The weak acid hydrofluoric acid, HF, and the strong base lithium hydroxide react to form the salt lithium fluoride, LiF. Given that the value of Ka for hydrofluoric acid is 3.50 x 104, what is the pH of a 0.185 M solution of lithium fluoride at 25 °C? • Your answer should have three significant figures. Provide your answer below: pH-

The weak acid hydrofluoric acid, HF, and the strong base lithium hydroxide react to form the salt lithium fluoride, LiF. Given that the value of Ka for hydrofluoric acid is 3.50 x 104, what is the pH of a 0.185 M solution of lithium fluoride at 25 °C? • Your answer should have three significant figures. Provide your answer below: pH-

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.49QE: Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen...

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Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
Acids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.
Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases. (a) hydrazoic add, HN3 (b) citric acid, H2C6H6O7 (c) squaric acid, H2C4O4
Classify each of the following substances as an acid, a base, or a salt. a. AlPO4 b. KOH c. HNO3 d. HC2H3O2
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?