Formic acid has uses in preservatives, cleaning agents, beekeeping and a growing list of potential uses. The pKa for formic acid is 3.75. What is the pH of a 0.200 M formic acid solution? What is the concentration of formate, the conjugate base of formic acid, in the solution at equilibrium? What percent of lactic acid is "ionized" or reacted? Enter your final answers into the table below. Round your answers to 2 significant figures. pH of 0.200 M solution (6 pt) [formate] (the conjugate base of formic acid) (2 pt) % reacted (2 pt) pH = M %

Formic acid has uses in preservatives, cleaning agents, beekeeping and a growing list of potential uses. The pKa for formic acid is 3.75. What is the pH of a 0.200 M formic acid solution? What is the concentration of formate, the conjugate base of formic acid, in the solution at equilibrium? What percent of lactic acid is "ionized" or reacted? Enter your final answers into the table below. Round your answers to 2 significant figures. pH of 0.200 M solution (6 pt) [formate] (the conjugate base of formic acid) (2 pt) % reacted (2 pt) pH = M %

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 34Q: Which of the following statements is(are) true? Correct the false statements. a. When a base is...

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For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
In a particular solution, acetic acid is 11% ionized at 25 C. Calculate the pH of the solution and the mass of acetic acid dissolved to yield 1.00L of solution.
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
A certain sample of rainwater gives a yellow color with methyl red and a yellow color with bromthymol blue. What is the approximate pH of the water? Is the rainwater acidic, neutral, or basic? (See Figure 15.10.)
Which of the following statements is(are) true? Correct the false statements. a. When a base is dissolved in water, the lowest possible pH of the solution is 7.0. b. When an acid is dissolved in water, the lowest possible pH is 0. c. A strong acid solution will have a lower pH than a weak acid solution. d. A 0.0010-M Ba(OH)2 solution has a pOH that is twice the pOH value of a 0.0010-M KOH solution.
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in Table 13-3. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?
Thymolphthalein is an indicator that changes from colorless to blue at pH 9.5. (a) What is its Ka? (b) What is its pH range? (c) What is the color of a solution with a pH of 10.0 and a few drops of thymolphthalein?
Two strategies are followed when solving for the pH of an acid in water. What is the strategy for calculating the pH of a strong acid in water? What major assumptions are made when solving strong acid problems? The best way to recognize strong acids is to memorize them. List the six common strong acids (the two not listed in the text are HBr and HI). Most acids, by contrast, are weak acids. When solving for the pH of a weak acid in water, you must have the Ka value. List two places in this text that provide Ka values for weak acids. You can utilize these tables to help you recognize weak acids. What is the strategy for calculating the pH of a weak acid in water? What assumptions are generally made? What is the 5% rule? If the 5% rule fails, how do you calculate the pH of a weak acid in water?
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?