Part AA buffer is prepared by adding 12.0 g of ammoniumchloride (NH,CI) to 240 mL of 1.00M NH3solution. You will need to look up the Kb fromAppendix D.What is the pH of this buffer?pH =SubmitRequest AnswerPart BWrite the net ionic equation for the reaction that occurs when a few drops of nitric acid are addedto the buffer.Express your answer as a chemical equation. Identify all of the phases in your answer.U ΑΣΦOA chemical reaction does not occur for this question.SubmitRequest AnswerPart CWrite the net ionic equation for the reaction that occurs when a few drops of potassium hydroxidesolution are added to the buffer.Express your answer as a chemical equation. Identify all of the phases in your answer." ΑΣφ?DA chemical reaction does not occur for this question.SubmitRequest Answer

Answer : part a) mole = mass/ molecular weight molecular weight of NH4Cl = 53.491 g/mole mole of…

Part A A buffer is prepared by adding 12.0 g of ammonium chloride (NH,CI) to 240 mL of 1.00M NH3 solution. You will need to look up the Kb from Appendix D. What is the pH of this buffer? να ΑΣΦ ? pH = Submit Request Answer • Part B Write the net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ DA chemical reaction does not occur for this question. Submit Request Answer • Part C Write the net ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer. DA chemical reaction does not occur for this question. Submit Request Answer

Part A A buffer is prepared by adding 12.0 g of ammonium chloride (NH,CI) to 240 mL of 1.00M NH3 solution. You will need to look up the Kb from Appendix D. What is the pH of this buffer? να ΑΣΦ ? pH = Submit Request Answer • Part B Write the net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ DA chemical reaction does not occur for this question. Submit Request Answer • Part C Write the net ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer. DA chemical reaction does not occur for this question. Submit Request Answer

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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A 0.1724-g sample of an unknown monoprotic acid was dissolved in 26.9 mL of water and titrated with 0.0623 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 19.8 mL. (a) Calculate the molar mass of the acid. (b) After 11.5 mL of base had been added during the titration, the pH was determined to be 5.66. What is the Ka of the unknown acid?
Consider the following information to answer the questions below. A volume of 10.00 mL of 0.100 M acetic acid (HC2H3O2) is titrated with 0.148 M sodium hydroxide solution. Given the chemical equation below. Calculate the volume (in milliliters) of NaOH needed to reach the equivalence point of the titration. HC2H3O2(aq) + NaOH(aq) -> H2O (l) + NaC2H3O2(aq)
You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?
We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.44. We titrate this solution with a 0.250 M NaOH solution and we need 33.3 mL of this 0.250 M NaOH solution to reach the equivalence point. The temperature is 25.0 ◦C throughout. (a) What is the molar mass of HA? (b) What is the dissociation constant, Kb, of A−(aq)? (c) What would be the pH of a 2.222 M solution of A−(aq)?
Buffer Preparation: Acid-Base Reactions An aqueous solution contains 0.496 M hydrocyanic acid. Calculate the pH of the solution after the addition of 2.18x10 2 moles of sodium hydroxide to 125 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide) pH = Submit Answer Retry Entire Group 8 more group attempts remaining An aqueous solution contains 0.498 M ammonia. Calculate the pH of the solution after the addition of 3.30x102 moles of hydrobromic acid to 155 mL of this solution. (Assume that the volume does not change upon adding hydrobromic acid.) pH = Submit Answer Retry Entire Group 8 more group attempts remaining Use the References to a An aqueous solution contains 0.336 M ammonia. Calculate the pH of the solution after the addition of 2.95x102 moles of hydrochloric acid to 155 ml of this solution. (Assume that the volume does not change upon adding hydrochloric acid.) pH = Submit Answer Retry Entire Group 8 more group attempts remaining
Consider the “window cleaner” problem, question 2 on page 12 of your lecture notes. Suppose that prior to the titration, the 10 mL sample of window cleaner was diluted by adding about 10 mL of DI water so that the solution could have better contact with the pH meter. What effect would this dilution have on the volume of titrant needed? (a) The amount of titrant would be the same because the moles of analyte was not changed.(b) The amount of titrant would be doubled because the analyte solution volume was doubled.(c) The amount of titrant would be halved because the was diluted by half.
You are asked to prepare a buffer solution with a pH of 3.50. The following solutions, all 0.100 M, are available to you: HCOOH, CH3COOH, H3PO4 , NaCHOO, NaCH3COO, and NaH2PO4. What ratio of [conjugate base]/[acid] would yield the best result for the required buffer solution created in the question above? ENTER YOUR ANSWER AS ONE NUMBER ROUNDED TO TWO DECIMAL PLACES.
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4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH as a titrant in varying volumes. Calculate the pH of the solution at the following points: (Ka for HCN=6.2×10-¹0) (a) Before addition of NaOH (initial pH), (b) After 10.00 mL of titrant addition, (c) After 25.00 mL of titrant addition, (d) After 50.00 mL of titrant addition.
Consider the reaction of a 20.0 mL of 0.220 M C;H;NHCI (Ka = 5.9 x 10) with 12.0 mL of 0.239 M CSOH. Write the net ionic equation for the reaction that takes place. What quantity in moles of C;H;NH" would be present at the start of the titration? What quantity in moles of OH" would be present if 12.0 mL of OH were added? -What species would be left in the beaker after the reaction goes to completion? d. What quantity in moles of C,H,NH would be left in the beaker after the reaction goes to completion?
33. Consider a buffer solution that contains 0.45 M HCOOH and 0.55 M NaHCOO. Note that the Ka for formic acid (HCOOH) is 1.8 x 104. (a) Calculate the pH of this buffer solution. pH = (b) Write the net ionic chemical equation that occurs when potassium hydroxide (KOH) (MW of KOH = 56.1 g/mol) is added to the buffer. (c) If 0.260 g of solid KOH is added to 250. mL of this buffer solution, what is the resulting pH of the solution? New pH =
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