Analysis of Soda Ash and Volumetric Analysis of a Carbonate-Bicarbonate Mixture Belardo‚ Pia Jobelle J. Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas España‚ Manila 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
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solution in the volumetric flask to finally prepare an acidic KHP solution. The molar mass of KHP was calculated and came to be 208.252 grams per mole. To find the moles of KHP‚ the mass of KHP (1.980 g) was divided by the molar mass of KHP ( 208.252 g) and .00951 moles are in the 1.980 grams of KHP. To find the molarity‚ the number of moles of KHP (.00951 moles) was divided by the volume of water in liters (.100 L) giving an answer of 0.0951 M. The second part of the experiment is the reaction
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2KI 2K(NO3)+ PbI2 1 mole of Pb(NO3)2 react with 2 moles of KI. Molecular mass of Pb(NO3)2: 207.19 + (14.01+16x3)x2 = 331.21m.m.u. Molecular mass of KI: 39.10+126.90 = 166m.m.u. Number of moles of Pb(NO3)2: 1.01g/331.21m.m.u. = 0.00305 mol (rounded). Number of moles of KI: 0.8g/166m.m.u. = 0.0048 mol (rounded). There is only 0.0048 moles of KI‚ therefore the limiting reagent is KI. Molecular mass of PbI2: 207.19 + 126.90x2 = 460.99m.m.u. Number of moles of PbI2:
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than the normal saline. Results: 1. Determine the molar mass of NaCl. Show the workup. Na= 23g/mole Cl= 35g/mole Molar mass of NaCl 23g/mole+35g/mole= 58g/mole 2. Determine the molarity of the two solutions you prepared in terms of NaCl. Show the workup. Normal Saline M=Mole/L of NaCl Mass= .9g NaCl .9g=1mole/58g= .015 moles/L Nasal Irrigation Saline M=Mole/L 1.23g=1mole NaCl/58g= 71.34 moles/L 3. The University of Wisconsin recommends that if stinging or burning occurs‚ than individuals
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Data collection Quantitative Data Raw Data Table 1: Table showing the mass of the amount of unknown acid X measured in grams (±0.001g) Table 2: Table of reading of the burette initially filled with 25mL of 0.201moldm-3 sodium hydroxide (NaOH) to titrate 25mL (±0.03mL) of unknown acid X in mL (±0.05mL) after each titre. Reading on the burette initially filled with 25mL of 0.201moldm-3 NaOH (±0.05mL) First titre 21.3 Second titre 18.2 Third titre 15.2 Fourth titre 12.0 Qualitative
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We will have one species conservation equation (IC.6.15) for each of CH4‚ O2‚ N2‚ CO2 and H2O concentrations and one equation for temperature. All of these equations use fuel consumption rate which is in the following form (from table 5.1): ⎛ mole ⎞ & {ω F }n = { .3E8 × exp(−24358 / T ) × [CH 4]−0.3 [O 2]1.3 }n ⎜ 1 ⎟ ⎝ cc. sec ⎠ Where “n” indicates the time‐step number. Assuming zero heat transfer to the reactor‚ the temperature equation is: & ⎧ − ∑ (h f ‚i + c p ‚i (T − Tref
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reaction: 2HCl(g) ⇄ H2(g) + Cl2(g) is 0.0213 at 400 oC. If 20.0 moles of HCl(g) are heated at 400 oC‚ what amounts of HCl(g)‚ H2(g) and Cl2(g) would be present in the equilibrium mixture? (H2 = Cl2 = 2.26 moles; HCl = 15.48 moles) 3. The equilibrium constant Kc for the reaction: 2CO(g) + O2(g) ⇄ 2CO2(g) is 2.24 x 1022 at 1273oC. Calculate the Kp for the reaction at the same temperature. (1.76 x 1020) 4. A 2.50 mole sample of NOCl was placed in a 1.50-L container at 400oC. When equilibrium
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property which could be monitored in order to measure the rate of reaction. ("a" is done as an example.) a) 3H2(g) + N2(g) 2NH3(g) Pressure will decrease as reaction proceeds because you are going from 4 moles of reactants to 2 moles of products. Assuming you have a constant volume‚ less moles exert less pressure. b) CaCO3(s) CaO(s) + CO2(g) Two things could be monitored here. Look at the states of everything carefully. c) 2NO2(g) N2O4(g) brown colourless Two things could be monitored
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GRAVIMETRIC ANALYSIS OF A CHLORIDE SALT Report Submitted by: Ronald Milner Laboratory partner: Kiesha Mantik Lab Performed: February 16th‚ 2012 Group: Thursday Afternoon‚ Group F Date submitted: March 14th‚ 2012 Purpose: To determine the chloride content of an unknown soluble salt while illustrating the techniques involved in gravimetric analysis. Theory: In order to find the chloride content of an unknown soluble salt‚ that chloride can first be extracted from the
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react together: They must collide with each other The collisions must have enough energy The independent variable in this particular reaction is the concentration of the hydrochloric acid. Each time the concentration will be increased by 0.25 moles. This will ensure that our readings are close and help when working out the rate of reaction. So that it will be easier to make comparisons. The dependent variable will be the volume of hydrogen gas produced and this will be measured using the inverted
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