the concentration of sodium carbonate in an unknown sample by titration. The solution of hydrochloric acid was prepared and standardized using Na2CO3. Observations: Week 1: Standardizing hydrochloric acid using sodium carbonate with bromocresol green indicator Table 1: Titration of sodium carbonate using hydrochloric acid Trial | Mass of Na2CO3 (g) | Burette Reading (mL) | Final Volume of HCl (mL) | | | Initial | Final | | 1 | 0.2123 | 0.00 | 42.34 | 42.34 | 2 | 0.2195 | 0
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Analysis of Soda Ash and Volumetric Analysis of a Carbonate-Bicarbonate Mixture Buti‚ Mary Daphne A. Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas España‚ Manila Abstract Sodium carbonate (Na2CO3)‚ commonly known by trade name soda ash‚ is a white‚ anhydrous‚ powdered or granular material that is an essential raw material used in the manufacturing of glass‚ detergents‚ chemicals‚ and other industrial products. In this experiment‚ the percent alkalinity
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In this practical the aim was to determine the concentration of Na2CO3 in a standard solution‚ by using Hydrochloric acid to neutralise it. This experiment involved using distilled water to dissolve the sodium carbonate until 250 ml of solution were made. I had to calculate‚ from the information provided‚ how much sodium carbonate to use in the making of the solution. Using the volume and concentration of the solution‚ I was able to calculate the moles of the solution (concentration x volume). Using
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Chemistry Investigation 14: ------------------------------------------------- To determine the enthalpy change of reaction for: ------------------------------------------------- Na2CO3(aq) + H2O(l) + CO2(g) → 2NaHCO3(aq) Given: S1— Anhydrous sodium carbonate (Na2CO3) S2— Anhydrous sodium hydrogen carbonate (NaHCO3) A1—Aqueous sulfuric acid (H2SO4)‚ 0.500mol dm-3 Apparatus | Uncertainty | Measuring cylinder | ± 0.5 ml | Electronic Balance | ± 0.001 g | Data logger | ±0.2 ℃ |
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February 27‚ 2013 Abstract The analyte used is the soda ash which is titrated with an HCl titrant‚ standardized by Na2CO3. The indicators used are phenolphthalein for basicity and methyl orange for acidity. The two volumes of the titrant are then used to calculate percent composition of soda ash analyte. At the end of the experiment‚ the calculated average percent by mass of Na2CO3 is 4.92% and the average percent by mass of NaHCO3 is 5.07%. Introduction Soda ash is the common name for sodium carbonate
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using Method of Double Indicators Student Handout Purposes To determine the composition of the following mixture by double indicator method: 1. NaOH(aq) and Na2CO3(aq) 2. NaHCO3(aq) and Na2CO3(aq) Introduction Consider a mixture of NaOH(aq) and Na2CO3(aq). Reaction between HCl(aq) and Na2CO3(aq) takes place in two stages: HCl(aq) + Na2CO3(aq) ⎯→ NaHCO3(aq) + H2O(l) …………………. (1) HCl(aq) + NaHCO3(aq) ⎯→ NaCl(aq) + CO2(g) + H2O(l) …………. (2) While that between HCl(aq) and NaOH(aq) completes in only
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between Na2CO3 and CaCL2. Sample Observations Na2CO3 solution COLORLESS CaCL2 solution COLORLESS Na2CO3 + few drops of CaCL2 Produced a cloudy‚ white mixture After Filtration Precipitate WHITE Filtrate COLORLESS C. FILTRATE TEST Table 4.5. The filtrate test. Condition Observations Filtrate + CaCL2 COLORLESS SOLUTION Filtrate + Na2CO3 FORMATION OF WHITE PRECIPITATE Table 4.6. Summary of the filtrate test. Group No. Color of filtrate Filtrate + CaCl2 Filtrate + Na2CO3 Limiting
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include determining the amount of Na2CO3 needed to do a full reaction. This was calculated through stoichiometry calculations: Molar mass was first calculated for CaCl2*2H2O Ca = 40.078g Cl2 = 35.453g*2 = 70.906g 2H2 = 1.00794g*4 = 4.03176g 2O = 15.9994g*2 = 31.9988g 40.078g + 70.906g + 4.03176g + 31.9988g = 147.01456g or 147.0 g CaCl2 1g CaCl2 * 2H2O x (1 mol CaCl2 *2H2O/147g CaCl2 *2H2O) = 0.0068 mol of CaCl2*2H2O Molar mass was then calculated for Na2CO3: Na2 = 22.9898g*2 = 45.9796g
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Heating 2NaHCO3→Na2CO3+CO2+H2O a) Experimental results i) Trial 1 Mass of NaHCO3 | 0.3g | Temperature of hot plate | 400 ˚C | Time interval | 10 min. | Mass of mini beaker and product (Na2CO3) | 31.3g | Mass of mini beaker | 31.21g | Final mass of Na2CO3 | 0.09g | ii) Trial 2 Mass of NaHCO3 | 0.3g | Temperature of hot plate | 400 ˚C | Time interval | 10 min. | Mass of mini beaker and product (Na2CO3) | 31.52g | Mass of mini beaker | 31.31g | Final mass of Na2CO3 | 0.21g |
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2(0.1002±0.0002)(0.999)(0.04050±0.00005)(105.99)=0.0467±0.0012 AverageMHCl= 0.0424 ±0.0114+ 0.0420 ±0.0113+ (0.0467 ±0.0112)3=0.0437 ±0.0009 %Na2CO3=(Ave. MHCl)(Vph)(MW Na2CO3)g samplex100% %Na2CO3(1)=(0.0437)(0.004 ±0.00005)(105.99)0.0998 ± 0.0002x100%= 18.56 %± 0.0127% %Na2CO3(2)=(0.0437)(0.0041 ±0.00005)(105.99)0.0998 ± 0.0002x100%= 19.06 %± 0.0122% %Na2CO3(3)=(0.0437)(0.003 ±0.00005)(105.99)0.1002 ± 0.0002x100%= 13.87 %± 0.0167% %NaHCO3(3)=0.0437[0.00980±0.0005-(0.0030±0.00005)](105.99)0.1002±0
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