1) Generate a titration curve (pH vs. mL NaOH) for the titration
of 10 mL 0.15M HCl with 0.15M NaOH ( suggest 2mL intervals up to 16
mL).
Calculations:
mL NaOH
pH
0
2
4
6
8
10
12
14
16
2) Make another titration curve using acetic acid instead of HCl
(same concentration)
Consider the titration of of 5.00 mL of 0.450 M HBr using 0.120
M NaOH as the titrant.
a)Calculate the volume of 0.120 M NaOH that must be added in
order to reach the equivalence point.
b)Determine the pH of this titration solution at the equivalence
point.
c)Calculate the pH of this solution after 20.00 mL of 0.120 M
NaOH has been added.
Consider the titration of 100.0 mL of 0.100 M NaOH with
1.00 M HBr. Find the pH at the following volumes of acid
added.
Va = 0 mL
Va = 1.0 mL
Va = 5.0 mL
Va = 9.0 mL
Va = 9.9 mL
Va = 10.0 mL
Va = 10.1 mL
Va = 12.0 mL
Make a graph of pH versus Va = 0, 1.0, 5.0,
9.0, 9.9, 10.0, 10.1, and 12.0 mL.
1. In the titration of 25.00mL of 0.10M HCN using 0.10M NaOH as
the titrant, what is the pH after the addition of 12.50mL of
NaOH?
2. In the titration of 25.00mL of 0.10M HCN using 0.10M NaOH as
the titrant, what is the pH after the addition of 25.00mL of
NaOH?
3. What is the pH of 0.050M NaCN? Ka for HCN is 4.9x10-10.
consider the rotation of 50.0mL of a 0.2M HNO3 with
0.10M NaOH calculate the pH of the solution
a) before any extra NaOH has been add
b) after 50mL of NaOH
c) add 100mL of NaOH
d) add 150mL of NaOH
1. In the titration of a 25.00mL sample of 0.10M HAc
(Ka=1.75x10-5) using 0.10M NaOH as the titrant, what is the pH at
the following points during the titration?
a). After the addition of 25.00mL NaOH?
2. You want to prepare at least 1L of a NH3/NH4+ buffer with pH
= 9.65. You have available the following solutions, all 0.10M: NH3,
NaOH, NH4Cl, and HCl. For NH3, Kb= 1.8x10-5. Which solutions and
what volumes would you mix to prepare the...