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Chemistry on how to determine the mass of sodium ethanedioate

By nekonyan_sakura Oct 12, 2013 481 Words
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Name:
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Experiment 3

Topic:Volumetric analysis – Acid base and redox

Purpose:To determine the mass of sodium ethanedioate used to prepare a solution containing sodium ethanedioate and hydrated ethanedioic acid.

Materials:KA 1 is a solution containing hydrated ethanedioic acid, H2C2O4.2H2O, and sodium ethanediote.
KA 2 is a solution containing 3.5 g potassium manganate (VII) per dm3
KA 3 is a solution containing 1.7 g hydroxyl ions per dm3.
KA 4 is 1.0 mol dm-3 sulphuric acid
Phenolphthalein as indicator

Apparatus:Beaker
Filter funnel
Retort stand and clamp
White tile
250 cm³ conical flask
25.00 cm³ pipette
Pipette filler
Burette
Bunsen burner
Wire gauze
Thermometer
Tripod
Wash bottle with distilled water

Procedure:
a)

1. 25cm³ of KA1 is titrated into a titration flask and 3 drops of phenolphthalein is added into the titration flask. 2. The solution is titrated with KA3 which is filled in the burette. 3. Readings are recorded in the table.

Results:(b)Record your titration readings in the table below.

Titration number
Rough
Accurate

1
2
3
Final reading/cm³
-
17.40
17.30
17.20
Initial reading/cm³
-
0.00
0.00
0.00
Volume of KA 3/cm³
-
17.40
17.30
17.20

( i )25.0 cm³ of KA 1 required cm³ of KA 3 for a complete reaction.
( ii )calculate your average titre value showing the suitable titre values that you use.

Procedure:
c)

1. 25cm³ of KA 1 is pipette into a titration flask and 25cm³ of KA 4 is added into the solution. The solution is then heated until 60°c using a Bunsen burner the solution is then titrated with KA 2 until a slight pink colour is seen. 2. The titration was repeated a few times to get more accurate results.

Results:(d)Record your titration readings in the table below.

Titration number
Rough
Accurate

1
2
3
Final reading/cm³
-
31.40
30.40
28.70
Initial reading/cm³
-
0.00
0.00
0.00
Volume of KA 2/cm³
-
31.40
30.40
28.70

( i )25.0 cm³ of KA 1 required cm³ of KA 2 for a complete reaction.
( ii )calculate your average titre value showing the suitable titre values that you use.

Question:

(e) Calculate the concentration, in mol dm-3, of hydrated ethanedioic acid in solution KA 1.

Since H2C2O4  2H + C2O42-
The concentration is

(f) Calculate the mass of ethanedioate ions, , in 1 dm3 of KA 1.

Mr for

the mass of ethanedioic ions is

(g) Calculate the concentration, in mol dm-3, of ethanedioate ions which originated from the sodium enthaedioate salt.

From H2C2O4,
The concentration of H2C2O4

Total concentration
0.2157
X

(h) Calculate the mass of sodium ethanedioate present in 1 dm3 of solution KA 1.

Mass M
Sodium ethanedioate Na2C2O4

M of Na2C2O4

(i) Calculate the percentage of sodium ethanedioate in solution KA 1.

Percentage of Na2C2O4 =?

Mass of H2C2O4.2H2O

Percentage of Na2C2O4

(j) Why was solution KA 4 added to solution KA 1 before the titration?

H2SO4 act as catalysts that help to boast the rate of oxidation reaction of KMnO4.

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