Consider the titration of 25.0 mL of aqueous sample of
methamphetamine (C10H14NH) with 0.0955M HCl. It took 21.25 mL of
HCl to reach the equivalence point. Methamphetamine Kb = 1.0
x10^-10
a. Write the balanced net ionic equation for the titration
reaction (including states)
b. calcuate the molar concentration of methamphetamine in the
sample
c. calculate the initial pH of the methamphetamine sample
d. identify the predominant species that affects the pH at the
equivalence point and calculate its molarity...
25.0 mL of a 1.00 M Fe(No3)2 solution was reacted with 25.0 mL
of a 0.700M solution of K3PO4 to produce the solid Fe3(PO4)2 by the
balanced chemical equation
3 Fe(NO3)2(aq)+ 2 K3PO4(aq)--->Fe3(PO4)2(s)+ 6 KNO3(aq)
What is the limiting reagent?
How many grams of Fe(PO4)2 will be produced?
Consider the titration of a 25.0 −mL sample of 0.110 M HC2H3O2
with 0.125 M NaOH. Determine each of the following.(please do
all)
a)the initial pH
b)the volume of added base required to reach the equivalence
point
c)the pH at 6.00 mL of added base
d)the pH at one-half of the equivalence point ,andt he pH at the
equivalence point
Consider the titration of a 25.0 −mL sample of 0.110 M HC2H3O2
with 0.130 M NaOH.
Ka(H2C2H3O2) = 1.8x10-5
A) Initial PH
B) the volume of added base required to reach the
equivalence point
C) the pH at 4.00 mL of added base
D) the pH at one-half of the equivalence point
Consider the titration of a 25.0 ml sample of 0.175 M
CH3NH2 with 0.150 HBr. Determine each
quantity.
a) The volume of added acid required to reach the equivalence
point.
b) The ph at one-half the equivalence point.
c) The ph at the equivalent point.
d) The ph after adding 5.0 ml of acid beyond the equivalent
point.
Consider the titration of a 25.0 −mL sample of 0.100 M HC2H3O2
with 0.120 M NaOH. Determine each of the following.
the initial pH
Express your answer using two decimal places.
pH =
2.87
B)
Part B
the volume of added base required to reach the equivalence point
in mL?
Part C
the pH at 4.00 mL of added base
Express your answer using two decimal places.
Part D
the pH at one-half of the equivalence point
Express your answer...
mL HCl added
pH
0.00
11.86
25.0
10.71
50.0
6.09
A titration of 25.0 mL of 0.100 M triethylamine
((CH3CH2)3N) was performed with
0.0500 M HCl. Given the following data calculate the pKa for
triethylammonium ion.
Consider the titration of a 25.0 mL sample of 0.100 M CH3COOH (Ka=
1.8e-5) with 0.130 M NaOH. Determine the pH after adding 4.0 mL of
base beyond the equivalence point.
For the titration of 50.00 mL of
a 0.1000 M solution of compound H2SO4 with a
0.2000
M solution of compound NaOH in the following table.
For each titration, calculate the pH after the addition
of 0.00, 20.00, 25.00, 37.50,
50.00, and 60.00 mL of com-
pound NaOH.
Please explain all the steps.