The table shows respective color change when a universal indicator is added to the clear solutions. Rank the samples based on increasing order of acid strenc Solutions Color change 0.001 M lactic acid Light red 0.01 M phenol Light yellow 0.01 M nitrous acid Light orange 0.001 M hydrogen peraxide Light green Rank the solutions by increasing order of their acid strength. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help

The table shows respective color change when a universal indicator is added to the clear solutions. Rank the samples based on increasing order of acid strenc Solutions Color change 0.001 M lactic acid Light red 0.01 M phenol Light yellow 0.01 M nitrous acid Light orange 0.001 M hydrogen peraxide Light green Rank the solutions by increasing order of their acid strength. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help

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 58P

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Similar questions

. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Explain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
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)?
. Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.
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.
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.
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.