Please provide only typed answer solution no handwritten solution needed allowedPlease do it all instant positive rating MISSED THIS? Read Section18.2 (Pages 788-799): Watch KCV 18.28.IWE 18.2.Solve an equilibrium problem (using an ICE table)to calculate the pH of each of the followingsolutions.Express your answer using two decimal places.PHMSubmitPart CΑΣΦpH =Request Answera mixture that is 0.17 M in CH₂NH₂ and 0.17 M in CH₂NH,CIExpress your answer using two decimal places.VO ΑΣΦ MISSED THIS? Read Section18.2 (Pages 788-799): Watch KCV 18.28.WE 18.2.Solve an equilibrium problem (using an E table)to calculate the pH of each of the followingsolutions.com/myct/item/viewTassignment ProblemiD-200959836YPart A0.17 M CH3NH₂ (where K, for CH₂NH₂ is 4.4 x 10-¹)Express your answer using two decimal places.15. ΑΣΦpH =SubmitPart BRequest Answer0.17 M CH,NH,C1Express your answer using two decimal places.pH =IVE ΑΣΦΑ?

Given - 0.17 M CH3NH2 Kb for CH3NH2 = 4.4 × 10 -4 CH3NH2 Is weak base therefore…

MISSED THIS? Read Section 18.2 (Pages 788-799): Watch KCV 18.28. IWE 18.2. Solve an equilibrium problem (using an E table) to calculate the pH of each of the following solutions. com/nyct/itentViewTassignment ProblemiD-200959836 Part A 0.17 M CH3NH₂ (where K₁, for CH₂NH₂ is 4.4 x 10) Express your answer using two decimal places. 15. ΑΣΦ PH Submit Part B Request Answer 0.17 M CHÍNH,CH Express your answer using two decimal places. VE ΑΣΦΑ pH =

MISSED THIS? Read Section 18.2 (Pages 788-799): Watch KCV 18.28. IWE 18.2. Solve an equilibrium problem (using an E table) to calculate the pH of each of the following solutions. com/nyct/itentViewTassignment ProblemiD-200959836 Part A 0.17 M CH3NH₂ (where K₁, for CH₂NH₂ is 4.4 x 10) Express your answer using two decimal places. 15. ΑΣΦ PH Submit Part B Request Answer 0.17 M CHÍNH,CH Express your answer using two decimal places. VE ΑΣΦΑ pH =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 127QRT

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In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…