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.
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
CHOOSE ALL THE FOLLOWING
5.
Example 2What is the pH of the solution that results when 0.093 g of Mg(OH)2 Ksp = 7.1 × 10–12 is mixed with(a) 75.0 mL of 0.0500 M HCl?(b) 100.0 mL of 0.0500 M HCl?(c) 15.0 mL of 0.0500 M HCl? (d) 30.0 mL of 0.0500 M MgCl2?
Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5.FW(propanoic acid) = 74.08 g/mol; FW(calcium propanoate) = 186.22 g/mol a) At what pH will a solution of propanoic acid and sodium propanoate best resist changes to its pH? How do you know? b) 75 g calcium propanoate Ca(CH3CH2COO)2 is diluted to 150.0 mL with deionized water. 50.0 mL of a 3.0 M propanoic acid solution is added. Determine the equilibrium concentrations of each species and the pH of the resulting solution.
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?
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
Analyzing pH & finding a concentration of a species in solution.
The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explain
The acetate ion, CH-COO", reacts with water as a weak base: CH,CO0 (aq) + H2O02 CH COOH(ag) + OH"(ag), with K-5.7x 10 10 at 25°C. If sodium acetate were dissolved in water to make a 0.35 M solution, what would be the resulting concentration of OH ? (M)