Question

In Part 1 of Lab 2 you will make and standardize a solution of NaOH(aq). Suppose...

In Part 1 of Lab 2 you will make and standardize a solution of NaOH(aq). Suppose in the lab you measure the solid NaOH and dissolve it into 100.0 mL of water. You then measure 0.2013 g of KHP (KC8H5O4, 204.22 g/mol) and place it in a clean, dry 100-mL beaker, and then dissolve the KHP in about 25 mL of water and add a couple of drops of phenolphthalein indicator. You titrate this with your NaOH(aq) solution and find that the titration requires 9.91 mL of NaOH(aq).

Part 1: What is the concentration of your NaOH(aq) solution? ___________M NaOH Part 2: You will then make a Kool-Aid solution by dissolving the powder in an entire packet of lemon-lime Kool-Aid in 250.00 mL solution. You find the powder in a packet of lemon-lime Kool-Aid has a mass of 3.646 g.

In Part 2 of the lab you titrate 5.00 mL of the lemon-lime Kool-Aid (with 5 drops of thymol blue indicator) with your NaOH(aq) solution. The titration requires 10.07 mL of NaOH(aq). Determine the number of moles of NaOH(aq) required to titrate 5.00 mL of your Kool-Aid solution. _____mol NaOH

Part 3: Determine the number of moles of NaOH(aq) that would be required to titrate 250.00 mL of your Kool-Aid solution (the entire packet). __________mol total acid

Part 4: In Part 3 of the lab you titrate 25.00 mL of the lemon-lime Kool-Aid (with KI, HCl, and starch) with 0.001000 M KIO3(aq) solution. The titration requires 10.10 mL of KIO3(aq). Determine the number of moles of ascorbic acid in 25.00 mL of your Kool-Aid solution. _________mol ascorbic acid

Part 5: Determine the number of moles of ascorbic acid in 250.00 mL of your Kool-Aid solution (the entire packet). ______mol ascorbic acid

Part 6: If you titrated the entire packet of Kool-Aid, how many moles of NaOH(aq) would be neutralized in the titration due to the ascorbic acid? ________mol NaOH

Part 7: To titrate the entire packet of Kool-Aid, how many moles of NaOH(aq) would be neutralized in the titration due to the citric acid? _______mol NaOH

Part 8: Determine the number of moles of citric acid in the packet of Kool-Aid solution. ______mol citric acid

Part 9: Determine the mass (in mg) of ascorbic acid (C6H8O6) in your packet of lemon-lime Kool-Aid. ____________mg ascorbic acid

Part 10: Determine the mass (in g) of citric acid (C6H8O7) in your packet of lemon-lime Kool-Aid. ________g citric acid

Part 11: Determine the % by mass ascorbic acid in lemon-lime Kool-Aid. ___________% ascorbic acid

Part 12: Determine the % by mass citric acid in lemon-lime Kool-Aid. _______% citric acid

Part 13: Each packet of Kool-Aid contains 8 servings. Consider 8 to be an exact number. Determine the mass (in mg) of ascorbic acid (C6H8O6) in one serving of lemon-lime Kool-Aid. ________mg ascorbic acid

Part 14: Determine the mass (in g) of citric acid (C6H8O7) in one serving of lemon-lime Kool-Aid. _____g citric acid

Part 15: The recommended dietary allowance (RDA) for ascorbic acid (vitamin C) is 70 mg. Consider 70 mg to be an exact number. What percent of RDA for ascorbic acid (C6H8O6) is in one serving of lemon-lime Kool-Aid? ________%RDA vitamin C

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Part 1: What is the concentration of your NaOH(aq) solution? 1.00×10-1 M NaOH Ok. Part 2:...
Part 1: What is the concentration of your NaOH(aq) solution? 1.00×10-1 M NaOH Ok. Part 2: You will then make a Kool-Aid solution by dissolving the powder in an entire packet of lemon-lime Kool-Aid in 250.00 mL solution.  You find the powder in a packet of lemon-lime Kool-Aid has a mass of 3.654 g. In Part 2 of the lab you titrate 5.00 mL of the lemon-lime Kool-Aid (with 5 drops of thymol blue indicator) with your NaOH(aq) solution. The titration...
Based off info below please answer blank boxes. Thanks! Application Questions: 12. Before using a solution...
Based off info below please answer blank boxes. Thanks! Application Questions: 12. Before using a solution of NaOH as a standard for a titration, its precise concentration must be determined by titration with a standard acid. This is because solid NaOH absorbs water from the atmosphere, so its solid form is difficult to keep free of contaminated H2O. A common acid used for standardization is the acid-salt, potassium hydrogen phthalate (KHP), KHC8H4O4. Another way is to use a standardized solution...
I need to find the M of citric acid from my lab experiment. (This is a...
I need to find the M of citric acid from my lab experiment. (This is a common titration experiment with NaOH solution and citric acid soda. H3C6H5O7 (aq) +3NaOH (aq) ---> Na3C6H5O7 (aq) + 3H2O (l) The average molarity of my NaOH solution is 0.00896. My first trial resulted in a net 13.26mL. Molar mass of citric acid is 192.12352. How do I figure Mcitirc acid? Mol/can (355 mL) and g citric acid/can?
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown...
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown acid solution containing HCl was added to flask containing 30.00 mL of deionized water and two drops of an indicator. The solution was mixed and then titrated with NaOH until the end point was reached. Use the following titration data to determine the mass percent of HCl in the acid solution. Mass of flask: 125.59 g Mass of flask + acid solution: 129.50 g...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution? 2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare the NaOH Solution Take a 250 mL volumetric flask from the Containers shelf and a balance from the Instruments shelf and place them on the workbench. Zero the mass of the volumetric flask on the balance. Take sodium hydroxide from the Materials shelf and add 1 g to the flask. Record the mass from the balance display. Place the volumetric flask on the workbench....
You will need the answer tio question 2 during the experiment. 1) At the endpoint of...
You will need the answer tio question 2 during the experiment. 1) At the endpoint of a titration, the color of the solution should be (a)bright pink, (b) pink, (c) faint pink, (d) colorless ? 2)We will calculate the amount of acid to use in each titration. Assume that you are using 0.0512 M NaOH (aq). A good violume of NaOH(aq) to use per titration is 15ml, From this molarity and volume, the moles of NaOH can be calculated. Since...
A solution of NaOH (aq) of unknown concentration, is added from a buret into an Erlenmeyer...
A solution of NaOH (aq) of unknown concentration, is added from a buret into an Erlenmeyer flask containing 25.00 ml of 0.2000 M HCI (aq). A small amount of phenolphthalein indicator is also present in the acid, initally. A very pale pink but permanent color appears in the Erlenmeyer upon the addition of 41.22 ml of the base solution. The appearance of the color signifies the end point of the titration. a) Please write a balanced molecular equation for the...
Molarity of NaOH and molecular weight of the unknown acid Part A Run 1 Run 2...
Molarity of NaOH and molecular weight of the unknown acid Part A Run 1 Run 2 Mass of H2C2O4*2H20 used in grams 0.2127 0.2124 Moles of H2C2O4*2H2O (mol) 1.69 *10^-5 1.69*10^-5 Number of protons available for reaction with OH- 2H 2H Moles of OH- which reacted (mol) 2 2 Volume of NaOH solution used (mL) 18.71 19.15 Molarity of NaOH soultion (M) .12 .12 Average molarity of NaOH (M) Part B with unkown sample Run 1 Run2 Mass of unknown...
Vitamin C tablets contain ascorbic acid (C6H8O6= 176.1232 g/mol) and a starch "filler" which holds them...
Vitamin C tablets contain ascorbic acid (C6H8O6= 176.1232 g/mol) and a starch "filler" which holds them together. Your goal today is to determine how much vitamin C or ascorbic acid, HC6H7O6 is present in the tablet. This can be determined by titrating ascorbic acid, HC6H7O6 with calcium hydroxide solution, Ca(OH)2(aq) (74.0918 g/mol) according to the following equation: 2HC6H7O6(aq) + Ca(OH)2(aq) ---> Ca(C6H7O6)2(aq) + 2H2O(l) First you must make 500 mL of a 0.1012 M standard solution of Ca(OH)2 from a...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT