PhMconductivityраз 9701 520Ph1'sasecDiluted bleach03 Pl60 Vрausip"Diluted virger 3Conductivitys2580us 15730.01M HL0.01M NaOH122. Using the pH values obtained above, calculate the H3O+ concentration for:a. Diluted bleach sample:19JEb. Diluted vinegar sample:3. Calculate the expected pH for the solutions below:a. 0.01 M HCI (aq)b. 0.01 M NaOH (aq)4. Experimental data does not always match expected results due to errors. Based onhan list species

3. The expected pH of 0.01M HCL is as follows:pH=−log[H+]pH=−log[0.01]pH=−log[10−2]pH=2log[10]pH=2…

Answered: Ph M conductivity раз 970 1 520 Ph 1'…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.34QAP

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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.
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.
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.
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
Consider a weak organic base (nonelectrolyte) with molar mass 281 g/mol. An aqueous solution of the base has a pH of 8.73 and an osmotic pressure of SS mm Hg at 25C. What is Kb for the weak base?
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?
Calculate the concentration of all solute species in each of the following solutions of acids or bases. Assume that the ionization of water can be neglected, and show that the change in the initial concentrations can be neglected, Ionization constants can be found in Appendix H and Appendix I. (a) 0.0092 M HCIO, a weak acid. (b) 0.0784 M C6H5NH2, a weak base. (c) 0.0810 M HCN, a weak acid. (d) 0.11 M (CH3)3N, a weak base. (e) 0.120 M Fe(H2O)62+ a weak acid, Ka=1.6107
A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C tablet is dissolved in enough water to make 200.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid.
Compare the percent ionization of the base in Exercise 22a with the percent ionization of the base in Exercise 22d. Explain any differences.
Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the ratio [C5H5N]/[C5H5NH+] if the solution has the following pH values: a. pH = 4.50 b. pH = 5.00 c. pH = 5.23 d. pH = 5.50
Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.
A solution of an unknown weak base (nonelectrolyte) at 25C has an osmotic pressure of 1.287 atm and a pH of 8.94. (Assume that, in the equation for [Chapter 101,i1.) What is Ka for its conjugate acid?

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