The ingredients contained in grape Kool-Aid can be approximated as: water (H2O, density = 1.000 g/mL), sugar (sucrose, solid at room temperature, C12H22011), citric acid (solid at room temperature, C6HO7), and grape flavouring (methyl anthranilate, liquid at room temperature, CeH,NO2, density = 1.168 g/mL). (The blue and red dyes used to produce the purple colour are present in such small quantities that they can be ignored.) A sample of grape Kool-aid having a final total volume of 500 mL can be prepared from: 485 mL of water, 32.0 g of sugar, 5.00 g of citric acid, and 3.50 g or grape flavouring. Calculate the molarity and molality of grape flavouring in this mixture (assume that only water is the solvent). Fun fact: methyl anthranilate is also used as a bird repellant (to keep geese away).

The ingredients contained in grape Kool-Aid can be approximated as: water (H2O, density = 1.000 g/mL), sugar (sucrose, solid at room temperature, C12H22011), citric acid (solid at room temperature, C6HO7), and grape flavouring (methyl anthranilate, liquid at room temperature, CeH,NO2, density = 1.168 g/mL). (The blue and red dyes used to produce the purple colour are present in such small quantities that they can be ignored.) A sample of grape Kool-aid having a final total volume of 500 mL can be prepared from: 485 mL of water, 32.0 g of sugar, 5.00 g of citric acid, and 3.50 g or grape flavouring. Calculate the molarity and molality of grape flavouring in this mixture (assume that only water is the solvent). Fun fact: methyl anthranilate is also used as a bird repellant (to keep geese away).

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

A particular beer is 6.50 % ethanol by volume (C2H6O). If a single bottle of beer contains 750.0 mL of beer, what mass, in g of ethanol (C2 H6O), is present in the bottle? The density of ethanol is 0.789 g ethanol/mL ethanol.
A 335 −mL−mL can of soda pop contains 44 gg of sucrose (C12H22O11C12H22O11). Part A What is the molarity of the solution with respect to sucrose? Express your answer using two significant figures.
If the true density of the urine is 1.023 g/ml what is the technician's percent error? Q3. Consider the hydrated compound potassium ferrioxalate: K3[Fe(C₂O4)3] • 3H₂O (a) Determine the molar mass (g/mol) of the hydrated compound (b) If a student heats 11.39 g of the hydrate and obtains 10.28 grams of product, what would be the experimental mass percent of water in the original compound?
The average concentration of dissolved gold in earth's oceans is 5.8 x 10^−9 g/L. of ocean water.How many micrograms of gold are in 1.1x10^3 m^3 of ocean water? (1 ml = 1 cm3)
You wish to prepare 237 grams of 26.7% (w/w) KI. Assume that the density of water is 1.00 g/mL. You will need grams of potassium iodide and mL of water.
What is the concentration, in units of grams of dye per liter of solution (g/L), of the dilute dye solution that is produced as follows? Transfer 16.51 mL of the stock solution (6.12 g/L) to a 200.0 mL volumetric flask and dilute to the 200.0 mL line with deionized water. Your answer should be reported to the correct number of significant figures.
Automobiles are often implicated as contributors to global warming because they are a source of the greenhouse gas CO2. How many pounds of CO2 would your car release in a year if it was driven 110. miles per week? Gasoline is a complex mixture of hydrocarbons. In your calculations, assume that gasoline is octane (molecular formula C8H18) and that it is burned completely to CO2 and H2O in the engine of your car. Also assume that the car averages 27.3 miles per gallon and that the density of octane is 0.703 g cm-3.
Caffeine occurs naturally in tea leaves and coffee beans. Pure caffeine (mp 236°C) is a white crystalline solid material at room temperature. It is classified as an alkaloid - a nitrogen-containing basic compound that is obtained from plants and has physiological effects in the body. A student pulverizes 8.78 grams (g) of coffee beans into a finely ground powder by using a mortar and pestle. The caffeine is then extracted into 300 mL of boiling dichloromethane (CH2CI2) by the same solid- liquid extraction technique used in Unit 1. After 30 minutes, the solution is filtered hot to remove a large amount of brown insoluble material. Dichloromethane is removed from the filtrate via rotary evaporation, leaving 916.3 milligrams (mg) of caffeine behind, as a white solid. What is the percentage of isolated caffeine with respect to the starting amount of crude coffee beans? caffeine
11)
A chemist prepares a solution of zinc nitrate (Zn(NO3),) by measuring out 5.2 x 10ʻ µmol of zinc nitrate into a 500. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's zinc nitrate solution. Be sure your answer has the correct number of significant digits. H mol 回山国

A student sets up and solves the following equation to solve a problem in solution stoichiometry. Fill in the missing part of the student's equation. 6.9 ml)(0.11 1) (119.86|[]) = 91. g x10 X μ 00 5
(Incorrect) An impure sample of hydrocarbon having a total mass of 41.0 g undergoes combustion analysis to generate 82.6 g CO₂(g) and 16.9 g H₂O(g). Assuming that the impurities do not contain carbon or hydrogen, what percentage of the initial sample is the pure hydrocarbon? Provide the numerical value of your response in decimal notation rounded to 3 significant figures. You answered: 4.58 The correct answer is: 59.5%