Use the table of indicators below to choose the most appropriate indicator to use when titrating Fill in the blanks by selecting benzoic acid with sodium hydroxide as described in the previous problem -- one option from each menu. methyl orange thymol blue 5 points Thymol blue Bromophenol blue Methyl orange Bromocresol green Methyl red Bromthymol blue Litmus Phenolphthalein bromocresol green methyl red bromophenol blue Alizarin yellow R T 0 1 2 3 4 6 7 9 10 11 12 13 PH

Use the table of indicators below to choose the most appropriate indicator to use when titrating Fill in the blanks by selecting benzoic acid with sodium hydroxide as described in the previous problem -- one option from each menu. methyl orange thymol blue 5 points Thymol blue Bromophenol blue Methyl orange Bromocresol green Methyl red Bromthymol blue Litmus Phenolphthalein bromocresol green methyl red bromophenol blue Alizarin yellow R T 0 1 2 3 4 6 7 9 10 11 12 13 PH

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter22: Properties Of Systems In Chemical Equilibrium-le Chatelier's Principle

Section: Chapter Questions

Problem 1ASA: Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the...

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Similar questions

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.
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
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?
Identify two oxides that are key producers of acid rain. Write chemical equations that illustrate how these oxides form acid rain.
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
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.
Water is not the only solvent that undergoes autoionization. Write the equation for the autoionization of acetic 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?
Define each of the following: a. Arrhenius acid b. BrnstedLowry acid c. Lewis acid Which of the definitions is most general? Write reactions to justify your answer.
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.
Do you expect a solution of anilinium chloride (aniline hydrochloride). C6H5NH3Cl, to be acidic or basic? (Anilinium chloride is the salt of aniline and hydrochloric acid.) Write the equation for the reaction involved. What is the equilibrium expression? How would you obtain the value for the equilibrium constant from Table 16.2?
Classify each of the following statements as true or false: aAll Brnsted-Lowry acids are Arrhenius acids. bAll Arrhenius bases are Brnsted-Lowry bases, but not all Brnsted-Lowry bases are Arrhenius bases. c HCO3 is capable of being amphoteric. d HS is the conjugate base of S2. eIf the species on the right side of an ionization equilibrium are present in greater abundance than those on the left, the equilibrium is favored in the forward direction. f NH4+ cannot act as a Lewis base. gWeak bases have a weak attraction for protons. hThe stronger acid and the stronger base are always on the same side of a proton transfer reaction equation. iA proton transfer reaction is always favored in the direction that yields the stronger acid. jA solution with pH=9 is more acidic than one with pH=4. kA solution with pH=3 is twice as acidic as one with pH=6. lA pOH of 4.65 expresses the hydroxide ion concentration of a solution in three significant figures.

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