changes when it is left in a sunny place. [1] © UCLES 2011 1113/01/SP/12 [Turn over 4 3 Maya investigates the reaction between calcium carbonate and hydrochloric acid. She adds dilute hydrochloric acid to some calcium carbonate (marble chips)‚ at room temperature. She collects the gas given off in a gas syringe. For Examiner’s Use dilute hydrochloric acid syringe calcium carbonate (a) Suggest one safety hazard in this experiment. How can Maya reduce the risk from this hazard? hazard how to
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fun in the process. LITERATURE: The acids in the vinegar make the shell deteriorate. Eggs contain "calcium carbonate"(this is what makes it hard)‚ and vinegar is an acid. When they both combine a chemical reaction takes place‚ and carbon dioxide is released. This is what bubbles are made of. The vinegar makes the egg soft because it takes all the carbon out. Since the egg shell is made out of "calcium carbonate" and is "eaten" up by the acidic vinegar. It leaves behind the inner membrane and gives
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is essential to their performance. In this laboratory exercise the aim is to test three drilling fluid samples for; density and rheological properties‚ Fluid loss‚ chemical analysis i.e. testing pH‚ alkalinity‚ testing for chloride ions‚ calcium carbonate‚ calcium‚ bentonite; also determining the amount of solids present in the samples as well as volumes of oil‚ water and solids contained in the sample‚ and to test for contaminates such as NaCl and KCl. These tests helps us to determine the properties
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weighing dish and Na2CO3 .72_g Net mass of the Na2CO3 .12_g Step 6: Mass of filter paper __1.0__g Step 10: Mass of filter paper and dry calcium carbonate __1.8__g Net mass of the dry calcium carbonate __.8__g (This is the actual yield) Step 11: Show the calculation of the theoretical yield of calcium carbonate. .0068 mol of CaCO3 *100.06 g CaCO3/1mol of CaCO3 =.6804 g of CaCO3 Show the calculation of the percent yield. (Actual yield/theoretical
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Rates of Reaction: Hydrochloric Acid + Calcium Carbonate Background Information: Hydrochloric acid is a clear‚ colourless‚ highly-pungent solution of hydrogen chloride (HCl) in water. It is a highly corrosive‚ strong mineral acid with many industrial uses. Hydrochloric acid is found naturally in gastric acid. Calcium carbonate is a chemical compound with the formula CaCO3. It is a common substance found in rocks in all parts of the world‚ and is the main
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Introduction: The back titration is a method used in determining the amount of excess of the reagent. The calcium carbonate is a substance which gives the eggshell stiffness. Research question: What is the amount of calcium carbonate in the eggshell measured by back titration? Table 1. Variables. Type of variable | Variable | Unit | Dependent | Amount of calcium carbonate in eggshell | % by mass | Independent | Volume of titrated excess of hydrochloric aced
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hydrochloric acid (HCl) with a pH of 2-3. When too much of this acid is formed in the stomach‚ heartburn and other discomfort occurs. This is when people grab for their antacids; these are bases that neutralize the excess acid in the stomach. Calcium carbonate‚ magnesium hydroxide‚ and aluminum hydroxide are all examples of bases used in antacids. In addition to these active ingredients‚ antacids also contain sweeteners‚ colourings‚ and “fillers” that may or may not affect the effectiveness of
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Republic of the Philippines DEPARTMENT OF EDUCATION REGIONAL SCIENCE HIGH SCHOOL FOR REGION I Division of La Union Bangar‚ La union Effectiveness of Snail shell (Nassariusmutabilis) asAdditive in Chalk Making Proponents: FERNAN MACUSI GERALD JAVAR (IV- Europium) ROGELIO C. VALDEZ (Research Adviser) Abstract Table of Contents Title……………………………………………………………………………………….…i Abstract…………………………………………………………………………………......ii
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The Effectiveness of Chalk Dust as Soil Neutralizer Queeneevi T. Quijano Carolyne B. Coronel Ergie P. Canillas IV-SSC A Mrs. Deborah Agustin Reseach Adviser TABLE OF CONTENTS Title Page Abstract . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . i Acknowledgement . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ii Introduction . . . . . . . . . . . . . . . . . . . . . . .
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Acetylene Materials Required: Large granules of Calcium Carbide Scoop or spatula to handle the calcium carbide 3 large test tubes of similar size with stoppers (held in large empty beaker) Wooden splint and lit candle Large beaker (500mL to 1L) half full of water Pre-lab Exercise: 1. In this lab we will produce acetylene by placing calcium carbide (CaC2) in water. Write the chemical formula for the reaction between calcium carbide and water knowing that the product is acetylene
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