First realize that this is a buffer solution problem. The common-ion effect dictates that the
LiNO2 will dissociate into Li and NO2 ions. The dissociated NO2\'s concentration will be part of
the solution you are trying to find the pH of.
The initial concentration of HNO2 is .150M, NO2 is .120M, and H is 0. Use the KA formula and
plug these values in accounting for change.
Equilibrium concentration of HNO2: (.150 -x)
Equilibrium concentration of NO2: (.120 + x)
Equilibrium concentration of H: (x)
Solve for x, and then take the -log of the concentration of H. This will be your pH.
Solution
First realize that this is a buffer solution problem. The common-ion effect dictates that the
LiNO2 will dissociate into Li and NO2 ions. The dissociated NO2\'s concentration will be part of
the solution you are trying to find the pH of.
The initial concentration of HNO2 is .150M, NO2 is .120M, and H is 0. Use the KA formula and
plug these values in accounting for change.
Equilibrium concentration of HNO2: (.150 -x)
Equilibrium concentration of NO2: (.120 + x)
Equilibrium concentration of H: (x)
Solve for x, and then take the -log of the concentration of H. This will be your pH..
First realize that this is a buffer solution problem. The common-ion.pdf
1. First realize that this is a buffer solution problem. The common-ion effect dictates that the
LiNO2 will dissociate into Li and NO2 ions. The dissociated NO2's concentration will be part of
the solution you are trying to find the pH of.
The initial concentration of HNO2 is .150M, NO2 is .120M, and H is 0. Use the KA formula and
plug these values in accounting for change.
Equilibrium concentration of HNO2: (.150 -x)
Equilibrium concentration of NO2: (.120 + x)
Equilibrium concentration of H: (x)
Solve for x, and then take the -log of the concentration of H. This will be your pH.
Solution
First realize that this is a buffer solution problem. The common-ion effect dictates that the
LiNO2 will dissociate into Li and NO2 ions. The dissociated NO2's concentration will be part of
the solution you are trying to find the pH of.
The initial concentration of HNO2 is .150M, NO2 is .120M, and H is 0. Use the KA formula and
plug these values in accounting for change.
Equilibrium concentration of HNO2: (.150 -x)
Equilibrium concentration of NO2: (.120 + x)
Equilibrium concentration of H: (x)
Solve for x, and then take the -log of the concentration of H. This will be your pH.
