consider a solution that has 0.00500 M HCl and 0.100 M HF. Ka of HF = 7.2x10-4. a. What is the pH of this solution? b. Suppose the solution was like that in A but also had 0.1 M HOI. (i.e. total solution was a mix of 0.00500 M HCl, 0.100 M HF, and 0.1 M HOI). Ka of HOI = 2.0x10-¹¹. Does this solution have an appreciably different pH than the solution in part a? Support your answer with relevant calculations. HINT: Work from strongest acid to the weakest acid.
A chemist titrates 110.0 mL of a 0.7452M aniline (C,H,NH,) solution with 0.5088M HCl solution at 25 °C. Calculate the pH at equivalence. The p K, of aniline is 4.87. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = ||
A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)
The pK, values for the dibasic base B are pKi = 2.10 and pk2 = 7.49. %3! Calculate the pH at each of the points in the titration of 50.0 ml. of a 0.55 M B(aq) solution with 0.55 M HCI(aq). What is the pH before addition of any HCI? pH What is the pH after addition of 25.0 ml. HCI? pH = What is the pH after addition of 50.0 mL HC? pH What is the pH after addition of 75.0 mlL HCI? pH = What is the pH after addition of 100.0 ml. HCI? pH =
Benzoic acid, HC7H5O2, has a Ka value of 6.4 x 10-5. B. Find the pH of a solution made by mixing 600. mL of the benzoic acid solution from part A with 450. mL of a 2.00 M solution of lithium benzoate, LiC7H5O2. C. Find the pH of a solution made by adding 36.0 grams of sodium hydroxide, NaOH, to the solution created in part B. Molarity of benzoic acid is 4.