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: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.78QE

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You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
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A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
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