Spontaneity of given reaction should be explained, when addition of given buffer to the cell. Concept introduction: Cell potential (EMF): The maximum potential difference between two electrodes of voltaic cell is known as cell potential. If standard reduction potentials of electrodes are given the cell potential (EMF) is given by, E cell = E cathode -E anode Where, E cathode is the reduction half cell potential E anode is the oxidation half cell potential Nernst equation: The relationship between standard cell potential and cell potential at non standard conditions and the reaction quotient are given by Nernst equation it is, E cell = E° cell - 0.0592 n logQ Where, E cell is cell potential E° cell is standard cell potential Q is reaction quotient n isnumber of electrons pH : Ph of the solution is nothing but the concentration of Hydrogen ion in given solution in given condition and it is given by negative logarithm of base ten Hydrogen ion concentration. pH=-log[H + ]
Spontaneity of given reaction should be explained, when addition of given buffer to the cell. Concept introduction: Cell potential (EMF): The maximum potential difference between two electrodes of voltaic cell is known as cell potential. If standard reduction potentials of electrodes are given the cell potential (EMF) is given by, E cell = E cathode -E anode Where, E cathode is the reduction half cell potential E anode is the oxidation half cell potential Nernst equation: The relationship between standard cell potential and cell potential at non standard conditions and the reaction quotient are given by Nernst equation it is, E cell = E° cell - 0.0592 n logQ Where, E cell is cell potential E° cell is standard cell potential Q is reaction quotient n isnumber of electrons pH : Ph of the solution is nothing but the concentration of Hydrogen ion in given solution in given condition and it is given by negative logarithm of base ten Hydrogen ion concentration. pH=-log[H + ]
Solution Summary: The author explains that the Spontaneity of given reaction should be explained when adding a buffer to the cell.
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
The relationship between standard cell potential and cell potential at non standard conditions and the reaction quotient are given by Nernst equation it is,
Ph of the solution is nothing but the concentration of Hydrogen ion in given solution in given condition and it is given by negative logarithm of base ten Hydrogen ion concentration.
What will happen if the pH of the following equilibrium system is increased?
H*(aq) + 2CrO4²a
yellow
The solution will turn yellow.
b. The solution will turn a darker orange.
There will be no effect on the equilibrium system.
2-
aq) O Cr20,² (aq)
+ OH
(аq)
orange
а.
с.
d. The concentration of OH
will decrease.
(aq)
All hydroxide ion will be used up.
е.
A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x
104) and 1.00M potassium fluoride, KF. The total volume was 250 mL.
(a) What ions and molecules are present in the solution? List them in order of decreasing
concentration:
Decreasing order of Concentration
(b) What is the pH of the buffer solution described above?
(c) What is the pH of 100. mL of the buffer solution if you add 100. x 10-3 g of NaOH? Assume
negligible change in volume. (USEFUL INFORMATION: MM NaOH = 39.997 g mol-1)
(7) Calculate the pH of each of the following solutions:
(a) 0.1000M Propanoic acid( HC H O,,K=1.3x105)
(b) 0.1000M sodium propanoate (Na C HỎ)
(c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂
3 5
52
(d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above.
(e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.
Chapter 19 Solutions
General Chemistry - Standalone book (MindTap Course List)
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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