Beyond the Course: Your beverage company is branching out from added sugar in their beverages to make a drink where the main ingredient is fresh-squeezed orange juice, called Beverage C. Yum! The beverage will still be subjected to the same taxes as Beverages A & B, so determining sugar content is still vital. Suggest a method of reliably examining the sugar concentration in each batch of Beverage C. Some considerations to address: Do you want to measure the same property for Beverage C as you did for Beverages A & B? Can you use the same calibration curve as you did for Beverages A & B? Describe the considerations you made when determining your method.

Beyond the Course: Your beverage company is branching out from added sugar in their beverages to make a drink where the main ingredient is fresh-squeezed orange juice, called Beverage C. Yum! The beverage will still be subjected to the same taxes as Beverages A & B, so determining sugar content is still vital. Suggest a method of reliably examining the sugar concentration in each batch of Beverage C. Some considerations to address: Do you want to measure the same property for Beverage C as you did for Beverages A & B? Can you use the same calibration curve as you did for Beverages A & B? Describe the considerations you made when determining your method.

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...

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1.) In a 15.00 g sample of ferilizer that is 10-30-10 by label, how many grams of pure phosphorus do you expect if the label is accurate, and how many grams of phosphorus do you expect if the label measures diphosphorus pentoxide? 2.) Assuming that the label from the previous question is accurate, and represents the phosphorus content, how many moles of magnesium would you need to fully precipitate the phosphorus (what is the molar ratio between phosphorus/phosphate and magnesium)? How many mL of 0.5 M MgSO4 x 7H2O is needed to fully deliver this molar amount?
7. Given: • The solubility of X at 100°C in water is 18.0 g/100 mL water. • The solubility of X at 0°C in water is 3.6 g/100 mL water. How many mL of boiling water would be required to dissolve 25g of X? If that solution was then cooled down to 0°C, how many grams of X could then crystallize out? What would be the maximum yield recovery for X?
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Predicting the product The names and chemical formulae of some chemical compounds are written in the first two columns of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. Then, write down in the third column of the table the chemical formula of the major chemical species that will be present in this solution. For example, you know water itself will be present, so you can begin each list with the chemical formula for water (H₂O). Note: "major" chemical species are those present in concentrations greater than 10 -6 compound potassium hydroxide iron(11) iodide iron(II) sulfate Explanation Check formula KOH Fel₂ FeSO4 major species present when dissolved in water 0 0 0 X mol/L. 0.0.... S Graw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessit
Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in this solution are written in the second column of the table. Use the checkboxes to dassify each compound.
Suppose you test a sample of a carbonated beverage with concentrated nitric acid and 2.5% ammonium molybdate, and a precipitate forms. What would this tell you about your carbonated beverage? a. This will tell you that the test solution turned into a solid. Carbonation refers to carbon dioxide dissolved in a liquid, and the rate at which carbon dioxide dissolves or is soluble depends on temperature. b. Testing a sample of a carbonated beverage would prove to be carbonated. c. A precipitate forming would show the beverage contains calcium ions. d. The carbonated beverage would test positive for ammonium ions. e. The carbonated beverage may have similar contents to the milk. f. The test would tell you that the carbonated beverage contains phosphate.
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