Chemistry What is the color of bromthymol blue indicator at pH 7, the midpoint at which yellowand blue are in equal concentration?Select one:O A. greenO B. orangeO C. yellowO D. blueO E. red

Bromthymol blue is a pH indicator that changes color based on the acidity or basicity of a solution.…

Answered: What is the color of bromthymol blue…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 79E

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Similar questions

Compare the percent ionization of the base in Exercise 22a with the percent ionization of the base in Exercise 22d. Explain any differences.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific 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.
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.
Phthalic acid, H2C8H4O4, is a diprotic acid used in the synthesis of phenolphthalein indicator. Ka1 = 1.2 103, and Ka2 = 3.9 106. a Calculate the hydronium-ion concentration of a 0.015 M solution. b What is the concentration of the C8H4O42 ion in the solution?
. For each hydrogen or hydroxide ion concentration listed. calculate the concentration of the complementary ion and the pH and pOH of the solution. a. [H+]=5.72104M b. [OH-]=8.91105Mc. [H+]=2.871012Md. [OH-]=7.22108M
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Each of the following statements concerns a 0.010 M solution of a weak acid, HA. Briefly describe why each statement is either true or false. a [HA] is approximately equal to 0.010 M. b [HA] is much greater than [A]. c [OH] is approximately equal to [H3O+]. d The pH is 2. e The H3O concentration is 0.010 M. f [H3O+] is approximately equal to [A].
A solution contains 0.675 g of ethylamine, C2H5NH2, per 100.0 mL of solution. Electrical conductivity measurements at 20C show that 0.98% of the ethylamine has reacted with water. Write the equation for this reaction. Calculate the pH of the solution.
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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.
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)?

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What is the color of bromthymol blue indicator at pH 7, the midpoint at which yellow and blue are in equal concentration? Select one: O A. green O B. orange O C. yellow O D. blue O E. red