CHEMISTRY EXPERIMENT NUMBER 8 PERCENTAGE OF WATER IN A HYDRATE Objectives 1. To determine the percentage of water in barium chloride dihydrate. 2. To determine the percentage of water in an unknown hydrate salt. 3. To calculate the water of crystallization for the unknown hydrate salt. Discussion A hydrate salt is composed of anions (negative ions) and cations (positive ions) which are surrounded by and weakly bonded water molecules. Each hydrate salt has a fixed number
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law of conservation of matter. His theory was that matter cannot be created or destroyed and that chemical reactions only rearrange the way that atoms are combined; the atoms themselves don’t change. The procedure went like this... 1) Pour 15 ml of Barium Chloride into the bottle. 2) Pour 4 ml of Sodium Sulfate Solution into the test tube. 3) Stand the test tube in the bottle as shown below. 4) Weight the whole apparatus. 5) Record the weight‚ now turn the bottle over slowly to allow the solutions
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equation will be: CuSO45H2O + Ba(NO3)2 →BaSO4+ Cu(NO3)2 We can measure the mass of copper (Ⅱ) sulfate and the mass of the barium nitrate. Thus‚ we can calculate the theoretical yield of barium sulfate. By this‚ it is possible to find out the percent yield of barium sulfate; if we found the experimental yield. The percent yield of barium sulfate= experimental yield of barium sulfate
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seven wells in rows A through E: cobalt (II) nitrate‚ copper (II) nitrate‚ iron (III) nitrate‚ barium nitrate‚ and nickel (II) nitrate. Afterward‚ two drops of each of sodium phosphate‚ sodium iodide‚ sodium sulfate‚ sodium chloride‚ sodium bicarbonate‚ sodium carbonate and sodium hydroxide were added to the five vertical wells under columns 1-7. |cobalt(II)nitrate|copper(II)nitrate|iron(III)nitrate|barium nitrate|nickel(II)nitrate| sodium phosphate|Precipitated a purple color|Precipitated a light
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Tl+ = low solubility (insoluble) silver chloride‚ AgCl‚ forms a white precipitate + any other cation = soluble potassium bromide‚ KBr‚ is soluble Sulfate (SO42-) + Ca2+‚ Sr2+‚ Ba2+‚ Ag2+‚ Pb2+‚ Ra2+‚ Hg2+ = low solubility (insoluble) barium sulfate‚ BaSO4‚ forms a white precipitate + any other cation = soluble copper sulfate‚ CuSO4‚ is soluble sulfide (S2-) + alkali ions (Li+‚ Na+‚ K+‚ Rb+‚ Cs+‚ Fr+)‚ alkali earth metals (Be2+‚ Mg2+‚ Ca2+‚ Sr2+‚ Ba2+‚ Ra2+)‚ and H+(aq)
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conductimetric titration and by gravimetric determination. The conductivity was analyzed during the reaction between the sulfuric acid (H2SO4) and barium hydroxide (Ba(OH)2). Through the conductivity‚ the equivalence point can be determined; from there‚ the concentration of the Ba(OH)2 solution can be found. The final product of the reaction between sulfuric acid and barium hydroxide is insoluble. According to the lab manual‚ during the reaction‚ the total number of dissociated ions in solution is greatly reduced
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to green. Sodium sulphide forms H2S gas with rotten egg smell and also turns lead acetate paper silvery black. c)Sodium sulphide (Na2S)& Sodium sulphate (Na2SO4) using barium chloride(BaCl2) Ans: Sodium sulphate (Na2SO4) forms white ppt. with barium chloride (BaCl2)‚ Sodium sulphide (Na2S) does not form any ppt. with barium chloride(BaCl2) d)Sodium chloride (NaCl)&Sodium nitrate (NaNO3) using conc. Sulphuric acid Ans: Sodium chloride (NaCl) forms HCl gas with conc. Sulphuric acid
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Discussion The data supported the hypothesis that if Daphnia are placed in differently concentrated solutions of barium and calcium chloride‚ then the highest concentration of calcium chloride would affect them the most because of the production of hydrochloric acid and calcium oxide from the mixing of water and calcium chloride‚ two very dangerous acids‚ with the highest concentration having the biggest chemical reaction. Within five minutes of putting the Daphnia into the 10 (ppt) solution of
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added to a carbonate solution and an effervescent reaction would confirm the presence of carbonate anions. Another sample of carbonate solution was to be reacted with hydrochloric acid and the gaseous product was to be reacted with a suspended drop of barium carbonate. The presence of clouding in the droplet would also confirm the presence of carbonate anions. Silver nitrate was to be added to chloride solution and the
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identified it to be iron as it gave a yellow colour during the flame test narrowing it down to be barium or iron(iii). It then produced a yellow precipitate during sodium hydroxide test showing that it was iron(iii) instead of barium. The chemical equation for this reaction is: Fe2(SO4)3(aq) + NaOH(aq) Fe(OH)3(s) + Na2SO4(aq) I identified it as being a sulphate as it produced a white precipitate during the barium chloride test‚ indicating that sulphate ions are present. The chemical equation for this reaction
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