Question

Solve an equilibrium problem (using an ICE table) to calculate the pH of of each solution:

**Part A**

a solution that is 0.17 *M* in HCHO2 and 0.15 *M*
in NaCHO2

**Part B**

a solution that is 0.10 *M* in NH3 and 0.17 *M* in
NH4Cl

Answer #1

Use the Henderson-Hasselbalch equation to calculate the pH of
each solution:
Part A
a solution that is 0.17 M in HCHO2 and 0.15 M
in NaCHO2
Express your answer using two decimal places.
Part B
a solution that is 0.16 M in NH3 and 0.19 M in
NH4Cl
Express your answer using two decimal places.

Use the Henderson-Hasselbalch equation to calculate the pH of
each solution:
Part A a solution that is 0.20 M in HCHO2 and 0.15 M in
NaCHO2
Part B a solution that is 0.16 M in NH3 and 0.22 M in NH4Cl

Solve an equilibrium problem (using an ICE table) to calculate
the pH of each of the following solutions A) 0.14 M CH3NH2 B) 0.14
M CH3NH3Cl C) a mixture that is 0.14 M in CH3NH2 and 0.14 M in
CH3NH3Cl

Please use an ice table and lable which answer is Ka for NH4+
and pka NH4+
balanced, ionic equation for the reaction of ammonium ion [NH4+]
with water.
NH4+(aq) + H2O(l) ⇄ NH3(aq) + H3O+(aq)
equilibrium constant expression, Ka, for aqueous NH4+ Ka =
[NH3][H3O+]/[NH4+]
measured pH values for each solution (A-B) to calculate [H3O+]
.
Make an ICE table for each solution to find EQUILIBRIUM
concentrations.
Calculate Ka for NH4+ and pka NH4+
Solution A - pH = 4.56...

Calculate the concentration of Ag+ present in solution at
equilibrium when concentrated ammonia is added to a 0.013 M
solution of AgNO3 to give an equilibrium concentration of [NH3] =
0.17 M. The formation constant for Ag(NH3)2+ at this temperature is
1.7 × 107. How do you solve a problem like this? Thanks!

1.
The pH of a 0.25 M NH3 solution was measured to be 11.33. Calculate
the Keq for NH3.
2. An amount of 0.500 g of NH4Cl was added to 50.0 mL of the
solution in Problem 1 above. Use the Keq calculated from Problem 1
to calculate the pH of this solution.

What is the pH of a 0.15 M solution of HClO? Ka for
HClO = 3.5 x 10-8
The value of Ka for the weak acid Benzoic acid
(C6H6COOH) is 1.5 × 10-5. What are
the equilibrium concentrations of all species if 1.50 g of Benzoic
acid is dissolved in enough water to make a 250.0 mL solution? What
is the pH of the solution?
Ammonium ion is the conjugate acid of Ammonia. What
is the pH of a 0.25...

solution
[NH4+],
M
NH3], M
ΔpH on adding H+
pH on adding H+
Initial pH
pH on adding OH
ΔpH on adding OH-
a
0.10
0
2.43
2.13
4.56
9.07
4.51
b
1.0
0
2.12
2.09
4.21
8.37
4.16
c
0.050
0.050
1.14
8.38
9.52
10.06
0.54
d
0.50
0.50
0.17
9.52
9.69
9.73
0.04
e
0
0.10
0.78
9.62
10.4
11.39
0.99
pure water
2.39
2.26
4.65
12.06
7.41
Sorry I know that this is a lot but having...

Calculate the pH of a 1 L solution made by mixing 0.25mol of NH3
and 0.35mol NH4Cl. (Kb = 1.8x10^- 5). What is the new pH if 0.15
mol HCl is added to the solution?

For each of the following solutions, calculate the initial pH
and the final pH after adding 0.010 mol of NaOH .
Part B
250.0 mL of a buffer solution that is 0.200 M in HCHO2 and 0.305
M in KCHO2
Part C
250.0 mL of a buffer solution that is 0.265 M in CH3CH2NH2 and
0.245 M in CH3CH2NH3Cl
Express your answers using two decimal places separated by a
comma.

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