In Experiment 4, you used phenolphthalein HIn as indicator in titrating the acid content of samples. The indicator forms this equilibrium in an aqueous solution: HIn + H2O ↔ H3O+ + In-. During the course of the titration, the concentration of H3O+___________, shifting the equilibrium towards ___________ , until end-point is reached. a. decreases, HIn b.increases, In- c. increases, HIn d.decreases, In-

In Experiment 4, you used phenolphthalein HIn as indicator in titrating the acid content of samples. The indicator forms this equilibrium in an aqueous solution: HIn + H2O ↔ H3O+ + In-. During the course of the titration, the concentration of H3O+_, shifting the equilibrium towards _ , until end-point is reached. a. decreases, HIn b.increases, In- c. increases, HIn d.decreases, In-

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 9P

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How to distinguish between an Acidic Buffer and Acidic Solution as well as Basic Buffer and Basic Solution? Is it based on the color exhibited sol. w/ indicator or pH level of a solution? Ex. Solution 1: 30.0 mL 0.10 M CH3COOH Solution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COO Both used methyl orange as indicator Solution Observed Color & Estimated pH range Classification (acidic/basic & buffer/solution) 1 a 1.0 M HCl Red pH < 3.1 (2.01pH) b 1.0 M NaOH Orange 3.1 < pH < 4.5 (3.98pH) c Control Red pH < 3.1 (2.91pH) 2 a 1.0 M HCl Yellow pH > 4.5 (4.73) b 1.0 M NaOH Yellow pH > 4.5 (4.82) c Control Yellow pH > 4.5 (4.76)
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1. The reaction of ??? with ???3 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq) ---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (???3) when 40.5−?? of 0.674 ? ???is required to quench 101.0?? of Nitric acid over phenolphthalein indicator.
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An acid-base indicator is usually a weak acid with a characteristic color in the protonated and deprotonated forms. In this assignment, you will monitor the color of an acetic acid solution containing Bromocresol Green as an indicator, as the pH is changed and then you will estimate the ionization constant, Ka, for the indicator. This is a lab I have to do. I have it done I just need an introduction to it. It was on Ionization Constants of Weak Acids Example of first question. Rememember just need. wirtten introduction. Thank you!
An acid-base indicator is usually a weak acid with a characteristic color in the protonated and deprotonated forms. In this assignment, you will monitor the color of an acetic acid solution containing Bromocresol Green as an indicator, as the pH is changed and then you will estimate the ionization constant, Ka, for the indicator. 1. Start Virtual ChemLab, select Acid-Base Chemistry, and then select Ionization Constants of Weak Acids from the list of assignments. The lab will open in the Titration laboratory. Bottles of 0.1104 M NaOH and 0.1031 M HAc (acetic acid) will be on the lab bench. The buret will be filled with the NaOH solution and a beaker containing 10.00 mL of the HAc solution will be on the stir plate. The stir plate will be on, Bromocresol Green indicator will have been added to the beaker, and a calibrated pH probe will also be in the beaker so the pH of the solution can be monitored. 2. What is the color and pH of the solution? Yellow, 2.87 3. On the…
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