ChemistryHow do I calculate the equilibrium constantsfor the reactions with the given Ka and Kbvalues? Thanks!Complete the following reactions and calculate the corresponding equilibrium constants using, whenappropriate, the information: Ka(HF) = 6.8 x 104, and Kь(CH3NH₂) = 4.4 x 10-4.a) HCl(aq) + NaOH(aq) -b) HF(aq) + NaOH(aq) +c) CH3NH₂(aq) + HCl(aq) →→→1

Answered: Image /qna-images/answer/0a76d0b7-c6c4-48e5-9e49-a0ac2a042122.jpg

ite the corresponding equilibrium constants using, when appropriate, the information: Ka(HF) = 6.8 x 104, and Kb(CH3NH₂) = 4.4 x 10-4, a) HCl(aq) + NaOH(aq) + b) HF(aq) + NaOH(aq) - c) CH3NH2(aq) + HCl(aq) +

ite the corresponding equilibrium constants using, when appropriate, the information: Ka(HF) = 6.8 x 104, and Kb(CH3NH₂) = 4.4 x 10-4, a) HCl(aq) + NaOH(aq) + b) HF(aq) + NaOH(aq) - c) CH3NH2(aq) + HCl(aq) +

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

If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00125 M, determine the bicarbonate ion (HCO3-) concentration required to buffer the pH of blood at pH = 7.40. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7 Show all calculations including equation(s) used.
The pH for 0.0850 M solution of CoHsCH2COOH is 2.68. Determine the value of Ka for CoHsCH2COOH. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C&H:CH2COOH(a_ H2O(1) H;O*(aq) CoHsCH2CO0 (aq) q) Initial (M) Change (M) Equilibrium (M) RESET 0.0850 2.68 -2.68 2.1 x 10-3 -2.1 x 10 3 0.0829 -0.0829 0.428 -0.428 +x 2.68 + x 2.68 - x 2.1 x 10-3 + x 2.1 x 10-3-x 0.428 + x 0.428 x
For the following reactions, write Ka or Kb expressions (as appropriate) and predict in which direction the equilibrium will lie if the initial concentration of aqueous reactant is 0.10 M.a) HCl(aq) + H2O(l) ⇌ H3O+(aq) + Cl–(aq)b) HClO(aq) + H2O(l) ⇌ H3O+(aq) + OCl–(aq)c) (CH3)3N(aq) + H2O(l) ⇌ (CH3)3NH+(aq) + OH–(aq)d) Ca(OH)2(aq) ⇌ Ca+(aq) + 2HO–(aq)
(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.
Calculate the K of A" given HA(aq) + H2O(l) = H₂O† (aq) + A¯¯(aq) K = 5.90×108
The strongest known acid is fluoroantimonic acid, [H₂F][SbF6]. It is 1016 times more acidic than concentrated sulfuric acid and has a pH of -31.3; it is strong enough to protonate both xenon and molecular hydrogen. It is an ionic liquid made by reacting hydrogen fluoride with antimony(V) fluoride: 2 HF + SbF5 → H₂F+ + SbF6 Explain why this acid is so strong.
Calculate the [NH₃] in a solution of 0.250 M ammonium fluoride (NH₄F). Hint: Use the Ka of HF (6.8 × 10⁻⁴) and the Kb of NH₃ (1.8 × 10⁻⁵) to calculate Kc for the reaction NH₄⁺(aq) + F⁻(aq) ⇌ NH₃(aq) + HF(aq). Want solution ASAP Your answer
A solution is prepared at 25 °C that Is initlally 0.43M in dimethylamine ((CH, NH, a weak base with K, =5.4x10, and 0.15M in dimethylammonlum -4 and 0.15M In dimethylammonium bromide ((CH,),NH,Br) ((CH,) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. bгomide 2. pH Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privac hp
Calculate the pH of a weak base which dissociates as BOH ⇌ B+ + OH- ( like NH3 (g) + H2O(l) → NH4OH(aq) , where in water NH4OH ⇌ NH4+ + OH- ) knowing that the initial concentration of the base is 0.86 M, and the base dissociation constant, Kb , is 1.39e-7.
Calculate the equilibrium concentration of HC2O4−HC2O4− in a 0.20 mol L−1mol L−1 solution of oxalic acid. Express your answer to two significant figures and include the appropriate units
The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5. What will be the pH of a 0.10 M HC2H3O2 solution which is 0.10 M in NaC2H3O2
9) The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid, H₂X+) are Kal = 4.6 × 10-3 and Ka2=2.0 × 10-10. What is the pH of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been added? Para Ofind moles