A buffer solution is prepared in which the concentration of NH3 is 0.20 M and the concentration of NH4* is 0.30 M. What is the pH of this solution? The equilibrium constant, Ka for NH,1+ equals 5.56 x 10-10. А. 8.73 В. 9.08 С. 9.43 D. 11.72

A buffer solution is prepared in which the concentration of NH3 is 0.20 M and the concentration of NH4* is 0.30 M. What is the pH of this solution? The equilibrium constant, Ka for NH,1+ equals 5.56 x 10-10. А. 8.73 В. 9.08 С. 9.43 D. 11.72

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

5. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC₂H3O2 mixed with 15.00mL of 0.3000M NaOH c. 22.50mL of 0.2000M NH3 mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HClO₂ mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH₂ mixed with 25.00mL of 0.1500M HCI
What combination of substances will give a buffered solution that has a pH of 5.05? (Assume each pair of substances is dissolved in 5.0 L of water.) (Kb for NH3 = 1.8 ´ 10–5; Kb for C5H5N = 1.7 ´ 10–9) a. 1.0 mole NH3 and 1.5 mole NH4Cl b. 1.5 mole NH3 and 1.0 mole NH4Cl c. 1.0 mole C5H5N and 1.5 mole C5H5NHCl d. 1.5 mole C5H5N and 1.0 mole C5H5NHCl e.none of these
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
Answer the following questions by circling the correct response. a. A0.100 M solution of NaOH has a higher pH than a 0.100 M solution of Ba(OH)2. TRUE / FALSE b. What is the pH of a solution made by dissolving Fe(NO:)2 in water? ACIDIC / NEUTRAL / BASIC c. If you have a buffer solution made from 1 parts ammonia and 2 parts ammonium ions, what is the pH of that solution? 8.95 / 9.55 d. You have a saturated solution of NH,CI with a small amount of undissolved NH,CI sitting at the bottom of the container. Adding which of the following would cause the solid NHẠCI to dissolve? Naci / HCI / NaOH e. The entropy of the universe increases when NaOH is dissolved into water. TRUE / FALSE
A 25.0 ml sample of 1.00 M HCl is titrated with 50.0 ml of 1.00 M NaOH solution. What is the pH of this solution ? 13.5 10.5 5.52 3.06
I. Consider a 1.00 L of 1.50x10 -3 M hydrocyanic acid (HCN,K=4.9×1019) 1. Write the equilibrium expression. 2. Calculate the pH of the solution. 3. If a 9.00x10 mol sodium cyanide, NaCN, is added, what is the pH of the resulting solution? Assume negligible volume change.
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.
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
1. Create a set of rules for determining which anions and cations will react with water (Hydrolyze) and which won't. Then write another set of rules to describe what happens when a cation reacts with water, and what happens when an anion reacts with water. 2. What is the pH of a solution made by dissolving 8.50 g of potassium formate, KCHO2, in 500.0 mž of 0.100M formic acid, HCHO2. State any assumptions you need to make to answer this question.
1. all the aqueous solutions that are good buffer systems 2. a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is the PH of this buffer solution. b. a buffer solution is 0.495 m in h2s and 0.354 m in khs, if Ka1 for H2s is 1.0 * 10^-7. what is the PH of this buffer solution. c. a buffer solution is 0.455 m in NaHSO and 0.299 m in Na2SO3, if Ka for HSO3 is 6.4 * 10^-8. what is the PH of this buffer solution. 3. A 28.9 ml sample of a 0.385 m aqueous hydrocyanic acid solution is titrated with a 0.372 m aqueous sodium hydroxide solution. what is the ph at the start of the titration, before any sodium hydroxide has been added. b. A 31.9 ml sample of a 0.599 m aqueous hydrofluoric acid solution is titrated with a 0.242 m aqueous barium hydroxide solution. what is the ph after 15.8ml of base has been added. c. when a 23.8 ml sample of a 0.357 m aqueous acetic acid solution is titrated with a 0.459 m aqueous barium hydroxide solution. what is the ph…
8. A 0.0320M solution of a weak base has a pH of 9.45. Determine the Kp of this weak base.
Please don't provide hand written solution....