Procedure: Research on the pH of these common household liquids. Data: Solution pH pOH [H3O* [OH] 1) juice-lemon, orange, calamansi, or dalandan 2) vinegar 3) table salt dissolved in water 4) soap solution 5) baking soda so!ution 6) drain cleaner 7) dishwashing liquid 8) eyewash Computations: (Show pertinent computations for the completion of the data in the table above)

Procedure: Research on the pH of these common household liquids. Data: Solution pH pOH [H3O* [OH] 1) juice-lemon, orange, calamansi, or dalandan 2) vinegar 3) table salt dissolved in water 4) soap solution 5) baking soda so!ution 6) drain cleaner 7) dishwashing liquid 8) eyewash Computations: (Show pertinent computations for the completion of the data in the table above)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 17P

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Similar questions

A chilled carbonated beverage is opened and warmed to room temperature. Does the pH change and, if so, how does it change?
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.
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
Vitamin C is ascorbic acid (HC6H7O6), for which Ka is 8.0105. Calculate the pH of a solution made by dissolvinga 500-mg tablet of pure vitamin C in water anddiluting to 100 mL.
A weak acid, HA, is dissolved in water. Which one of the following beakers represents the resulting solution? (Water molecules have been omitted for clarity.)
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?
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
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.
Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a) What is the pH of a 0.100 M solution of HF at 100C? (b) Compare with the pH of a 0.100 M solution of HF at 25C.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Aluminum chloride, AlCl3, behaves more as a molecular compound than an ionic one. This is illustrated in its ability to form a fourth covalent bond with a chloride ion: AlCl3+ClAlCl4. From the Lewis diagram of the aluminum chloride molecule and the electron configuration of the chloride ion, show that this is an acidbase reaction in the Lewis sense, and identify the Lewis acid and the Lewis base. Aluminum chloride is a white solid at room conditions, although it is typically manufactured mixed with some yellow ironIII chloride. Its appearance is that of an ionic compound.
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?

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