(Redox) Titration Problem
Testing for the concentration of ozone dissolved in water can be
accomplished by titrating a known volume of the solution to be
tested a with standardized potassium bromide solution. The reaction
that takes place forms oxygen gas and the bromate ion which can be
detected spectroscopically. In a particular experiment, a 25.00 mL
ozone containing solution was titrated with 37.41 mL of 0.3290 M
potassium bromide. Determine the concentration of ozone in the
original solution.
*Please show...
Redox titration of oxalate
1.00g of K3[Fe(C2O4)3] (Molar mass 437.25g/mol)
Mixed with 20ml .984M sulfuric acid.
TItrated with 13.4ml .028MKmNO4
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What is
Moles of KMnO4 reduced?
Moles of C2O42 oxidized?
Mass of C2O42 oxidized?
Actual weight % C2O42 in KTOF3
Theoritical weight % of C2O42 in KTOF3
%Error of weight % of C2O42 in KTOF3
A titration experiment is done with 1.37E-2 M
NaOH to determine the acid concentration in 0.631
L of an unknown acidic solution. It was found that to reach the
equivalence point 12.3 mL of strong base was
needed. What was the pH of the original acidic solution?
Imagine that you are attempting to determine the
concentration of an acid by titration with a solution of sodium
hydroxide with a known concentration, using phenolphthalein as an
indicator. For each of the following sources of error, indicate
whether the calculated concentration of acid would be too
high or too low.
i. An air bubble was present in the tip of the buret before
beginning the titration but was absent at the end of the
titration.
ii. You added too...
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design an experiment to determine the concentration of HbA1c in
the blood sample by following these six steps
Step 1, pick one differentiating characteristic
Step2 how will u probe that differentiating characteristic
Step3 tell the anticipated response to the probe
step4 measure the response to the probe
step 5 how will u interpret the response to the probe to obtain
the desired information
step6 tell the likely interference with the method you have
chosen.
you...
Goal #2: Determine the aqueous concentration of
IO3- in each sample by
titration.
Molarity
Formula
Name
Quantity
Determined in Part I
Na2S2O3(aq)
Sodium Thiosulfate
250 mL
KI(s)
Potassium Iodide
10 scoops using the spoon provided in your kit
1.0 M
HCl
Hydrochloric Acid
25 mL
0.20%
Starch Solution
10 mL
Fill the buret with the thiosulfate titrant. Drain some titrant
out until the level is a milliliter or so below 0.0 mL. Make sure
you don't have a bubble at...
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1157 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 14.02 mL of the standard solution. What...
A sample is analyzed to determine its iron content Fe2+ via a
redox titration with potassium chromate as the titrant. In the
titration Fe2+ is oxidized to Fe3+ and CrO4 2- is reduced to Cr 3+.
What is the percent by mass of iron in the sample if 0.9087g of the
sample required 45.68mL of a 0.04322 M K2CrO4 solution to reach the
endpoint?
I worked out the balanced equation to be:
8H+ + 3Fe2+ + CrO4 2- = 3Fe3+...
Cyanide recovered from the refining of gold ore
can be determined indirectly by EDTA titration. A known
excess of Ni2 is added to the cyanide to form
tetracyanonickelate(
II):
4CN + Ni ---> Ni(CN)4
When the excess Ni2 is titrated with standard EDTA,
Ni(CN)4 does not react. In a cyanide analysis, 12.7 mL of
cyanide solution were treated with 25.0 mL of standard
solution
containing excess Ni to form tetracyanonickelate. The excess
Ni required 10.1 mL of 0.013 0 M...