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 up
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dissolved minerals. (2) Some of the minerals come from chalk‚ limestone or marble‚ which the water may have flowed over or through. (4) Hard water contains calcium or magnesium ions. Limestone‚ marble or chalks are insoluble in pure water however they will dissolve slowly in acidic rain. If your water has emerged through limestone or chalk (calcium carbonate) it will be hard. (1) Soft water is gratification water in which the only cation (positively charged ion) is sodium. The minerals in water give it an
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carbon dioxide in the atmosphere that we don’t see or feel because its effects are happening underwater. When carbon dioxide is absorbed by seawater a chemical reaction occurs that reduces the seawaters pH‚ carbonate ion concentration‚ and saturation states of biologically significant calcium carbonate minerals. It decreases the pH of seawater‚ meaning it increases the seawater’s acidity. Over the past 250 years‚ ocean acidity has increased by 30 percent. At least one-quarter of the carbon dioxide CO2
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HARVESTING THE OCEAN BY: SHUN ITCHIGAWA AQUACULTURE • the use of agricultural techniques to breed and raise marine organisms. • is the farming of freshwater or marine organisms. -MONOCULTURE -POLYCULTURE what is the important of aquaculture? It supply commercial species to the world’s markets. Common Aquaculture in the World • Fish aquaculture- raising fish commercially in tanks‚ ponds‚ or ocean enclosures. - carp‚ salmon‚ tilapia and catfish. • Raft culture- aquaculture using floating rafts
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0.0899 g/L 1.640 g/L 1.54 g/L 1.25 g/L 1.34 g/L 1.43 g/L 2.532 g/cm 3 2.165 g/cm 3 2.92 g/L 1.00 g/cm 3 −101 −35 −259 −115 −85 −253 −85 −61 −210 −164 −218 851 801 −73 −196 −152 −183 Decomposes 1413 −10 100 Oxygen Sodium carbonate Sodium chloride Sulfur dioxide *Water (at 4°C) 0 NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 2 Formulas D= m V D = density K = °C + 273 PV1 PV 1 = 2 2 T1 T2 Pt = P1 + P2 + P3 + ... M1V1 = M2V2 PV = nRT
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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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composition of each substance in a salt mixture To better understand the concepts‚ we look at the reaction below. The reaction of sodium carbonate and calcium chloride is an aqueous system. The molecular form of the equation is Na2CO3.H2O + CaCl2.2H2O → CaCO3 + 2NaCl + 3H2O As the two reactant salts and sodium chloride are soluble in water but calcium carbonate is insoluble‚ the ionic equation for the reaction is that we present only the ions that react (after removing the spectator ions)we have
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reaction in between calcium carbonate and hydrochloric acid. My hypothesis was that if the surface area to volume ratio of calcium carbonate was increased‚ then the rate of the reaction will increase because there are more particles that are accessible by the hydrochloric acid‚ thus more particles that can react with each other. Variables Independent- Surface area of calcium carbonate Dependent- Amount of carbon dioxide produced (cm3) Controls- Amount of calcium carbonate (g) Volume of
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Introduction The major component of eggshells is calcium carbonate (CaCO3). Calcium carbonate cannot be dissolved in water‚ but can dissolve in an acid using the reaction: 2HCl(aq)+CaCO3(s) Ca2+(aq)+CO2(g)+H2O+2HCl-(aq) This reaction is not used to titrate the CaCO3 because it is very slow when the reaction is close to the endpoint. Instead adding an excess of acid to dissolve all of the CaCO3 and then titrating the remaining H3O+ with NaOH solution can achieve the determination of the amount
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and Na2CO3 __1.4__g Net mass of the Na2CO3 __0.7__g Step 6: Mass of filter paper __0.7__g Step 10: Mass of filter paper and dry calcium carbonate __1.2__g Net mass of the dry calcium carbonate _0.5___g (This is the actual yield) Step 11: Show the calculation of the theoretical yield of calcium carbonate. The mole ration between CaCl2-.2H2O and CaCO3 is 1:1 that means that if we have 0.00680 moles of CaCl2-.2H2O we will get 0.00680 moles CaCO3 Convert
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