What are the concentrations of all the solute species in 0.150 M lactic acid, HC3HSO2? What is the pH of the solution? This acid has a Ka - 1.4 x 104. For the concentrations, use scientific notation where necessary, using the following notation: for example, an answer of 2.0 x 108 is typed as 2.0E-8. pH - [HC3H5O2] - [H+]- M. [CH302] -

What are the concentrations of all the solute species in 0.150 M lactic acid, HC3HSO2? What is the pH of the solution? This acid has a Ka - 1.4 x 104. For the concentrations, use scientific notation where necessary, using the following notation: for example, an answer of 2.0 x 108 is typed as 2.0E-8. pH - [HC3H5O2] - [H+]- M. [CH302] -

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 153AE: The following illustration displays the relative number of species when an acid, HA, is added to...

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Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
A solution is tested for pH and conductivity as pictured below: The solution contains one of the following substances: HCl. NaOH, NH4Cl. HCN, NH3, HF, or NaCN. If the solute concentration is about 1.0 M, what is the identity of the solute?
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Papaverine hydrochloride (abbreviated papH+Cl; molar mass = 378.85 g/mol) is a drug that belongs to a group of medicines called vasodilators, which cause blood vessels to expand, thereby increasing blood flow. This drug is the conjugate acid of the weak base papaverine (abbreviated pap; Kb = 8.33 109 at 35.0C). Calculate the pH of a 30.0-mg/mL aqueous dose of papH+Cl prepared at 35.0C. Kw at 35.0C is 2.1 1014.
Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
The following illustration displays the relative number of species when an acid, HA, is added to water. a. Is HA a weak or strong acid? How can you tell? b. Using the relative numbers given in the illustration, determine the value for Ka and the percent dissociation of the acid. Assume the initial acid concentration is 0.20 M.
The pH of a 0.10-M solution of caffeine is 11.16. Determine Kb for caffeine from these data: C8H10N4O2(aq)+H2O(l)C8H10N4O2H+(aq)+OH(aq)
You mix a solution of a strong acid with a pH = 4.0 and an equal volume of another strong acid solution having a pH = 6.0. Is the final pH less than 4.0, equal to 4.0, between 4.0 and 5.0, equal to 5.0, between 5.0 and 6.0, equal to 6.0, or greater than 6.0? Explain.