Answered: Ka = 5.0 x 1010 for formic acid, CHOOH.…

Ka = 5.0 x 1010 for formic acid, CHOOH. Given a 0.20 mol/L of this acid solution, calculate the following: a) [H] b) pH c) pOH

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.118EP: Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer...

See similar textbooks

Similar questions

Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
CH3CH2CO2H , Ką = 1.3 x 105 CH3CH2CO2 , Kp = 7.7 x 10-10 F, Kp = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For the reaction between propanoic acid (CH3CH2CO2H) and a solution containing fluoride ions (F"): (a) The name of the conjugate base produced is (b) The name of the conjugate acid produced is (c) The reaction is favoured (write 'reactant' or 'product'), because the reactants are the (write 'weaker' or 'stronger') set of acid and base.
Consider the following chemical equilibrium for the weak base CN in water: CN (aq) + H₂O(1) HCN(aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d H pH will go up; [OH-]will go up; net amount of OH will go up pH will go down; [OH-] will go up; net amount of OH will go down pH will go down: [OH-] will go down; net amount of OH will go down pH will go up; [OH will go up; net amount of OH will go down X Your answer
The values of Ka for hydrozoic acid (HN3) and hypobromous acid (HBrO) are given below. HN3 Ka = 1.9 × 10-5 HBrO Ka = 2.0 × 10-9 If we mix 0.50 mol HN3 and 0.50 mol NaBrO into a 1-L aqueous solution, which of the following statements is correct concerning the final solution at equilibrium after mixing? Choose one option only. Options: a. The pH of the final solution is less than 7 because Ka (HN3) < Kb( BrO- ). b. The pH of the final solution is greater than 7 because Ka (HN3) > Kb(BrO-). c. The pH of the final solution is equal to 7 because the neutralization reaction between HN3 and NaBrO. d. The pH of the final solution is less than 7 because Ka (HN3) > Kb( BrO- ). e. The pH of the final solution is greater than 7 because Ka (HN3) < Kb( BrO- ).
PR: (a) Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 800. mL of solution. (10). (b) Calculate the pH after 0.050 moles of NaOH are added to the buffer solution (assume no volume change) (10). Ka (HCNO) = 2.0 × 10-4
CHOOSE ALL THE FOLLOWING
A student is provided with a 0.1 M stock solution of NaOH. Student was then asked to mix 50.0 mL of this stock solution of NaOH with 450.0 mL of water to prepare a dilute solution of NaOH. (A) Calculate the molarity of the diluted solution. (B). Calculate the hydronium ion concentration, [H3O+] in the final diluted solution. (8 points) (C ) Calculate the pH of the diluted NaOH solution. (D) Is the final diluted solution acidic, basic or neutral?
The acid dissociation constants for sulfurous acid are: Ka1 3D 1.2 х 10-2 and Ka2 - 6.6 х 10-8 (a) Calculate the pH of a solution of 0.10 M H2SO3. (b) Calculate the pH of a solution of 0.10 M Na2SO3. (c) Calculate the pH of the solution resulting when equal volumes of the solutions described in parts (a) and (b) are mixed.
Consider a 1.0-L solution that is 0.280 M C5H5N and 0.46 M C5H5NHCl at 25 °C. What is the pH of this solution before and after 0.01 moles of NaOH have been added? Kb of C5H5N is 1.7E-9 the correct answer is pH=5.01; pH=5.04 Looking for an explanation.
shobha
7
< 9:58 Question 39 of 45 A) 0.50 M HF and 0.20 M NaF Which of the following solutions has the highest H* concentration? B) 0.50 M HF and 0 M NaF C) 0.50 M HF and 0.50 M NaF D) 0.50 M HF and 0.70 M NaF 294 Tap here or pull up for additional resources Submit