Solve an equilibrium problem (using an ICE table) to calculate
the pH of each solution:
a solution that is 0.195 M in HC2H3O2 and 0.125 M in KC2H3O2
a solution that is 0.255 M in CH3NH2 and 0.135
M in CH3NH3Br
Solve an equilibrium problem (using an ICE table) to calculate
the pH of each solution:
Express your answer using two decimal
places
a) a solution that is 0.170 mol L−1 in
HC2H3O2 and 0.125 mol
L−1 in CH3COOK
b) a solution that is 0.205 mol L−1 in
CH3NH2 and 0.100 mol L−1 in
CH3NH3Br
Solve an equilibrium problem (using an ICE table) to calculate
the pH of each of the following solutions. (Ka(HF)=6.8×10^−4)
a) 0.15 M HF
b) 0.15 M NaF
c) a mixture that is 0.15 M in HF and 0.15 M in NaF
Solve an equilibrium problem (using an ICE table) to calculate
the pH of each of the following solutions.
0.16 M CH3NH3Cl
a mixture that is 0.16 M in CH3NH2
and 0.16 M in CH3NH3Cl
Solve an equilibrium problem (using an ICE table) to calculate
the pH of each of the following solutions.
a) 0.13 mol*L−1 CH3NH2
b) 0.13 mol*L−1 CH3NH3Cl
c)a mixture that is 0.13 molL−1 in CH3NH2
and 0.13 molL−1 in CH3NH3Cl
Solve an equilibrium problem (using an ICE table) to calculate
the pH of each of the following solutions.
1.0.17M CH3NH2
.17M CH3NH3Cl
a mixture that is 0.17M in CH3NH2
and 0.17M in CH3NH3Cl
Solve an equilibrium problem (using an ICE table) to calculate
the pH of each of the following solutions.
A. a mixture that is 0.15M in HF and 0.15M in NaF
B.0.15M NaF
C. 0.15M HF
Use the Henderson–Hasselbalch equation to calculate the pH of
each solution: Part A a solution that contains 0.625% C 5 H 5 N by
mass and 0.820% C 5 H 5 NHCl by mass Part B a solution that is 16.0
g of HF and 24.0 g of NaF in 125 mL of solution
Use the Henderson–Hasselbalch equation to calculate the pH of
each solution:
Part A
a solution that is 16.5 g of HF and 22.0 g of NaF in 125 mL of
solution
Part B
a solution that contains 1.23% C2H5NH2 by mass and 1.30%
C2H5NH3Br by mass
Part C
a solution that is 15.0 g of HC2H3O2 and 15.0 g of NaC2H3O2 in
150.0 mL of solution