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.
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.
(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.
(a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer.
What is the pH of the buffer after the addition of 0.030 mol HCl?
note: Ka (NH4+) = 5.6 x 10 -10
NH3 (aq) + H+ (aq) → NH4+ (aq)
(b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.
Chapter 19 Solutions
Student Solutions Manual for Ebbing/Gammon's General Chemistry, 11th
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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