using stoichiometry. Another purpose is to measure and calculate percentage yield. Procedure: 1. Weigh out 1.0g of CaCl2*2H2O and put it into a 100mL beaker. 2. Add 25mL of distilled water and stir. 3. Using stoichiometry to determine how much Na2CO3 is needed for a full reaction. 4. Weigh the calculated amount and put it in a small paper cup. Add 25mL distilled water and stir. 5. Pour this solution into the beaker and watch as a precipitate forms instantly. 6. To set up a filtration assembly:
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Investigating Stoichiometry with Carbonic Acid Salts Problem: Testing the actual yield versus the theoretical yield of NaCl when HCl is titrated into Na2CO3 and NaHCO3. When 0.15g of both NaHCO3 and Na2CO3 are titrated with HCl‚ then 0.165g of NaCl should form from the NaHCO3‚ and 0.104g of NaCl should form from the 0.15g of Na2CO3. Procedure: Weigh 2 samples of 0.15g of dried unknown each‚ and dissolve each into 50mL of distilled water. Add 0.5 to 1mL of bromocresol green indicator until the
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Solvay process Raw materials - NaCl‚ salt - CaCO3‚ limestone - H2O‚ water - NH3‚ ammonia is recycled Useful products - sodium carbonate. Na2CO3 – reason for process Waste products - CaCl2‚ calcium chloride - Heat Chemical properties of the main product (Na2CO3) - Forms several hydrates which are used in many ways - It is moderately alkaline‚ so it can neutralise strong acids - Can precipitate many metal ions from solution as carbonates Uses of sodium carbonate - Glass
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carbonate. This formula is: Na2CO3(aq) + CaCl2. 2H2O(aq) à CaCO3(s) + 2NaCl(aq) + 2H2O 1. Put on your goggles. 2. Weigh out 1.0 g of CaCl2·2H2O and put it into the 100-mL beaker. Add 25 mL of distilled water and stir to form the calcium chloride solution. Use only distilled water since tap water may have impurities that interfere with the experiment. 3. Use stoichiometry to determine how much Na2CO3 you will need for a full reaction. 4. Weigh the calculated amount of Na2CO3 and put it in a small
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increasing atomic number with the elements having similar properties placed in vertical columns is known as periodic table. MATERIALS/REAGENTS AND EXPERIMENTAL PROCEDURE For the Group IA & IIA Elements‚ each small amount samples ofLi2CO3‚ Na2CO3‚ K2CO3‚ MgCO3‚ CaCO3 and BaCO3 was place in the different test tubes. After placing them in the test tubes‚ we identified the physical state‚ color‚ and appearance of each. Then we test the solubility of each sample by using water. For the Group IVA
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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 the net equation as below CO32- (aq) + Ca2+(aq) CaCO3(s) From the balanced net ionic equation‚ 1 mole of carbonate ion from the 1 mole of Na2CO3.H2O(molar mass 124.00 g/mol)reacts
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EXPERIMENT 2: SOLUTION PREPARATION AND STANDARDIZATION Submitted by Iris Olaso ______________________________________________________________________________ INTRODUCTION Generally‚ there are two ways in preparing a solution‚ one is by dissolving a weighed amount of solid in a required solvent and the other is by dilution of a concentrated solution into the desired concentration. In diluting concentrated solution‚ the concentration of the diluted solution can be determined by standardization
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AgCl - argentums/silver chloride HgCl - 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
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A double displacement reaction is a type of chemical reaction in which two compounds react in order to create two new chemicals. The two cations and anions switch places with each other which forms two new compounds. As an example AB+CC can switch to AD+CB. Both sides of these equations must balance out in order to be neutral. So any pairs of compounds (such as A+B) must have a total balanced charge. In this example A could have a charge of positive 2 (+2) and B could have a charge of negative
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Worked solutions to student book questions Chapter 4 Analysing acids and bases Q1. Antacid tablets should normally be chewed before they are swallowed. Why? A1. Antacid tablets are normally chewed to provide a larger surface area for faster reaction with stomach acids. Q2. A laboratory test to determine how much hydrochloric acid is neutralised by a brand of antacid does not give a complete picture of its effectiveness in the stomach. What other factors might be important? A2. Other factors to
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