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23 Nov 2019

Antacid 1

Antacid 2

Initial NaOH burette reading

3 ml

6 ml

Final NaOH burette reading

6 ml

41 ml

Total NaOH delivered

3 ml

35 ml

Moles of HCl _initial

0.01 M

0.01 M

Moles of HCl _{NaOH neutralized}

0.0006 M

0.007 M

Moles of HCl _{antacid neutralized}

0.0094 M

0.003 M

Moles of HCl _{antacid neutralized/dose}

0.019982 M

0.00686 M-- Mg (OH)₂

0.007692 M -- Al (OH)₃

Moles of HCl _{antacid neutralized/gram}

0.019982 M

0.0343 M -- Mg (OH)₂

0.03846 M -- Al (OH)₃

Total moles of HCl _{antacid neutralized/gram}

0.019982 M

0.07276 M

Which is the best antacid and why?

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Equipment Materials

50.00 ml buret, 250.ml volumetric flask, 1.00 ml volumetric pipet 10.0 mL volumetric pipet, 25.00 mL volumetric pipet, pipettor, 250 mL Erlenmeyer flask, 10.0 mL graduated cylinder, several beakers, several watchglasses, unkown bleach solution, 10% potassium iodide solution, 2M hydrochloric acid solution, 0.150 M sodium thiosulfate solution, 1% starch solution.

Background information regarding this experiment is as follows:

An aqueous solution of sodium hypochlorite (NaOCI) is a clear, slightly yellow liquid, and is commonly known as bleach. Aside from its uses as a bleaching agent, sodium hypochlorite solutions are also used as sterlizing agents and in water treatment. Industrial uses include agricultural, food handling, paper production, and textile production. Sodium hypochlorite is also added to waste water to reduce odors.

The concentration of sodium hypochlorite in bleach solutions can be determined by titration. Therefore, we must use a two-step method to titrate sodium hypochlorite. In the first step, sodium hypochlortie, hydrochloric acid, iodide ion, and starch are combined to form a starch-triiodide complex. In this step there are 3 reactions that take place:

The result of these 3 reactions is that when sodium hypochlorite is present the starch-triiodide complex is produced.

In the second step the starch-triiodide product is titrated by sodium thiosulfate to form a colorless solution of iodide, dithionate.

I do not know how to answer the following on the data sheet: (? means I do not know how to answer)

Table 1:

Mass of 1.00 ml of unknown (by tare): 10.552 g

Density of bleach: (g/ml) : 1.055 g/ml

Volume of diluted bleach used in each titration: 10.00

Concentration of sodium thiosulfate: ? (M)

Titration Data:

Initial buret reading (ml): trial1: 0.000 ml Trial 2: 0.00 ml Trial 3: 0.000ml

Final buret reading (ml): trial 1: 13.50ml Trial 2: 13.30ml Trial 3: 13.40ml

Volume delivered(ml: trial 1: ? Trial 2: ? trial 3:?

Calculations: (show clearly)

For trial 1,2,3 ???

1.Moles of Na₂S₂O₃ in titration: ??? trial 1,2,3

2.Moles of NaOCl: ???trial 1, 2,3

3.Average moles of diluted NaOCl: (one answer) ?

4.Average moles of undiluted NaOCl: (one answer.. mol) ?

5.Standard Deviation: (one answer) (mol)

6.Average mass of NaOCl in 25.00mL of undiluted bleach: ? (g)

7.mass of 25.00 mL of undiluted bleach: ? (g)

8. Mass % of NaOCL from experiment: ? (%)

9.Actual mass % of NaOCL (from prof; student does not make an entry):? (%)

More questions all need to be answered please:

1. Calculate the volume of the reagent thiosulafte solution which would be required if you titrated a 25ml sample of the original commercial bleach instead of 25ml of the diluted solution.

2. Why would we choose a graduated cylinder to measure the HCl and KI solutions instead of a volumetric pipette? When would we use a volumetric pippette?

3. You calculated the mass percent of sodium hypochlorite in the bleach( dilute and undiluted). Now calculate the molarity of the sodium hypochlorite in the diulte and undiluted solution/

4. Use oxidation states to show that equations (2) and (4) in the introduction are redox reactions and that equation 1 is not a redox reaction. :

-(1) NaOCl(aq) + HCl(aq) yields HOCl(aq)+NaCl(aq)

-(2) HOCL (aq) + HCl(aq) + 3I(aq) yields I3(aq) + 2CL(aq) + H₂O(l)

-(4) (I₃) (Starch) + 2S₂O₃ yields 3I + S₄O₆ + starch

5. combine equation 1-3 to show the overall reaction for the products of the starch-triiodide complex.

-(1) NaOCl(aq) + HCl(aq) yields HOCl(aq)+NaCl(aq)

-(2) HOCL (aq) + HCl(aq) + 3I(aq) yields I3(aq) + 2CL(aq) + H₂O(l)

-(3) I₃ + Starch yields (I₃) (Starch)

6. What standard was used in this experiment?

7. Describe the naming of NaClO and HClO. What are the names of the following compounds? NaClO₂ , NaClO_3, NaClO₄ , HClO₂, HClO₃, HClO₄

8 Submit a one paged (typed double spaced) report that discusses the following topics:

a. the goals or objectives of the experiment

b.your results as they relate to the goals and objectives

c. the quality of your results.

Balance the following Chemical Equations:

____Fe(s) + ____H₂O(g) Â® ____Fe₃O₄(s) + ____H₂(g)

____C₂H₆(g) + ____O₂(g) Â® ____CO₂(g) + ____H₂O(g)

___ C₆H₁₄ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (g)

___ C₃H₈O₃ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (l)

___ NaN₃ (s) Â® ___ Na (s) + ___ N₂ (g)

__ C₃H₅N₃O₉ Â® __ CO₂ + ___ N₂ + ___ H₂O + ___ O₂

Write and Balance the equations:

Aqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide.

Solid iron reacts with Oxygen gas to form solid Iron (II) oxide

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.)

(A) H₂O(g) + C(s) â¶ CO(g) +H₂(g)

(B) 2KClO₃(s) â¶ 2KCl(s) +3O₂(g)

(D) Pb(NO₃)₂(aq) + H₂SO₄(aq) â¶ PbSO₄(s) + 2HNO₃(aq)

4. Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

5. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(A) H₃PO₄

(B) Al(OH)₃

6. Complete and balance the following acid-base equations:

(A) A solution of HClO₄ is added to a solution of LiOH.

(B) Aqueous H₂SO₄ reacts with NaOH.

7. Write the molecular, total ionic, and net ionic equations for the following reactions:

(A) Ca(OH)₂(aq) + HC₂H₃O₂(aq) â¶

(B) H₃PO₄(aq) + CaCl₂(aq) â¶

8. Write the balanced equation, then calculate the number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl₂ and H₂. Ans: 1.67 g Mg

9. H₂ is produced by the reaction of 118.5 mL of a 0.8775-M solution of H₃PO₄ according to the following equation: 2Cr + 2H₃PO₄ â¶ 3H₂ + 2CrPO₄. How many grams of H₂ are produced? Ans: .315 g H₂

10. Automotive air bags inflate when a sample of sodium azide, NaN₃, is very rapidly decomposed.

2NaN₃(s) â¶ 2Na(s) + 3N₂(g)

What mass of sodium azide is required to produce 2.6 ft³ (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Ans: 142 g NaN₃

11. Urea, CO(NH₂)₂, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO₂ produced by combustion of 1.00 x 10⁴ grams of CO₂?

CO₂(g) + 2NH₃(g) â¶ CO(NH₂)₂(s) + H₂O(l)

Ans: 1360 g urea

12. What volume o f 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s) + H₂SO₄(l) â¶ HCl(g) + NaHSO₄(s)

Ans: .570 L

13. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction? CaCO₃(s)â¶CaO(s) + CO₂(s)

Ans: 92.0 %

14. Citric acid, C₆H₈O₇, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is

C₁₂H₂₂O₁₁ + H₂O +3O₂ â¶2C₆H₈O ₇+ 4H₂O

What mass of citric acid is produced from the reaction of 150. grams of sucrose if the yield is 92.30%?

Ans: 155 g

15. The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(A) What is the limiting reactant when 0.200 mol of P₄ and 0.200 mol of O₂ react according to P₄+5O₂ â¶ P₄O₁₀?

(B) Calculate the percent yield if 10.0 g of P₄O₁₀ is isolated from the reaction.

Ans: 88.0 %

16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li + N₂ â¶ Li₃N

Ans: Li

17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO₃ requires 20.22 mL of the AgNO₃ solution to reach the end point?

AgNO₃(aq) + NaCl(aq) â¶ AgCl(s) +NaNO (aq)

Ans: .3374 M

18. In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO₃)₂ solution.

2Cl^â(aq) + Hg(NO₃)₂(aq) â¶ 2NO₃^â(aq) + HgCl₂(s)

What is the Cl^â concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of .000825 M Hg(NO₃)₂(aq) to reach the end point?

