QUESTION 11A 500.00 mg vitamin C (MW176.12g/mol) tablet was ground, acidified, and dissolved in H20 to make a 250.0 ml solution. A 50.00 ml aliquotcontaining vitamin C, Kl and starch was analyzed and titrated with 12.31 mL of 0.01042 M KIO3. What is the % (w/w) vitamin C in the tablet?KIO3 + 5 KI + 6 H* = 3 12 + 6 K* + 3 H20C6H806 + 12 = C6H6O6 + 21 + 2H*3.39 %67.77 %22.59 %33.89 %

KIO3(aq) first forms I2(aq), and the I2(aq) reacts with vitamin C (C6H8O6). Hence the required mole…

A 500.00 mg vitamin C (MW176.12g/mol) tablet was ground, acidified, and dissolved in H20 to make a 250.0 mL solution. A 50.00 ml aliquot containing vitamin C, KI and starch was analyzed and titrated with 12.31 mL of 0.01042 M KIO3. What is the % (w/w) vitamin C in the tablet? KIO3 + 5 KI + 6 H* = 3 12 + 6 K* + 3 H20 C6H8O6 + l2 = C6H606 + 21" + 2H* 3.39 % 67.77 % 22.59 % 33.89 %

A 500.00 mg vitamin C (MW176.12g/mol) tablet was ground, acidified, and dissolved in H20 to make a 250.0 mL solution. A 50.00 ml aliquot containing vitamin C, KI and starch was analyzed and titrated with 12.31 mL of 0.01042 M KIO3. What is the % (w/w) vitamin C in the tablet? KIO3 + 5 KI + 6 H* = 3 12 + 6 K* + 3 H20 C6H8O6 + l2 = C6H606 + 21" + 2H* 3.39 % 67.77 % 22.59 % 33.89 %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

On an emergency cart, you have sodium bicarbonate solution (NaHCO3), 44.6 mEq/50 ml. A physician orders an aerosol of 5 cc and 3.25% strength. How many milliliters of the bicarbonate solution do you need? 1 mEq=1/1000 GEW; GEW= gram formula wt/valence Atomic weights: Na, 23; H, 1; C, 12; 0, 16
Give handwritten answer- Calculate the amount of chlorine needed to disinfect 50 ML water to a residual dose of 0.3 mg/L. You need to add an additional 0.4 mg/L to the water in order to reach the breakpoint for chlorine addition based upon jar tests for this particular drinking water.
Too much manganese in drinking water can cause the following undesirable effects: black to brown color; black staining; bitter metallic taste . The EPA's Secondary Maximum Contaminant Level for manganese in drinking water is5.00×10-2 mg/L.(1) If 1.52×104 liters of water in a storage tank contains 1.08 grams of Mn , what is the contaminant level in ppm? ppm Assume that the density of the impure water is 1.00 g/mL.(2) Is this level acceptable based on EPA guidelines?
Need asap. Give 3 objectives for distillation of alcoholic beverage
A sample (50 mL) of a bottled water was added to a 100 mL volumetric flask and then diluted to the mark. From this stock solution, 50 mL was taken, added to a 100 mL volumetric flask and diluted to the mark. Final concentration of the serial dilution: 587.7161ppm. 1. what is the concentration in the original bottle (ppm)
1. A 0.68 gram sample of a volatile liquid was heated to 358 K. The gas occupied 265 mL of space at a pressure of 0.95 atm. What is the molecular weight of this gas? PV = nRT and R = 0.082 atmL/moleK. (Make sure that all your units agree/match R)2. An aspirin sample, 0.62 grams, was titrated with 28 mL of 0.105 M NaOH solution. What is the percent purity of this aspirin sample? (MM of Aspirin = 180. g/mol)3. A sample of hydrate was heated thoroughly. How many waters of hydration are there if the anhydrous salt had a dry mass of 12 grams and a molar mass of 185 g/mol? The mass of water evaporated from the hydrate was 5.0 g.4.A sample of water (80 grams) had a temperature change of 6. ℃. What was the heat change of this sample? (q = m c ΔT, c = 4.18 J/ g ℃)5. A 6.0 gram sample of epsom salt, MgSO4 ·nH2O, was heated. After heating, 2.9 grams of anhydrous salt remained. How many waters of hydration does epsom salt contain?6. What is the theoretical yield of aspirin if you started your…
114.7 mg of NaCl (MM=58.44 g) is dissolved in 246.42 L of water. What is the concentration of Na+ ion (MM=22.99 g/mol) in ppm? Give your answer rounded to four digits to the right of the decimal point. Hint: If you are stuck, calculate the %w/w of Na in NaCl using the molar masses - from pe106. Convert g to mg.
Tea leaves were boiled in water and around 1.50 grams of caffeine were extracted by 200.0 mL of water. If three portions of 25.0 mL of dichloromethane were used to extract the caffeine from the aqueous layer, how much caffeine will be extracted by the dichloromethane? Solubility of caffeine in water: 2.18 g per 100 mL waterSolubility of caffeine in dichloromethane: 18.2 g per 100 mL dichloromethane
A 1 mL microbial suspension comparable to 1 mL of 1.0 McFarland standard was subjected to a series of dilutions. An aliquot of 0.2 mL was transferred into a 100-mL volumetric flask and diluted with sterile saline solution to its final volume. Then a 0.1 mL of the resulting solution was transferred into a 50-mL volumetric flask diluted to its final volume. What would be the final concentration?
Have 50 gallons of water dripping concentrated nutrients into the water system. Need a concentration of 1500 ppm. Using 16% N, 5% P, 30% K, 15% Mg, and 5% Ca.
Your supervisor asks to make 300 mL of a 1.0% (w/v) starch solution using a 5% (w/v) stock solution. You have calcuated how much stock solution you need. But, how much water (in mL) will you need to add to the stock to achieve the correct final concentration?
2. Place a cup of water in a beaker or a pan. Then heat it using a hot plate or stove. Place a thermometer in the liquid and record the temperature at which it starts to boil. Repeat the experiment, but this time, use corn oil instead of water. Which has a higher boiling point, water or corn oil? Explain the results of your experiment. 3. Why is ethanol (C2H6O) soluble in water? What products in the market use the solution of ethanol and water? 4. During respiration, we inhale oxygen gas (O2) and exhale carbon dioxide (CO2). Why do you think these compounds exist as gases at room temperature?