The indicator methyl red has a p K HIN = 4.95 . It changes born red to yellow over the pH range from 4.4 to 6.2. a. If the indicator is placed in a buffer solution of pH= 4.55,what percent of the indicator will, be present in the acid form. Hin, and what percent Will, be present in the base or anion form, In - ? b. Which form of the indicator has the “stronger”(that is more visible) color—the acid (red) form or base (yellow) form? Explain
The indicator methyl red has a p K HIN = 4.95 . It changes born red to yellow over the pH range from 4.4 to 6.2. a. If the indicator is placed in a buffer solution of pH= 4.55,what percent of the indicator will, be present in the acid form. Hin, and what percent Will, be present in the base or anion form, In - ? b. Which form of the indicator has the “stronger”(that is more visible) color—the acid (red) form or base (yellow) form? Explain
The indicator methyl red has a
p
K
HIN
=
4.95
. It changes born red to yellow over the pH range from 4.4 to 6.2. a. If the indicator is placed in a buffer solution of pH= 4.55,what percent of the indicator will, be present in the acid form. Hin, and what percent Will, be present in the base or anion form, In-? b. Which form of the indicator has the “stronger”(that is more visible) color—the acid (red) form or base (yellow) form? Explain
A certain indicator, HA, has a ?a value of 7.9×10^−7. The protonated form of the indicator is yellow and the ionized form is red.
What is the p?a of the indicator?
p?a=
A generic salt, AB2, has a molar mass of 287g/mol and a solubility of 2.80 g/L at 25 °C.
AB2(s)↽−−⇀A2+(aq)+2B−(aq)
What is the ?sp of this salt at 25 °C?
?sp=
The indicator methyl red has a pKHIn = 4.95. It changes from red to yellow over the pH range from 4.4 to 6.2.
If the indicator is placed in a colourless buffer solution of pH = 4.55, what percent of the indicator will be present in the acid form, HIn?
What colour would you expect the solution in question 13 above to most look like?
Select one:
a. red
b. colourless
c. magenta
d. yellow
A 1.0 liter solution contains 0.745 M hydrogen fluoride (HF) and 0.786 M sodium fluoride (NaF). What is the pH of this solution? (Ka for HF is 7.2 x 10 –4)
How many moles of solid sodium acetate would have to be added to 2.0 L of 0.293 M acetic acid solution to achieve a buffer of pH 4.77? Assume there is no volume change. Ka for HC2H3O2 is 1.8 × 10 –5
What molar ratio of sodium acetate to acetic acid, is required to create a buffer solution having a pH of 4.58 at 25°C? Ka for HC2H3O2 is 1.8 × 10 –5.
Chapter 17 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell