timothystark

How to reduce inflation rate in country?

Consider a sample of 47 football games, where 30 of them were won by the home team. Use a 0.01 significance level to test the claim that the probability that the home team wins is greater than one-half.

 

 

 

 

Name this reaction type, CO2 + H2O --> H2CO3

    Question 14 options:

Decomposition

Single Replacement

Combustion

Synthesis

What is the overall order or a reaction between sodium hydroxide and phenolphthalein?

A thymine nucleotide is replaced by a guanine after an error happens during the copying of some DNA. When it comes to the site where this replacement takes place on the double helix, what kind of an impact would this have on the double helix and why are you anticipating that kind of change?

Water dripping out of a hole in a cup would be what kind of change in energy?

please help with work shown so I can understand how the answers were found.

A student weighs an empty flask and stopper and finds the mass to be 55.844 g. She then adds about 5 mL of an unknown liquid and heats the flask in a boiling water bath at 99.7 degrees C. After all the liquid is vaporized, she removes the flask from the bath, stoppers it, and lets it i s cool. After it is cool, she momentarily removes the stopper, then replaces it and weighs the flask and condensed vapor, obtaining a mass of 56.101 g. The volume of the flask is known to be 248.1 mL. The barometric pressure in the laboratory 752 mm. Hg. a. What was the pressure of the vapor in the flask atm? P = ______ amtb. What was the temperature of the vapor in K? the volume of the flask in liters? T =______K, V=______ Lc. What was the mass of vapor that was present in the flask? g = ___________gramsd. How many moles of vapor are present? n =___________gramse. What is the mass of one mole of vapor? MM=___________g/mole

a student ways an empty flask and stopper in find the mass to be 54.868g. she then adds about 5 ml of unknown liquid and heats the flask in a boiling water bath 100°C. after all the liquid is vaporized she removes the flask from the bath, stoppers it, and let's it cool. after it is cool she momentarily removes the stopper, than replaces it and weighs the flask and condensed vapor, obtaining a mass of 55.496g. the volume of the flask is known to be 235.7mL. the barometric pressure in the laboratory that is 738mmhg.

a. what was the pressure of the vapor in the flask in atm?

b. what was the temperature of the vapor in K?

c. what was the mass of vapor that was present in the flask

D. how many moles of vapor are present?

e. what is the mass of one mole of vapor?

Three students measured an empty Erlenmeyer flask and a tight-fitting stopper and found the mass to be 62.371 g. The students then carefully measured out 4.4 ml of a volatile liquid, poured the liquid into the flask, and heated the flask containing the liquid in a 101.1 degree C boiling water bath. As soon as all the liquid had vaporized, the students covered the flask with the stopper and set it aside to cool. Then, after a few minutes, they very quickly removed and replaced the stopper and reweighed the flask. The mass of the flask, stopper, and condensed vapor was 63.088 g. At the conclusion of the experiment, the students rinsed out the flask, filled it with water to the top, replaced the tight-fitting stopper (being sure there were no air bubbles), and obtained a volume of 261.9 ml. The barometric air pressure that day was 733 mm Hg. What is the pressure of the vapor inside the flask (in atmospheres) after the vapor had cooled and the students opened the flask momentarily?

Procedures: 1. Obtain a thermometer and place it on the bench at your work area. Be careful it does not roll off the bench. 2. Weigh an empty Erlenmeyer flask with a rubber stopper firmly capping it. Record the mass. 3. Place a small piece of solid CO2 (dry ice) in the flask (use about twice the amount you calculated in pre-lab question c). Place the stopper loosely on top of the flask. Watch the flask while the CO2 sublimes. Firmly stopper the flask immediately after all the solid CO2 disappears. 4. Wait until the flask is equilibrated to room temperature (around 5-10 minutes), and then “burp” it by lifting one side of the stopper, and then quickly pushing it back in. This is to ensure that the pressure is the same inside and outside the flask. 5. Dry off any accumulated moisture from the outside of the flask, weigh the stoppered flask (on the same scale) and record the mass. 6. To determine the volume of the flask: fill the flask all the way to the brim with water and stopper it while holding it over a sink. If there is any air trapped inside, try again until only water is present inside the stoppered flask. The volume of the water should be the same as the volume of the air in the stoppered flask. Dry off the outside of the flask completely. Measure the volume of water in a graduated cylinder in batches and add up the volumes to get the total volume of all the water in the flask. Record this as the stoppered flask volume. 7. Read the thermometer in your work area and record the temperature. 8. Read the barometer in the lab and record the pressure in mmHg. Ask me if you need help with the barometer. Don’t forget to correct the barometer reading for room temperature using the table hanging on the wall. Q: Why do we measure the volume of the flask with water rather than using the volume listed on the side?

Procedures: 1. Obtain a thermometer and place it on the bench at your work area. Be careful it does not roll off the bench. 2. Weigh an empty Erlenmeyer flask with a rubber stopper firmly capping it. Record the mass. 3. Place a small piece of solid CO2 (dry ice) in the flask (use about twice the amount you calculated in pre-lab question c). Place the stopper loosely on top of the flask. Watch the flask while the CO2 sublimes. Firmly stopper the flask immediately after all the solid CO2 disappears. 4. Wait until the flask is equilibrated to room temperature (around 5-10 minutes), and then “burp” it by lifting one side of the stopper, and then quickly pushing it back in. This is to ensure that the pressure is the same inside and outside the flask. 5. Dry off any accumulated moisture from the outside of the flask, weigh the stoppered flask (on the same scale) and record the mass. 6. To determine the volume of the flask: fill the flask all the way to the brim with water and stopper it while holding it over a sink. If there is any air trapped inside, try again until only water is present inside the stoppered flask. The volume of the water should be the same as the volume of the air in the stoppered flask. Dry off the outside of the flask completely. Measure the volume of water in a graduated cylinder in batches and add up the volumes to get the total volume of all the water in the flask. Record this as the stoppered flask volume. 7. Read the thermometer in your work area and record the temperature. 8. Read the barometer in the lab and record the pressure in mmHg. Ask me if you need help with the barometer. Don’t forget to correct the barometer reading for room temperature using the table hanging on the wall. Q: Why is the flask not firmly stoppered during sublimation?

I have an experiment to measure the molar mass of CO2.

Procedures:

1. Obtain a thermometer and place it on the bench at your work area. Be careful it does not roll off the bench.

2. Weigh an empty Erlenmeyer flask with a rubber stopper firmly capping it. Record the mass.

3. Place a small piece of solid CO2 (dry ice) in the flask (use about twice the amount you calculated in pre-lab question c). Place the stopper loosely on top of the flask. Watch the flask while the CO2 sublimes. Firmly stopper the flask immediately after all the solid CO2 disappears.

4. Wait until the flask is equilibrated to room temperature (around 5-10 minutes), and then “burp” it by lifting one side of the stopper, and then quickly pushing it back in. This is to ensure that the pressure is the same inside and outside the flask.

5. Dry off any accumulated moisture from the outside of the flask, weigh the stoppered flask (on the same scale) and record the mass.

6. To determine the volume of the flask: fill the flask all the way to the brim with water and stopper it while holding it over a sink. If there is any air trapped inside, try again until only water is present inside the stoppered flask. The volume of the water should be the same as the volume of the air in the stoppered flask. Dry off the outside of the flask completely. Measure the volume of water in a graduated cylinder in batches and add up the volumes to get the total volume of all the water in the flask. Record this as the stoppered flask volume.

7. Read the thermometer in your work area and record the temperature.

8. Read the barometer in the lab and record the pressure in mmHg. Ask me if you need help with the barometer. Don’t forget to correct the barometer reading for room temperature using the table hanging on the wall.

--

And here are the questions:

1. Why was excess dry ice used in step 3 of the procedure?

2. Why do gas laws use degrees Kelvin rather than degrees Celsius?

3. Were you surprised at how accurately the mass of a molecule of CO2 could be determined with such simple equipment? Explain why or why not?

4. If you didn’t wipe away any frost or condensation formed during sublimation, how would your molar mass value be affected? Be specific please.

5. Why do we measure the volume of the flask with water rather than using the volume listed on the side?

6. Why is the flask not firmly stoppered during sublimation?

Mass of empty stoppered flask 154.685

mass of flask, stopper and CO2 154.795

stoppered flask volume 271

temperature 295.15 K

atmospheric pressure 772

Post Lab Questions:

Why was excess dry ice used in step 3 of the procedure?

Why do gas laws use degrees Kelvin rather than degrees Celsius?

Were you surprised at how accurately the mass of a molecule of CO₂ could be determined with such simple equipment? Explain why or why not?

If you didn’t wipe away any frost or condensation formed during sublimation, how would your molar mass value be affected? Be specific please.

Procedures:

1. Obtain a thermometer and place it on the bench at your work area. Be careful it does not roll off the bench.

2. Weigh an empty Erlenmeyer flask with a rubber stopper firmly capping it. Record the mass.

3. Place a small piece of solid CO₂ (dry ice) in the flask (use about twice the amount you calculated in pre-lab question c). Place the stopper loosely on top of the flask. Watch the flask while the CO₂ sublimes. Firmly stopper the flask immediately after all the solid CO₂ disappears.

4. Wait until the flask is equilibrated to room temperature (around 5-10 minutes), and then “burp” it by lifting one side of the stopper, and then quickly pushing it back in. This is to ensure that the pressure is the same inside and outside the flask.

5. Dry off any accumulated moisture from the outside of the flask, weigh the stoppered flask (on the same scale) and record the mass.

6. To determine the volume of the flask: fill the flask all the way to the brim with water and stopper it while holding it over a sink. If there is any air trapped inside, try again until only water is present inside the stoppered flask. The volume of the water should be the same as the volume of the air in the stoppered flask. Dry off the outside of the flask completely. Measure the volume of water in a graduated cylinder in batches and add up the volumes to get the total volume of all the water in the flask. Record this as the stoppered flask volume.

7. Read the thermometer in your work area and record the temperature.

8. Read the barometer in the lab and record the pressure in mmHg. Ask me if you need help with the barometer. Don’t forget to correct the barometer reading for room temperature using the table hanging on the wall.

Problem broken down into 4 individual questions.

Part 1: https://www.chegg.com/homework-help/questions-and-answers/problem-broken-4-individual-questions-part-1-4-supply-calculated-molarities-indicated-spec-q9055855

Part 2: https://www.chegg.com/homework-help/questions-and-answers/problem-broken-4-individual-questions-part-1-https-wwwcheggcom-homework-help-questions-ans-q9056129

Part 3 of 4:

Supply the calculated molarities of the indicated species in the solution mixtures.Assume the solutions are at 25 degrees Celsius.

Problem #C3: Calculate the Molarity for: H⁺(at equilibrium).

Given the following procedure (straight from lab book).

C3. pH of Deionized water: Obtain 19 mL of deionized water in each of two beakers. Read the pH of the deionized water. (NOTE: It will not be a pH of 7.00.)

Problem broken down into 4 individual questions.

Part 1: https://www.chegg.com/homework-help/questions-and-answers/problem-broken-4-individual-questions-part-1-4-supply-calculated-molarities-indicated-spec-q9055855

Part 2 of 4:

Supply the calculated molarities of the indicated species in the solution mixtures.Assume the solutions are at 25 degrees Celsius.

Problem #C2

A) Calculate the Molarities for: HC₂H₃O₂ (two molarities to calculate; once after dilution but before reaction and at equilibrium) , C₂H₃O₂^- (two molarities to calculate; once after dilution but before reaction and at equilibrium), H⁺ (at equilibrium), HCl (after dilution but before reaction)

B) Calculate the Molarities for: HC₂H₃O₂ (two molarities to calculate; once after dilution but before reaction and at equilibrium) , C₂H₃O₂^- (two molarities to calculate; once after dilution but before reaction and at equilibrium), H⁺ (at equilibrium), NaOH (after dilution but before reaction)

Given the following procedure (straight from lab book).

C2. Addition of Acid or Base to Buffer:

a. To the buffer in beaker "A", add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture.

b. To the buffer in beaker "B,", add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

In the unshaded portions of the following table, supply the calculated molarities of the indicated species in the solution mixtures. Assume the solutions are at 25 degrees Celsius. Note that in the rows labeled "Before Reaction," you must supply the appropriate concentrations after dilution occurs in the reaction mixture, but before any reaction takes place. C. pH of Buffer Solutions: 1. Preparation of Buffer Solution: Weigh 3.3 g of solid sodium acetate trihydrate, NaC2H3O2 * H2O, into a clean 150 or 250 mL beaker. Using graduated cylinders, add 46 mL of deionized water and 4.0 mL of 6.0 M HC2H3O2. Mix thoroughly. Measure 19.0 mL of this into each of two clean beakers. Label as "A" and "B". Measure the pH of this buffer solution using the remaining 10 mL. 2. Addition of Acid or Base to Buffer: a. To the buffer in beaker "A", add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture. b. To the buffer in beaker "B,", add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture. 3. pH of Deionized water: Obtain 19 mL of deionized water in each of two beakers. Read the pH of the deionized water. (NOTE: It will not be a pH of 7.00.) 4. Addition of Acid or Base to Deionized Water: a. To one beaker of deionized water, add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture. b. To the second beaker of deionized water, add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

I need C.2b, C.3, C.4a and C.4b-- PLEASE HELP!

In the unshaded portions of the following table, supply the calculated molarities of the indicated species in the solution mixtures. Assume the solutions are at 25 degrees Celsius. Note that in the rows labeled "Before Reaction," you must supply the appropriate concentrations after dilution occurs in the reaction mixture, but before any reaction takes place.

C. pH of Buffer Solutions:
Preparation of Buffer Solution: Weigh 3.3 g of solid sodium acetate trihydrate, NaC2H3O2 * H2O, into a clean 150 or 250 mL beaker. Using graduated cylinders, add 46 mL of deionized water and 4.0 mL of 6.0 M HC2H3O2. Mix thoroughly. Measure 19.0 mL of this into each of two clean beakers. Label as "A" and "B". Measure the pH of this buffer solution using the remaining 10 mL.

Addition of Acid or Base to Buffer:

a. To the buffer in beaker "A", add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture.

b. To the buffer in beaker "B,", add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

pH of Deionized water: Obtain 19 mL of deionized water in each of two beakers. Read the pH of the deionized water. (NOTE: It will not be a pH of 7.00.)

Addition of Acid or Base to Deionized Water:

a. To one beaker of deionized water, add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture.

b. To the second beaker of deionized water, add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

Problem broken down into 4 individual questions.

Part 1 of 4:

Supply the calculated molarities of the indicated species in the solution mixtures.Assume the solutions are at 25 degrees Celsius.

Problem #C1: Calculate the Molarities for: HC₂H₃O₂ , C₂H₃O₂^-, H⁺

Given the following procedure (straight from lab book).

C. pH of Buffer Solutions:
1. Preparation of Buffer Solution: Weigh 3.3 g of solid sodium acetate trihydrate, NaC₂H₃O₂ * 3H₂O, into a clean 150 or 250 mL beaker. Using graduated cylinders, add 46 mL of deionized water and 4.0 mL of 6.0 M HC2H3O2. Mix thoroughly. Measure 19.0 mL of this into each of two clean beakers. Label as "A" and "B". Measure the pH of this buffer solution using the remaining 10 mL.

Directions (taken straight from lab manual):

C. pH of Buffer Solutions:
1. Preparation of Buffer Solution: Weigh 3.3 g of solid sodium acetate trihydrate, NaC2H3O2 * H2O, into a clean 150 or 250 mL beaker. Using graduated cylinders, add 46 mL of deionized water and 4.0 mL of 6.0 M HC2H3O2. Mix thoroughly. Measure 19.0 mL of this into each of two clean beakers. Label as "A" and "B". Measure the pH of this buffer solution using the remaining 10 mL.

2. Addition of Acid or Base to Buffer:

a. To the buffer in beaker "A", add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture.

b. To the buffer in beaker "B,", add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

3. pH of Deionized water: Obtain 19 mL of deionized water in each of two beakers. Read the pH of the deionized water. (NOTE: It will not be a pH of 7.00.)

4. Addition of Acid or Base to Deionized Water:

a. To one beaker of deionized water, add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture.

b. To the second beaker of deionized water, add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

Task:

1. Calculate the pH for each.

2. Compare and explain the difference in pH change occurring for the buffer system and for the water on the addition of HCl.

Problem #C4:

A) Calculate the Molarity for: H⁺(at equilibrium) and HCl (after dilution occurs but before the reaction occurs).

B) Calculate the Molarity for: H⁺(at equilibrium) and NaOH (after dilution occurs but before the reaction occurs).

C. pH of Buffer Solutions:

1. Preparation of Buffer Solution: Weigh 3.3 g of solid sodium acetate trihydrate, NaC2H3O2 * H2O, into a clean 150 or 250 mL beaker. Using graduated cylinders, add 46 mL of deionized water and 4.0 mL of 6.0 M HC2H3O2. Mix thoroughly. Measure 19.0 mL of this into each of two clean beakers. Label as "A" and "B". Measure the pH of this buffer solution using the remaining 10 mL.

2. Addition of Acid or Base to Buffer: a. To the buffer in beaker "A", add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture. b. To the buffer in beaker "B,", add 1.0 mL of

3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture. 3. pH of Deionized water: Obtain 19 mL of deionized water in each of two beakers. Read the pH of the deionized water. (NOTE: It will not be a pH of 7.00.)

4. Addition of Acid or Base to Deionized Water: a. To one beaker of deionized water, add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture. b. To the second beaker of deionized water, add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

Given four beakers labeled A, B, C, and D.

Add 40 mL of distilled water to beakers A and C.

Add 40 mL of the prepared sodium acetate/acetic acid buffer solution to both beakers B and D.

Pipette 1.0 mL of 6 M HCl, hydrochloric acid solution into beakers A and B.

Pipette 1.0 mL of 6 M NaOH, sodium hydroxide solution into beakers C and D.

If the concentration of CH3CO2Na after dilution is 0.62M and the concentration of CH3CO2H after dilution is 0.51M

Calculated pH of beaker A and B after the addition of 6 M HCl.(Ka of CH3CO2H=1.32x10^-4)

1. Label four clean 100 and/or 150 mL beakers: A, B, C, and D.

2. Add 40 mL of distilled water to beakers A and C. Be sure that the graduated cylinder is well rinsed before using it.

3. Use a graduated cylinder to add 40 mL of the prepared sodium acetate/acetic acid buffer solution to both beakers B and D.

4. Record the initial pH of each the solutions A-D. Make sure to rinse the pH electrode with distilled water between readings.

5. Pipette 1.0 mL of 6 M HCl, hydrochloric acid solution into beakers A and B. Thoroughly mix the solutions.

6. Pipette 1.0 mL of 6 M NaOH, sodium hydroxide solution into beakers C and D. Thoroughly mix the solutions

What is the volume of 6HCl used for addition into beaker A,B,C,D and how do you calculate the ph of each beaker after the addition of 6M HCL

1. Label four clean 100 and/or 150 mL beakers: A, B, C, and D.

2. Add 40 mL of distilled water to beakers A and C. Be sure that the graduated cylinder is well rinsed before using it.

3. Use a graduated cylinder to add 40 mL of the prepared sodium acetate/acetic acid buffer solution to both beakers B and D.

4. Record the initial pH of each the solutions A-D. Make sure to rinse the pH electrode with distilled water between readings.

5. Pipette 1.0 mL of 6 M HCl, hydrochloric acid solution into beakers A and B. Thoroughly mix the solutions.

6. Pipette 1.0 mL of 6 M NaOH, sodium hydroxide solution into beakers C and D. Thoroughly mix the solutions

-What is the volume of 6HCl used for addition into beaker A,B,C,D?

-Calculate the pH of beaker A and B after the addition of beaker 6M HCL

-Calculate the pH of beaker C and D after the addition of beaker 6M NaOH

Given the following experimental procedure below: 1) What is the original concentration HCl and volume HCl used in dilution 2)Concentration of diluted HCl solution ------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------- 1. Obtain 60 mL of 0.1 M HCl, hydrochloric acid solution. 2. Using a clean, dry graduated cylinder, transfer 50 ml of this solution into a clean 100 or 150 mL beaker. Label the beaker with the concentration of the acid. 3. Pipette 5 mL of the remaining acid solution into a clean 50 or 100 mL graduated cylinder. The graduated cylinder only needs to be rinsed with distilled water. 4. Dilute the 5 mL of HCl to 50 mL with distilled water in the graduated cylinder. 5. This solution can now be transferred into a second clean 100 or 150 mL beaker and mixed thoroughly. Label the beaker with the new concentration of this acid solution. 6. Measure the pH of each of the two hydrochloric acid solutions with a pH meter. Make sure to rinse the pH electrode with distilled water between readings. Record each pH value. 7. Transfer these two solutions into a 600 mL waste beaker which will be taken care of at the end of the experiment and clean out the small beakers.

Measurement and Accuracy

Procedure

Obtain 5 large test tubes (all the same size), a test tube rack, 3 beakers of colored water A-C, and 3 graduated cylinders.

With a Sharpie, label the tubes 1-5

Measure 25 mL of solution from beaker A (red) using a clean graduated cylinder. Pour into tube 1.

Measure 28 mL of solution from beaker B (yellow) using a clean graduated cylinder. Pour into tube 3.

Measure 22 mL of solution from beaker C (blue) using a clean graduated cylinder. Pour into tube 5.

Pour 8 mL of solution from tube 3 into a clean graduated cylinder and add it into tube 4.

Pour 7 mL of solution from tube 5 into a clean graduated cylinder and add it into tube 4. Mix the solution by swirling the tube.

Pour 10 mL of solution from tube 1 into a clean graduated cylinder and add it into tube 2.

Pour 5 mL of solution from tube 3 into a clean graduated cylinder and add it into tube 2. Mix the solution by swirling the tube.

Data Sheet

For the column above labeled “Volume contained in the tube at the end”, calculate the volume that each solution should contain. After completing your calculations, do your test tubes appear to match your math?

If not, give an explanation of why they would be different.

Compare your tube 2 with two other groups’ tube 2, are they the exact same shade of color?

If not, give an explanation of why they would be different.

If the colors are different, which group has the “right” color? How did you determine this?

There are 0.10 M aqueous solutions of HCl and NaOH available in the lab for this part of the experiment. The acetic acid and sodium acetate solutions will have concentrations of 0.50 M.

3. Theoretical pH of solutions and deionized water after the addition of strong acid and strong base in Part II of the experiment.

Measure 20 mL of buffer solution A using a graduated cylinder and pour the solution into a clean beaker labeled A1. Measure 20 mL of buffer solution B using a clean graduated cylinder and pour the solution into a clean beaker labeled B1. Measure 20 mL of the deionized water sample from part I and pour the solution into a clean beaker labeled W1.

3. Using a clean graduated cylinder, add 10 mL of 0.10 M HCl (aq) to each solution A1, B1 and W1. Mix the solutions well using a glass stir rod making sure to rinse the stir rod in between mixing each solution. Measure and record the pH of all 3 solutions in your notebook.

4. Measure 20 mL of buffer solution A using a graduated cylinder and pour the solution into a clean beaker labeled A2. Measure 20 mL of buffer solution C using a clean graduated cylinder and pour the solution into a clean beaker labeled C2. Measure 20 mL of the deionized water sample from part I and pour the solution into a clean beaker labeled W2.

5. Using a clean graduated cylinder, add 10 mL of 0.10 M NaOH (aq) to each solution A2, C2 and W2. Mix the solutions well using a glass stir rod making sure to rinse the stir rod in between mixing each solution. Measure and record the pH of all 3 solutions in your notebook.

*** only need the second table filled out with theoretical, dont need the first table filled out

PLS HELP WITH CALCULATIONS

DATA:

PROCEDURE

You will be provided with two stock solutions, A and B. Solution A contains iodate ions and solution B contains sulfite ions along with some acid and starch. Note the concentration of each stock solution on your data sheet. In preparing your reaction systems, always add water first, followed by solution B, then add solution A.

Calculate the total volume of each needed reagent needed and record it on your data sheet. Pour approximately that amount from the reagent bottle into an appropriate size beaker. If you accidentally take too much, offer the extra to another group to minimize waste. For water, use distilled water.

Use 5.00 and 10.00 mL graduated pipets to measure out the larger volumes and 1.00 mL graduated pipets to measure out smaller volumes. Use a small (<250mL) beaker as your reaction vessel. Always add acid to water, never the other way around otherwise it can spatter and result in injury.

As temperature changes affect reaction rates, you will want to minimize contact with the solutions. After combining water and solution B, begin stirring using a glass stirring rod while another group member quickly adds solution A. Make sure the stopwatch is started as soon as solution A is added. Time each reaction using the stopwatch and record the time in ink on your data sheet. Record the temperature of the room for the reactions.