The Henderson-Hasselbalch equation can be written as p H = p K a − log ( 1 a − 1 ) where a = [ A − ] [ A − ] + [ H A ] . Thus, the degree of ionization (a) of an acid can be determined W both the pH of the solution and the p K g , of the acid are known a. Use this equation to plot the pH versus tie degree of ionization for me second ionization constant of phosphoric acid ( K 8 = 6.3 × 10 − 8 ) b. If p H = p K a what is the degree of ionization? c. If the solution had a pH of 6.0, what would the value of a be?
The Henderson-Hasselbalch equation can be written as p H = p K a − log ( 1 a − 1 ) where a = [ A − ] [ A − ] + [ H A ] . Thus, the degree of ionization (a) of an acid can be determined W both the pH of the solution and the p K g , of the acid are known a. Use this equation to plot the pH versus tie degree of ionization for me second ionization constant of phosphoric acid ( K 8 = 6.3 × 10 − 8 ) b. If p H = p K a what is the degree of ionization? c. If the solution had a pH of 6.0, what would the value of a be?
Solution Summary: The author explains how the pH value of a solution is determined by using the Henderson Hasselbalch equation.
The Henderson-Hasselbalch equation can be written as
p
H
=
p
K
a
−
log
(
1
a
−
1
)
where
a
=
[
A
−
]
[
A
−
]
+
[
H
A
]
. Thus, the degree of ionization (a) of an acid can be determined W both the pH of the solution and the
p
K
g
, of the acid are known
a. Use this equation to plot the pH versus tie degree of ionization for me second ionization constant of phosphoric acid
(
K
8
=
6.3
×
10
−
8
)
b. If
p
H
=
p
K
a
what is the degree of ionization?
c. If the solution had a pH of 6.0, what would the value of a be?
You are given a 27 % (w/v) solution of psicose.
Molar mass: psicose (C6H12O6) = 180.156 g/mol.
You dissolve 6.31 g of potassium formate in 250 mL of 0.25 M formic acid (HCOOH).
This solution was then made up to a total volume of 500 mL with distilled water.
Potassium formate (KHCO2): molar mass = 84.12 g/mol
Calculate the pH of this solution given the pKa of formic acid = 3.77.
The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?
A 0.025 M solution of an unknown organic acid has a pH of 3.23.
2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
Chapter 17 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.