What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators HIn → In- pH range Solution X methyl orange red-yellow 3.2-4.4 yellow methyl red red-yellow 4.8-6.0 yellow bromthymol blue yellow-blue 6.0-7.6 green phenolphthalein colorless-pink 8.2-10.0 colorless 8.2-10.0 3.2 -4.4 6.0 - 7.6 4.8-6.0

What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators HIn → In- pH range Solution X methyl orange red-yellow 3.2-4.4 yellow methyl red red-yellow 4.8-6.0 yellow bromthymol blue yellow-blue 6.0-7.6 green phenolphthalein colorless-pink 8.2-10.0 colorless 8.2-10.0 3.2 -4.4 6.0 - 7.6 4.8-6.0

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 9RQ: What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a...

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Similar questions

What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
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?
The common ion effect for weak acids is to significantly decrease the dissociation of the acid in water. Explain the common ion effect.
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)?