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Lab F: Standardization of a Sodium Thiosulfate Solution
Jayden Podmoroff 17122912
Partner: Josh Thomson
Lab performed: Nov 2, 2018
Chem 121 L08
TA: Nitin
Lab Submitted: Nov 16, 2018
1
Introduction:
The purpose of this experiment was to find the standardize a provided sodium thiosulphate
solution through titration using a dilute primary standard solution of potassium iodate. The
standardized solution obtained from this experiment can be used as a secondary standard
solution in future experiments.
A primary standard solution is defined by a solution having been prepared by direct
measurements of the mass of solute and the volume of solution, whereas a secondary standard
solution is defined by a solution whose concentration cannot be determined directly from
weight of solute and volume of solution.
1
Primary standard solutions are generally used to
standardize solutions, such as sodium thiosulphate, and secondary solutions are generally used
in more specific analytical experiments.
This experiment involves two separate chemical reactions leading up to and during titration.
Before titrating, a known quantity of iodine is produced from chemical reaction (1), where a
known amount of iodate reacts with excess iodide in acid solution.
1
The iodine is then titrated
with the sodium thiosulphate while using a starch indicator to mark the end point (reaction (2)).
The corresponding reactions are given below.
1
KIO
3
+ 5KI + 3H
2
SO
4
3I
2
+ 3K
2
SO
4
+ 3H
2
O
(1)
2Na
2
S
2
O
3
+ I
2
2NaI + Na
2
S
4
O
6
(2)
2
Procedure:
The procedure of Lab F given by the First Year Chemistry Lab Manual
2
was followed as described
below.
In order to make the concentrated KIO
3
primary standard solution, 1.0126 g of potassium
iodate was weighed using an analytical balance and then transferred into a 150 mL beaker. The
potassium iodate was dissolved in the beaker and then transferred into a 250 mL volumetric
flask and then inverted about 15 times to ensure proper mixture.
The dilute KIO
3
primary standard solution was made by first pipetting 25.00 mL of the
concentrated KIO
3
solution from a separate dry beaker into a 250 mL volumetric flask. The flask
was then filled with deionized water up to the mark in order to dilute the solution and then
inverted about 15 times to ensure proper mixture.
Roughly 100 mL of the provided sodium thiosulphate solution was obtained in a beaker and
used to fill a burette. 25.00 mL of the dilute KIO
3
standard solution was pipetted into a 125 mL
Erlenmeyer flask. 0.2 g of potassium iodate was obtained using a scoop and mixed with the
solution in the flask. 20 drops of 1 M H
2
SO
4
were then added to the solution under the fume
hood, forming a brownish-yellow iodine solution.
The solution obtained from the previous step was slowly titrated with the provided sodium
thiosulphate solution until the iodine solution was a much lighter yellow. 5 drops of starch
3
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Related Questions
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Trial 3
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Which is more basic - an aqueous solution of borax or an equivalent concentration aqueous solution of lime water?
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1 (1x10)
0.0
14.0
1x10-14
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1x10-1
1.0
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1x10 13
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1x10-2
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1x10-3
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8.0
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7.0
1×10-7
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5.0
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4.0
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1 (1x10)
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7. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record.
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After 45 µl of 5 | After 205 µl more
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Original
After 205 µl more
After 45 µl more
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M NaOH
of 5M NaOH
of 5 M NaOH
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11.29
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Hd
A: initial
Vertical (Value) Axis Title
0
B: half equivalence
C: equivalence
5
10
15
20
Titrant: mL of 0.100 M HCI added
25
20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl.
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O Macmillan Learning
Na₂CO3 is used to standardize a solution of HC1. What is the
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Next, 0.4242 g of an unknown sample containing Na2CO3
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left.
9.0x10-2 M Cala; K2SO4
Express your answer using two significant figures.
[K₂SO4]=
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ΜΕ ΑΣΦ
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M
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Calculate [H3O*], [HSO3], and [SO32-] in the solution:
Ka1 1.0 x 10-2, Ka2 = 6.0 x 10-8
1
C
e
+
H₂SO₂H₂O + HSO₂"
HS03
0.10 M
0.10M-X
O
+X
X
2
(H₂0°) (HSO₂) _x²
(H₂SO₂)
(0.10-x)
Val
=1₁0×10²² = x ²
(0.10) 0.40
10.01=1x²
0.032= X
Assume x <<<0110-x
0.10- 20.10
(040)
Validity = 0.032x100,
0.10
= 0.32% <5%
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Following the monograph procedure, a 724-mg of aspirin (MW+180 g/mol) dissolved in 18.5 ml of cold neutralized alcohol. This solution was then initially titrated with 0.101 N sodium hydroxide solution, then later neutralized with 0.104 sulfuric acid.
