Consider the titration of 25.00 mL of 0.0200 M MnSO4
with 0.0100 M EDTA at a...
Consider the titration of 25.00 mL of 0.0200 M MnSO4
with 0.0100 M EDTA at a pH of 8.00. Calculate the value of
pMn+2 after adding the following EDTA volumes:
Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121
M NaOH. Calculate the milliliters of base that must be added to
reach the first, second, and third equivalence points.
Ascorbic asic (0.0100 M) was added to 10.0 mL of 0.0200 M Fe3+
at pH = 0.30, and the potential was monitored with Pt and saturated
Ag/AgCl electrodes.
Dehydroascorbic acid + 2H+ + 2e- -->
ascorbic acid + H2O (Eo = 0.390 V)
Using Eo = 0.767 V for the
Fe3+/Fe2+ couple, calculate the cell voltage
when 5.0, 10.0, and 15.0 mL of ascorbic acid have been added.
Correct answers are: 0.570 V, 0.307 V, and 0.184 V but not...
Consider the titration of 50.0 mL of a 0.0200 M solution of
butanoic acid with 0.100 M NaOH. First, calculate the equivalence
point (Ve). Then, calculate the pH at the following points along
the titration curve. Assume fractions are exact numbers and ignore
activities for all calculations in this problem.
A) VNaOH= 0.000 mL
B) VNaOH= 1/2Ve
C) VNaOH= 4/5Ve
D) VNaOH= Ve
E) VNaOH= 3/2Ve
A 35 mL sample of water is triated with 0.0100 M EDTA. Exactly
9.70 mL of EDTA are required to reach the EBT endpoint. Calculate
the total hardness in ppm CaCO3.
Consider the titration of 20.00 ml of 0.0200 M sodium benzoate,
C6H5COO-Na+, with
0.0125 M HCl.
Write the chemical reaction occurring in this titration as a net
ionic equation.
Does the reaction go to completion? Show the relevant
calculation.
What is the equivalence point of this titration?
Calculate the pH of the initial point, before addition of HCl
(VHCl = 0.00 mL).
Calculate the pH after the addition of 10.00 mL of HCl
(VHCl = 10.00 mL).
Calculate the pH...
Calculate the pZn of a solution prepared by mixing 25.0 mL of
0.0100 M EDTA with 50.0 mL of 0.00500 M Zn2+. Assume
that both the Zn2+ and EDTA solutions are buffered with
0.100 M NH3 and 0.176 M NH4Cl.
Consider titration of 10.00 mL of 0.120 M Cu2+ solution with
0.100 M EDTA at pH 10.0. Find the concentration of free Cu2+ at the
equivalence point of this titration.
Consider the titration of 80.0 mL of 0.0200 M NH3 (a
weak base; Kb = 1.80e-05) with 0.100 M HBrO4.
Calculate the pH after the following volumes of titrant have been
added:
(a) 0.0 mL (d) 12.0 mL
(b) 4.0 mL (e) 16.0 mL
(c) 8.0 mL (f) 17.6 mL
Consider the titration of 80.0 mL of 0.0200 M C5H5N (a weak
base; Kb = 1.70e-09) with 0.100 M HNO3.
Calculate the pH after the following volumes of titrant have
been added:
(a) 0.0 mL pH =
(b) 4.0 mL pH =
(c) 8.0 mL pH =
(d) 12.0 mL pH =
(e) 16.0 mL pH =
(f) 25.6 mL pH =
PART TWO:
A buffer solution contains 0.14 mol of ascorbic acid
(HC6H7O6) and 0.84 mol of sodium
ascorbate...