Sub parts 2, 3, and Read the following statements. Choose the letter of the correct answer.1. An antimicrobial agent preservative that inhibits the growth of molds, yeastand bacteria in food.C. SorbatesA. BenzoatesВ. NitratesD. Acids2. Which of the following are natural food preservatives?I. VinegarII. SaltA. I and IIIIII. PotassiumIV. SugarС. I, IVВ. В. I, II,IVD. I,IV3. Preservatives that kill bacteria and other microorganisms in foods especiallyin acidic conditions.A. BenzoatesC. SorbatesВ. NitratesD. Acid 7. Statement 1: All food additives are carcinogenic.Statement 2: Food additives must be avoided as much as possible.A. True, FalseB. True, TrueC. False, FalseD. False, True8. How do thickeners improve a food product?A. They prevent spoilage due to oxygenationB. They increase the viscosity of a productC. They preserve the flavor of a productD. They keep food from drying out._9. It makes the food thicker by keeping oil and water mixed together.A. EmulsifiersC. HumectantsB. Flavor EnhancerD. Antioxidants

Food preservatives are the substances which are added to food items in order to preserve them for a…

An antimicrobial agent preservative that inhibits the growth of molds, yeast and bacteria in food. C. Sorbates D. Acids A. Benzoates B. Nitrates Which of the following are natural food preservatives? I. Vinegar П. Salt A. I and III III. Potassium IV. Sugar С. II, IV В. В. I, II,IV D. I,IV

An antimicrobial agent preservative that inhibits the growth of molds, yeast and bacteria in food. C. Sorbates D. Acids A. Benzoates B. Nitrates Which of the following are natural food preservatives? I. Vinegar П. Salt A. I and III III. Potassium IV. Sugar С. II, IV В. В. I, II,IV D. I,IV

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 12CR: Without consulting your textbook, list and explain the main postulates of the kinetic molecular...

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The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O
A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?
Without consulting your textbook, list and explain the main postulates of the kinetic molecular theory for gases. How do these postulates help us account for the following bulk properties of a gas: the pressure of the gas and why the pressure of the gas increases with increased temperature; the fact that a gas tills its entire container; and the fact that the volume of a given sample of gas increases as its temperature is increased.
Physiological saline concentration—that is, the sodium chloride concentration in our bodies—is approximately 0.16 M . A saline solution fur contact lenses is prepared to match the physiological concentration. If you purchase 25 mL of contact lens saline solution, how many grams of sodium chloride have you bought?
It is stated in Section 6.3 of the text that to balance equations by inspection you start “with the most complicated molecule.” What does this mean? Why is it best to do this?
What is the difference between a solute and a solvent?
In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A 0.256-g sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it bad a mass of 0.308 g. A second sample of 0.416 g of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was 0.145 g. a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.
Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C), filtering to remove insoluble impurities, cooling to 0 C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 C is 164 g/L. Its solubility in cold water of 0 C is 69 g/L. What is the percent yield of NaHCO3 when ills purified by this method?
A certain grade of steel is made by dissolving 5.0 g of carbon and 1.5 g of nickel per 100. g of molten iron. What is the mass percent of each component in the finished steel?
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?
Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?