When 25 mL of 0.12 M aqueous ammonia is titrated with 0.12 M hydrobromic acid, what is the pH at the equivalence point?X Incorrect.10.2Equivalence point pH =Use correct number of significant digits;X Incorrect.Using the table below, select all indicators that could be used for the titration given above.Approximate pH Range overwhich the Color ChangesColor Change(lower to higher pH)IndicatorMethyl greenYellow to blue0.2-1.8Thymol blue1.2-2.8Yellow to blueMethyl orange3.2-4.4Red to yellowEthyl red4.0-5.8Colorless to redMethyl purplePurple to greenYellow to purple4.8-5.4Bromocresol purple5.2-6.8Bromothymol blue6.0-7.6Yellow to bluePhenol red6.4-8.2Yellow to red/violetLitmus4.7-8.3Red to blueCresol red7.0-8.8Yellow to redThymol blue8.0-9.6Yellow to blue Phenolphthalein8.2–10.0Colorless to pinkThymolphthalein9.4-10.6Colorless to blueAlizarin yellow R10.1-12.0Yellow to redClayton yellow12.2–13.2Yellow to amberlitmusbromothymol bluemethyl orangemethyl greenethyl redthymol bluemethyl purpleclayton yellowphenol redbromocresol purplecresol redthymol bluephenolphthaleinthymolphthaleinalizarin yellow R

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When 25 mL of 0.12 M aqueous ammonia is titrated with 0.12 M hydrobromic acid, what is the pH at the equivalence point?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

When 25 mL of 0.12 M aqueous ammonia is titrated with 0.12 M hydrobromic acid, what is the pH at the equivalence point?
X Incorrect.
10.2
Equivalence point pH =
Use correct number of significant digits;
X Incorrect.
Using the table below, select all indicators that could be used for the titration given above.
Approximate pH Range over
which the Color Changes
Color Change
(lower to higher pH)
Indicator
Methyl green
Yellow to blue
0.2-1.8
Thymol blue
1.2-2.8
Yellow to blue
Methyl orange
3.2-4.4
Red to yellow
Ethyl red
4.0-5.8
Colorless to red
Methyl purple
Purple to green
Yellow to purple
4.8-5.4
Bromocresol purple
5.2-6.8
Bromothymol blue
6.0-7.6
Yellow to blue
Phenol red
6.4-8.2
Yellow to red/violet
Litmus
4.7-8.3
Red to blue
Cresol red
7.0-8.8
Yellow to red
Thymol blue
8.0-9.6
Yellow to blue

Phenolphthalein
8.2–10.0
Colorless to pink
Thymolphthalein
9.4-10.6
Colorless to blue
Alizarin yellow R
10.1-12.0
Yellow to red
Clayton yellow
12.2–13.2
Yellow to amber
litmus
bromothymol blue
methyl orange
methyl green
ethyl red
thymol blue
methyl purple
clayton yellow
phenol red
bromocresol purple
cresol red
thymol blue
phenolphthalein
thymolphthalein
alizarin yellow R

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