Ans: 0.009636 M

Show transcribed image text 47 EXPERIMENT 47 Report Sheet 1. The kind of fruit drink appl Jwic 2. Molarity of iodine solution ad 3. Titration results Sample 1 (100 mL) Sample 2 (20.0 mL) Sample 3 (30.0 mL) a. Initial buret reading b. Final buret reading c. Total volume of iodine ,',ã¼, mL u. 2 mL 2.5 mL 4.amL 10.5 mL 10.5 mL 20.5 mL solution used: (b)-(a) 4. The weight of vitamin C in the fruit drink sample: [(3c) x 1.76 mg/mL] 5. Concentration of vitamin C in the fruit drink (mg/100 mL): [(4)/volume of drink] x 100 O,20,30 5S 6. Average concentration of vitamin Cin the fruit drink 52 mg/100 mL
Post-Lab Questions 1. Use the average concentration of vitamin C from your data, and calculate the volume that would satisfy your minimum daily requirement of vitamin C. Show your work 2. Vitamin C is ascorbie acid. If you examine the structure of ascorbic acid given in the Background t. In the structure shown, the ascorbic acid is section (equation 2), there is no -COOH grou - as a lactone or cyclic ester. Write the equation for the hydrolysis (cleavage by addition of water) of E ste the lactone to the carboxylic acid. 3. Write the net ionic equation for the conversion of iodine, la, to iodide, I. What kind of reaction is this? 4. Refer to the Background section and examine the chemical reaction for the oxidation of ascorbic acid (equation 2) a. What happened to the hydrogen atoms that were present in the ascorbic acid? b. Acid was added in the titration, but it is not present in equation (2) in a stoichiometric amount. So, what is the purpose of the acid? 5. The iodine for this experiment is in the form of 15, and not 12 (see equation (1), Background section]. Why is this form of iodine used? 577
ts for General Organic and Blochemistry Bettelheim/Landesberg Vitamin C is oxidized by 12 (as 15) according to the following chemical reaction: HO-CH- CH2OH HO-CH-CH,OH O. . o 2HI Ð½ Ð¾Ð½ Ð¾Ð½ Oxidized product (MW 174) (MW 254) Vitamin C (MW 176) As vitamin C is oxidized by iodine, I2 becomes reduced to I. When the end point is reached (no vitamin C is left), the excess of 12 will react with a starch indicator to form a starch-iodine complex, which is blackish-blue in color. I2 +starch iodine-starch complex (blackish-blue) It is worthwhile to know that although vitamin C is very stable when dry, it is readily oxidized by air (oxygen) when in solution; therefore, a solution of vitamin C should not be exposed to air for long periods. The amount of vitamin C can be calculated by using the following conversion factor 41 mL of 12 (0.01 M) = 1.76 mg vitamin C OBJECTIVE To determine the amount of vitamin C that is present in certain commercial food products by the titration method. Pro to this laboratory, there are techniques that you should revieo. You uoll find the relevant techmiques in the following experiments: (a) Use of the Spectroline pipet filler is in Experiment 2; (b) buret use and titration techniques are im Experiment 19.
terps Tile logical antioxidant (reducing agent). It helps to keep the iron in the yme, prolyl hydroxylase, in the reduced form and, thereby, it helps to to prevent scurvy is ascorbic acid. It is a powerful Acave ingredient in fruits and intain th thesis of normal ions and broken blood vessels. e enzyme activity. Prolyl hydroxylase is essential for the collagen. In scurvy, the abnormal collagen causes skin Vitamin C cannot be synthesized tained from the diet ( in the human body and must be e.g., citrus fruits, broccoli, turnip greens, sweet ppers, tomatoes) or by taking synthetic vitamin C (e.g, vitamin C blets, "high-C" drinks, and other vitamin C-fortified commercial foods). he minimum recommended adult daily requirement of vitamin C to y is 60 mg. Some people, among them the late Linus Pauling, wice Nobel Laureate, suggested that very large daily doses (250-10,000 ng) of vitamin C could help prevent the common cold, or at least lessen he symptoms for many individuals. No reliable medical data support this At present, the human quantitative requirement for vitamin C is still revent scurv claim. In this experiment, the amount of vitamin C is determined quantita- tively by titrating the test solution with a water-soluble form of iodine, I5: controversial and requires further research. [I: 1:1: -(triioode ion) (1) :11:+:1:-- Expanded octets 569

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	Antacid 1	Antacid 2
Initial NaOH burette reading	3 ml	6 ml
Final NaOH burette reading	6 ml	41 ml
Total NaOH delivered	3 ml	35 ml
Moles of HCl _initial	0.01 M	0.01 M
Moles of HCl _{NaOH neutralized}	0.0006 M	0.007 M
Moles of HCl _{antacid neutralized}	0.0094 M	0.003 M
Moles of HCl _{antacid neutralized/dose}	0.019982 M	0.00686 M-- Mg (OH)₂ 0.007692 M -- Al (OH)₃
Moles of HCl _{antacid neutralized/gram}	0.019982 M	0.0343 M -- Mg (OH)₂ 0.03846 M -- Al (OH)₃
Total moles of HCl _{antacid neutralized/gram}	0.019982 M	0.07276 M