Based on the results obtained in the following table, which indicator has approximately a pka of 4?Acid-baseColor StandardsSampleindicatorAYYYYYYYYYYRRRYYYYYYYCВВВVRRRRYYYCCCCCCCCRRRCpH3.457891011121314LEGEND: R-red Y-yellow 0-orangeB-blueV-violetC-colorless P-pinkAR1.B.

The indicators are chemical compounds that show changes in color at a definite change in pH. Hence…

Based on the results obtained in the following table, which indicator has approximately a pka of 4? Acid-base Color Standards Sample indicator A R R R Y Y Y Y Y Y Y Y Y Y B R R R R Y Y Y Y Y Y Y R В B В Y Y Y В C C C C C C C C R R R R R C pH 1 2 3 4 5 6. 7 8. 9. 10 11 12 13 14 LEGEND: R-red Y-yellow O-orange B-blue V-violet C-colorless P-pink O D B. R B. Cl

Based on the results obtained in the following table, which indicator has approximately a pka of 4? Acid-base Color Standards Sample indicator A R R R Y Y Y Y Y Y Y Y Y Y B R R R R Y Y Y Y Y Y Y R В B В Y Y Y В C C C C C C C C R R R R R C pH 1 2 3 4 5 6. 7 8. 9. 10 11 12 13 14 LEGEND: R-red Y-yellow O-orange B-blue V-violet C-colorless P-pink O D B. R B. Cl

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 46E: Use Table 13-2 to order the following from the strongest to the weakest base. ClO2,H2O,NH3,ClO4

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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.
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.
Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
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)?
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Compare the percent dissociation of the acid in Exercise 21a with the percent dissociation of the acid in Exercise 21d. Explain the large difference in percent dissociation of the acid.
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?
Using an acetic acid/sodium acetate buffer solution, what ratio of conjugate base to acid will you need to maintain the pH at 5.00? Describe how you would prepare such a solution.
The indicator dinitrophenol is an acid with a Ka of 1.1104. In a 1.0104 -M solution, it is colorless in acid and yellow in base. Calculate the pH range over which it goes from 10% ionized (colorless) to 90% ionized (yellow).
A solution has a pH of 7.0. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. thymol blue b. bromthymol blue c. methyl red d. crystal violet
Is the monoprotic acid Y or the monoprotic acid Z the stronger acid in each of the following situations? a. At equal concentrations, Y dissociates to a greater extent than Z in water. b. Ka for Z is larger than Ka for Y. c. The equilibrium position for the dissociation of Y lies farther to the right than that for Z. d. Proton transfer to water occurs to a lesser extent for Z than for Y.
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.