1. What is the milliequivalent weight consumed by the acidic titrant?
a. 1.5392 g-meq
b. 2.0907 g-meq
c. 1.4948 g-meq
d. 2.1528 g-meq
2. What is the milliequivalent weight consumed by the basic titrant?
a. 5.8656 g-meq
b. 1.5392 g-meq
c. 5.6964 g-meq
d. 1.4948 g-meq
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a. -4.1572 g-meq
b. 4.3708 g-meq
c. 0.5515 g-meq
d. 4.1572 g-meq
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- Following the monograph procedure, a 724-mg of aspirin (MW=180 g/mol) dissolved in 18.5 ml of cold neutralized alcohol. This solution was then initially titrated with 0.101 N sodium hydroxide solution, then later neutralized with 0.104 sulfuric acid. 1. What is the total volume (mL) of excess titrant used in the titration? a. 56.400 mL b. 52.000 mL c. 44.600 mL 2. What is the milliequivalent weight consumed by the acidic titrant? a. 1.5392 g-meq b. 2.0907 g-meq c. 1.4948 g-meq d. 2.1528 g-meq 3. What is the milliequivalent weight consumed by the basic titrant? a. 5.8656 g-meq b. 1.5392 g-meq c. 5.6964 g-meq d. 1.4948 g-meq 4. What is the difference of milliequivalent weight consumed in the reaction? a. -4.1572 g-meq b. 4.3708 g-meq c. 0.5515 g-meq d. 4.1572 g-meq 5. What is the percentage purity of the sample? 6. What is the titer value (mg) based from the specific type of titration?arrow_forward1. A 0.1250-g sample of pure (100%) of K2Cr2O7 was dissolve in 250-mL volumetric flask, and dilute to volume, producing a concentration of 1.700 × 10-3 M. The resulting solution is an example of a standard solution prepared from a primary standard. Select one: a. True b. False 2. Which of the following is not an example of a standard solution? a. 1000 ppm Lead Nitrate solution b. 1.000g pure sodium carbonate dissolved in 1L of solution c. 3:4 nitric acid: hydrochloric acid solution d. NaOH solution standardized using KHP e. 0.104 M NaOHarrow_forwardData for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…arrow_forward
- M 23 (H) Inorganic Analytical Chemistry pard My courses CHEM 23 (H) FS-AY:20-21 Week 4-5: Quantitative Analysis by Gravimetry and Titration Quiz 4 Qu 10 The 500.0-mg sample of impure Na2 CO3 (FM: 105.96) required 22.00 mL of the HCI standard solution (the obtained concentration of HCI from the previous question, problem 5: Titrimetry short answer type) for complete neutralization. ut of 1. Give the balanced chemical equation between the sample, Na2CO3 and the standard, HCI. 2. What is the mass (g) of Na, CO3 in the sample? 3. Calculate the % (w/w) purity of a 500.0-mg sample of impure Na2 CO3 Note: Type your solution here or upload its pic in Jpeg or pdf format. Another option is to send it to me via email (subject: Fam name-Quiz 4) or messenger, privately. Do not forget to box the final answer and write your name. В I 1.arrow_forwardFollowing the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. Consider that the burette was completely filled to the 0 mL mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 21.2 mL C. 21.3 mL D. 22.7 mL 2. What is the unknown weight (grams) in the problem? Your Answer:arrow_forwardChemistry H,N. CH, H,N. HO, но Phenylalanine (1) Tyrosine (2) H,C HN CH, H,C `CH, H,C но Triethylamine (4) N-acetyl-OMe-Tyrosine (3) All four compounds are dissolved in ethyl acetate. If you started by extracting the solution with 1 M HCI, which of the following compounds would end up in the aqueous layer? 4 12 Instead, you decide to start by extracting the ethyl acetate solution with 5% NaHCO3 (sodium bicarbonate). What will remain in the organic layer? 1 2 4arrow_forward
- Only typde Solution.arrow_forwardAnswer the following: Maria was given a capsule of multivitamins and she was asked to determine the % by mass (w/w) of ascorbic acid present in the sample. The student analyzed 1.032 g sample using volumetric titration. Use the table as a reference of the data to be used for your solution. Given Choices: A. 66.0 % B. 54.6% C. 65.6% D. 7.30%arrow_forwardPreparation and Standardization of KMnO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 Weight of sodium oxalate (Na2C2O4, MM= 134 g/mol) Titration data 0.2050 g Final reading Initial reading 29.86 mL 0.00 mL 30.66 mL 30.52 mL 0.00 mL 0.00 mL Total vol. of KMNO4 used Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:arrow_forward
- Sample A B C D Identity Rationalizationarrow_forwardA. Calculate the solubility of PbI2 (Ksp = 1.5 x 10-8) in moles per liter. Ignore any acid–base properties. B. Calculate the solubility of CdCO3 (Ksp = 5.1 x 10-12) in moles per liter. Ignore any acid–base properties. C. Calculate the solubility of Sr3(PO4)2 (Ksp = 1.5 x 10-31) in moles per liter. Ignore any acid–base properties.arrow_forward9. wo samples of the same soil is subjected to pH analysis using a pH meter, the first is analysed using 1:1 soil:water ratio and the other with 1:1 soil:KCl ratio, what would be the most probable result? A. Soil analused using 1:1 soil:KCl ratio will register a higher pH compared to that of soil analysed using 1:1 soil water ratio B. Soil analysed using 1:1 soil:KCl will register a lower pH compared to that of soil analysed using 1:1 soil:water ratio C. Soil analysed using 1:1 soil:water ratio will register a lower pH compared to that of soil analysed using 1:1 soil:KCl ratio D. Soil analysed using 1:1 soil:water ratio will have the same pH with that of soil analysed using 1:1 soil:KCl ratioarrow_forward
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