these kinds of water for a long time‚ calcium hydroxide in the cement paste dissolves first (per liter water can dissolve calcium hydroxide of 1.3g). Under the role of still water or zero-pressure water‚ the dissolution will stop because the surrounding water is easy to get saturated due to the dissolved calcium hydroxide‚ and dissolution only occur on the surface‚ little impact. But if the cement paste is in fluid water or pressure water‚ the dissolved calcium hydroxide is easy to be washed away‚
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M(OH)y + Y HCl [pic] Y H2O + M+y + Y Cl- Additionally‚ some brands of antacids use calcium carbonate as a neutralizing reagent. CaCO3 + 2 HCl (aq) [pic] H2CO3 (aq) + Ca2+ (aq) + 2 Cl-(aq) The carbonic acid formed in this reaction may undergo further reaction: H2CO3 (aq) [pic] H2O (l) + CO2 (g) Procedure Outline This experiment will involve several steps. The first step will involve a simple reaction to determine the concentration of the NaOH that will be used in this experiment using a solid
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at least one risk factor. • over 65 and never had a test • You experience early menopause • You use medication that cause osteoporosis • You have type 1 Diabetes‚ Liver disease‚ Kidney disease or a family history T Score • A T-score that helps determine whether a person is at risk for fractures. • A T-score of -2.5 or lower is defined as osteoporosis. • The lower the score‚ the greater your fracture risk can be. NOF/WHO Criteria for Assessing Disease Severity • Bone Mass score- the standard deviation
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be made‚ as our results were not as accurate as we would have liked them to be. These improvements include being more careful when measuring out the hydrochloric acid in the graduated cylinder‚ putting the lid of the tube on faster right after the calcium chloride has been added so that no gas produced can escape‚ and making sure the very fine grains do not get stuck on the tube instead of going all the way down the tube into the hydrochloric acid. The rate of a chemical reaction is the speed at which
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concentration of CaCO3 obtained was 1034 ppm‚ with a standard deviation of 2.4495. The results indicate that the unknown solution can be considered as hard water. Introduction The hardness of water is defined in terms of its cation content‚ which includes calcium‚ magnesium‚ iron‚ zinc‚ and other polyvalent metal ions. These metal ions interfere with the use of the water for many applications. For example‚ these ions diminish the effectiveness of soap and detergent for cleansing operations; they diminish
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Limestone is a sedimentary rock composed largely of calcium carbonate (CaCO3). Many limestones are composed from skeletal fragments of marine organisms such as coral or foraminifera. Limestone makes up about 10% of the total volume of all sedimentary rocks. The solubility of limestone in water and weak acid solutions leads to karst landscapes‚ in which water erodes the limestone over thousands to millions of years. Most cave systems are through limestone bedrock. Limestone has numerous uses‚ including
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hydroargentum chloride‚ mercury chloride Sulphate All sulphate salt dissolve in water except; PbSO4 ‚ BaSO4 ‚ CaSO4 Carbonate All carbonate salt not dissolve in water except; Li2CO3 Na2CO3 ‚ K2CO3 ‚ (NH4)2CO3 Oxide All oxide not dissolve in water except; Na2O ‚ K2O ‚ CaO Hydroxide All hydroxide not dissolve in water except; NaOH‚ KOH‚ Ca(OH)2 ‚ Ba(OH)2 Formula to determine the heat change; Heat released/absorbed‚ H = mcӨ [unit = J or kJ] Symbol Description Unit m mass of solution
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Synopsis The objective of this experiment is to determine the percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the
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and detrimentally altered. In a process called ocean acidification‚ chemical reactions between absorbed carbon dioxide and H2O occur that reduce the pH of seawater‚ as well as decrease carbonate ion concentration and saturation states of calcium carbonate minerals (“Ocean Acidification‚” PMEL). This calcium carbonate is necessary for the formation of skeletons and shells of many marine organisms. Therefore‚ acidification is damaging‚ and likely killing‚ large amounts of sea life (Horsey‚ 2012). The
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is really gypsum (calcium sulfate)‚ but often people call it "chalk". People use it for drawing on hard things‚ because it is soft. If this chalk is rubbed on something hard or rough‚ it will leave a mark. People often write with chalk on a chalkboard or blackboard. A chalk eraser or water can be used to clean the chalk marks away so the board is blankagain. Shops usually sell blackboard chalk in sticks that are about 5 cm long. The main component of chalk is calcium carbonate (CaCO 3 )‚ a form
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