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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stone composition | Calcium oxalate | Diagnosis: PRIMARY HYPERPARATHYROIDISM Primary hyperparathyroidism is a disorder of the parathyroid glands wherein people with this disorder have one or more enlarged‚ overactive parathyroid glands that secrete too much parathyroid hormone (PTH).The parathyroid glands are located behind the thyroid gland. The effects of parathyroid hormone on serum calcium are mediated by increasing renal tubular resorption of calcium‚ increasing calcium absorption from the
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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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good fit. Builder’s putty also mainly contains chalk as a filler in linseed oil. Chalk may be used for its properties as a base. In agriculture‚ chalk is used for raising pH in soils with high acidity. The most common forms are CaCO3 (calcium carbonate) and CaO (calcium oxide). Small doses of chalk can also be used as an antacid. Additionally‚ the small particles of chalk make it a substance ideal for cleaning and polishing. For example‚ toothpaste commonly contains small amounts of chalk‚ which serves
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kettles and washing machines. The chemical name for lime scale is calcium carbonate‚ chemical formula CaCO3. It is usually caused by hard water (Water containing a higher than normal concentration of dissolved minerals such as calcium and magnesium). http://www.purewaterpeople.co.uk/blog/2013/06/what-is-limescale/ How is lime scale formed? Lime scale is built up over a long period of time. When hard water evaporates the calcium carbonate deposits are left behind and over time they start building
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