Answer the following question and indicate why. TABLE 16.1 Some Common Acid-Base IndicatorsColorIndicatorIn AcidIn BasepH RangeThymol blueRedYellow1.2-2.8Bromophenol blueYellowBluish purple3.0-4.6Methyl orangeОгangeYellow3.1-4.4Methyl redRedYellow4.2-6.3Chlorophenol blueYellowRed4.8-6.4Bromothymol blueYellowBlue6.0-7.6Cresol redYellowRed7.2-8.8PhenolphthaleinColorlessReddish pink8.3-10.0*The pl range is defined as the mnge over which the indicator changes from the acid color to the base color.9. Referring to Table 16.1, specify which indicator or indicators you would use for the following titrations:а нсоон versus NaOHb. HCI versus KOHc. HNO3 versus CH3NH2

a) Here HCOOH is a weak acid and NaOH is a strong base. Since it is a titration of strong base vs…

TABLE 16.1 Some Common Acid-Base Indicators Color In Base Indicator In Acid pH Range Thymol blue Bromophenol blue Red Yellow 1.2-2.8 Yellow Bluish purple 3.0-4.6 Methyl orange Огаnge Yellow 3.1-4.4 Methyl red Red Yellow 4.2-6.3 Chlorophenol blue Yellow Red 4.8-6.4 Bromothymol blue Cresol red Phenolphthalein Yellow Blue 6.0-7.6 Yellow Red 7.2-8.8 Colorless Reddish pink 8.3–10.0 *The pi range is defined as the nage over which the indicator changes from the acid color to the base color. 9. Referring to Table 16.1, specify which indicator or indicators you would use for the following titrations: a HCOOH versus NaOH b. HCI versus KOH C. HNO3 versus CH3NH2

TABLE 16.1 Some Common Acid-Base Indicators Color In Base Indicator In Acid pH Range Thymol blue Bromophenol blue Red Yellow 1.2-2.8 Yellow Bluish purple 3.0-4.6 Methyl orange Огаnge Yellow 3.1-4.4 Methyl red Red Yellow 4.2-6.3 Chlorophenol blue Yellow Red 4.8-6.4 Bromothymol blue Cresol red Phenolphthalein Yellow Blue 6.0-7.6 Yellow Red 7.2-8.8 Colorless Reddish pink 8.3–10.0 *The pi range is defined as the nage over which the indicator changes from the acid color to the base color. 9. Referring to Table 16.1, specify which indicator or indicators you would use for the following titrations: a HCOOH versus NaOH b. HCI versus KOH C. HNO3 versus CH3NH2

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter17: Acid-base(proton Transfer) Reactions

Section: Chapter Questions

Problem 8E: Aluminum chloride, AlCl3, behaves more as a molecular compound than an ionic one. This is...

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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.
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.
The pH and electrical of 4 differnt mixures were measured: (Table on picture) a Explain why the conductivity of mixture A is higher than that of mixture B, yet the pH of A is lower than the pH of B. Include relevant equations in your answer.b Explain why the pH of mixture C is the same as the pH of mixture A.c Why is the conductivity of mixture C larger than the conductivity of mixture A?d Why is the pH of mixture D the same as the pH of mixture B? Determine the final pH for the following two solutionsa) Solution A after mixing 500mL 0.2M HCl and 300 mL 0.6M HClb) Solution B after mixing 400mL 0.3M HCl and 200mL 0.8M NaOH
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