of moles of toluene = Mass/Mr = 43.35g/(92.15g/mol) = 0.470428648 moles ≈ 0.470 moles Volume of Sulphuric acid = 10mL (10cm3) Density of Sulphuric acid = 1.84g/cm3 Mass of Sulphuric acid = Density x Volume = 1.84g/cm3 x 10cm3 = 18.4g Mr of Sulphuric acid = 98.09g/mol No. of moles of Sulphuric acid = Mass/Mr = 18.4g/(98.09g/mol) = 0.187582832 moles ≈ 0.188 moles Limiting reagent: Sulphuric acid No. of moles of p-Toluenesulphonic acid = 0.188 moles Mr of p-Toluenesulphonic
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this fact and eventually presents him with examples that make up the rest of the chapter. The first key element that this paragraph addresses is Adrian. Throughout the chapter‚ Adrian doesn’t make the smartest choices while traveling on this mountain‚ which brings me back to the opening statement. Obviously‚ the Denali didn’t make a huge impact on Adrian because he dismissed what the Denali was trying to inform him of as he travels up the mountain. Another way that this paragraph addresses is on
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38 grams | Mass of hydrated MgSO4 | 3.00 grams | Mass of crucible‚ lid‚ and anhydrous MgS04 | 12.82 grams | Mass of anhydrous MgSO4 | 1.45 grams | Mass of water in hydrated MgSO4 | 1.55 grams | Moles of anhydrous MgSO4 | 0.0120 moles | Moles of water in hydrated MgSO4 | 0.0860 moles | Observation of anhydrous MgSO4 | Different shade of white‚ more thicker and solid; powder-like | 3. To obtain the mass of water‚ first measure the mass of the crucible with the lid and anhydrous MgSO4
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While sitting on his porch with his friend Adrian‚ Victor says‚ “Hey‚ we don’t drink no more‚ remember? How about a Diet Pepsi?” (Alexie‚ 44). Although they are no longer drinking alcohol‚ the issue of addiction still arises by this statement. Throughout the story there is multiple mentions of Adrian asking “Now when did that thing quit flashing?” (Alexie‚ 44) as in talking specifically the only traffic signal on the reservation
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AP Chemistry Analysis of Alum * Purpose: * In this lab we performed several tests to determine if our crystals were actually aluminum potassium sulfate. * Procedures: * Materials: * Chemicals: * Aluminum potassium sulfate‚ 2.5 g * Equipment – Part 1: * 150 mL beaker * Bunsen burner * 2 capillary tubes * Mortar and pestle * Notched stopper to hold thermometer *
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Marie Alessandra T. Reyes Group 4 18L Quantitative Determination of the Acidity of Soft Drinks I. Introduction Soft drinks are well known beverages among the young that are consumed mostly for pleasure. These beverages normally contain flavoring‚ sweeteners coloring‚ carbonic acid and acids. Carbonic acid and acids play an important part in the formulation of soft drinks. They enhance the flavor and give a pleasant refreshing ’lift ’ to the drink. The type of acid used can even affect the palatability
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Quantities The Mole General‚ Organic‚ and Biological Chemistry Copyright © 2010 Pearson Education‚ Inc. 1 Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans General‚ Organic‚ and Biological Chemistry 2 A Mole of Atoms A mole is a collection that contains the same number of particles as there are carbon atoms in 12.0 g of carbon 12C 6.02 x 1023 atoms of an element (Avogadro’s number) 1 mole of Element
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BSc Pharmaceutical Technology Practical - No 5 Preparation of a Primary Standard Solution Aim: to prepare a standard solution of pure silver nitrate and use it to determine the concentration of chloride ions in a sample of tap water and another sample of bottled water. Chemicals: * High grade purity silver nitrate * Potassium chromate indicator * Tap water * Bottled water * Distilled water Apparatus: * Laboratory oven * Dessicator * Conical flask
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amounts of a substance in terms of moles? The compound I was using in my experiment was NaOH. The first thing I needed to work out was the number of moles I needed. To do this I used the formula: Number of moles = Mass ÷ RFM. The mass is the amount that I weighed on the balance which was 1g. I then worked out the RFM of NaOH which is 40. I next put my mass and the RFM into the formula to find out the number of moles. Number of moles = 1 ÷ 40 Number of moles = 0.025
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number of moles of water molecules per mole of salt. Sample Calculations: Mass of hydrate= 35.232g - 32.005g =3.227g Mass of anhydrous salt= 33.583g - 32.005g =1.581g Mass of water liberated= 35.232g – 33.586g =1.646g Mass of h2O in hydrate= 1.646g/3.227g X 100 = 51% % anhydrous salt in hydrate= 1.581g/3.227g X 100 = 49% Moles of anhydrous salt in 100g hydrate= 49% X 1mol/120.38= 0.407moles Moles of water in 100g of hydrate= 51% X 1mol/18.02= 2.83moles Moles of water per mole of anhydrous
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