How can we quantitatively determine the chloride content in an unknown soluble salt by gravimetric analysis?

Select one:

a. dissolve the unknown salt in water, precipitate the chloride ion as silver chloride, collect silver chloride and calculate the chloride content in the original salt by using stoichiometry;

b. dissolve the unknown salt in water, titrate the solution with silver nitrate and calculate the chloride content in the original salt based on the titration curve;

c. all options are incorrect;

d. dissolve the unknown salt in water, measure the absorbance of the solution and calculate the chloride content in the original salt based on the Beer-Lambert law;

e. add dilute nitric acid in the solution;

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Tod ThielLv2

31 Dec 2019

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Answer the following questions:

Method 1: Titration with Potassium Permanganate
5 H2O2 + 2 MnO4- + 6 H+ --> 8 H2O + 5 O2 + 2 Mn2+
Method 2: Catalytic Decomposition to Water and Oxygen
2 H2O2 --> 2 H2O + O2
Method 3: Oxidation of Iodide to Iodine; Spectroscopic measurement of TriIodide ion.
IO3- + 5 I- + 6 H+ --> 3 H2O + 3 I2 (standard)
H2O2 + 2 I- + 2 H+ --> 2 H2O + I2 (unknown)
I- + I2 --> I3-
Method 1:
You weigh out Potassium Permanganate,
Mass of KMnO4 (MW=158.034).......... 0.1736 g
You dissolve it completely in water.......... 46.00 mL
(a) Molarity of MnO4- solution........................... ________________ M
You pipet out your UNKNOWN............. 0.90 mL
You acidify and titrate it with your KMnO4 solution until the permanganate color persists.
Volume of permanganate solution.......... 11.39 mL
(b) Molarity of the HOOH in the UNKNOWN...................................._____________ M
Method 2:
You pipet your UNKNOWN into a reaction tube.... 4.40 mL
Add a "boat" containing Manganese Dioxide, MnO2
Set up the gas collection apparatus shown on the right.
You sink the boat and allow the oxygen generated to collect in the collection flask. The water temperature is................. 27 oC
The Barometric Pressure is............... 761.9 mm Hg
Weight of the collection Flask with remaining water.... 154.81 g.
Weight of collection flask filled with water........... 200.70 g.
DensityH2O ................................. 0.996 g/cc

(c) Partial Pressure of Oxygen collected................................. ____________ mm Hg
(d) Volume of oxygen collected ...................................... ____________ mL
(e) Millimoles of oxygen gas generated.................................. ____________ mmol
(f) Molarity of Hydrogen Peroxide in UNKNOWN.......................... ____________ M
Method 3:
STANDARD: Put into a clean 250 mL volumetric flask exactly ..... 1.00 ml
of 0.95 mM iodate STANDARD.
Add an excess of 1M KI and 1M Sulfuric Acid and let stand for 5 minutes. Dilute to volume.
UNKNOWN: Pipet into a clean 250 mL volumetric flask 1.00 mL of your UNKNOWN and dilute to volume with distilled water.
Put into a clean 250 mL volumetric flask exactly ........ 1.00 mL
of this diluted H2O2 UNKNOWN.Add an excess of 1M KI and 1M Sulfuric Acid and let stand for 5 minutes. Dilute to volume (250 mL). Measure STANDARD and UNKNOWN spectroscopically at 360 nm using the same cuvet throughout.
% Transmission of BLANK.................................. 98.1 %
% Transmission of STANDARD................................ 48.5 %
% Transmission of UNKNOWN................................. 34.7 %
(g) Absorbance of STANDARD.................................... ___________________
(h) Absorbance of UNKNOWN.................................... ___________________
(i) Molarity of original UNKNOWN................................. ___________________ M

i need help for questions H and I
the last answer was wrong. the J is right tho. thanks guys

2 Ag+ + Cu --> Cu+2 + 2 Ag
You individually weigh out a piece of Copper Wire and an empty Reaction Tube. You add a measured volume of silver nitrate solution of known concentration to the Reaction Tube and drop in the copper wire.
Weight of copper wire 1.3771 g
Weight of empty Reaction Tube 6.4591 g
Volume of AgNO3 solution used 3.65 mL
Molarity of original AgNO3 solution 0.1536 M
While the silver is being reduced, you make the following spectroscopic measurements. The blank is distilled water. The STANDARD is made by pipetting 1.00 ml of the original standard into a cuvet and adding exactly 5.00 mL of ammonia + distilled water to give a total volume in the cuvet of 6.00 mL.
%T of Blank 99.1 %
Concentration of original Cu Standard 0.0361 M
%T of Cu Standard in cuvet 39.0 %
After the reaction is complete, 2.35 ml of 14 M ammonia is added to the Reaction Tube to give a total of 6.00 mL of blue solution. 1.00 mL is pipetted into the cuvet and 5.00 mL of ammonia and distilled water were added. The %T of this mixed homogeneous solution was measured in the spectrometer.
The mass of the remaining copper wire was measured
The precipitated silver metal in the Reaction Tube was washed with distilled water and dried and the reaction tube with silver crystals was weighed.
%T of Cu ion in Reaction Tube 24.8 %
Mass of Cu Wire after reaction 1.3579 g
Mass of dried Reaction Tube with Silver metal after reaction 6.5240 g
Calculate:
a) Mass of Silver Metal produced ______________ mg
b) Millimoles of Ag + used up ______________ mmol
c) Atomic Weight of Silver based on silver used up ______________ g/mol
d) Mass of Copper Metal lost from wire ______________ mg
e) Atomic Weight of Silver based on copper metal lost ______________ g/mol
f) Absorbance of Cu +2 standard ______________
g) Absorbance of Cu+2 in Reaction Tube ______________
h) Molarity of Cu+2 in Reaction Tube ______________ M
i) Millimole of Cu+2 in Reaction Tube ______________ mmol
j) Atomic Weight of Silver based on Cu+2 produced ______________ g/mol

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