Indigo Synthesis Author: Carolina Morales Group #1 Lab Partners: Jennifer Capeloto‚ Samantha Hoffman and Adriana Garibay Instructor: Saehan Park Chem. 152‚ Section 43 Date Work Performed: February 10‚ 2010 Date Work Submitted: February 24‚ 2010 Abstract: The percent yield of the color Indigo that is the color of blue jeans for the three trials was determined to be 13.50%‚ 15.30% and 14.80%. A series of experiments were performed to a cloth dye comparison. The absorbance
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sodium carbonate and 1.00 g of lead II nitrate was given to start the lab out with. To calculate the percent yield of lead II carbonate‚ the limiting reactant must be identified first. 1.00 g Na2CO3 x 1 mole106 g = 0.00943 mole Na2CO3 1.00 g Pb(NO3)2 x 1 mole331 g = .00302 mole Pb(NO3)2 Limiting reactant: lead II nitrate Next‚ the theoretical yield of lead II
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Introduction: The objective of this experiment is to utilize the techniques of weighing and titrating to determine the total amount of MgSO4 present in an unknown sample. Standardized EDTA will be used to titrate the unknown solution. This type of reaction is a complexation reaction‚ which usually involves Lewis acids and bases. EDTA in complexation reactions serves as a chelating ligand. The base‚ EDTA‚ will bind to the metal ions‚ which serve as the Lewis acid‚ thus playing a role as a ligand
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WORKSHEET MOLE By Sir Shah Murtaza Q1. Potassium reacts with water as shown in the equation. a. Describe what you would see when potassium reacts with water. b. A sample of 0.195 g of potassium was added to 500 cm3 of cold water. When the reaction was finished‚ 100 cm3 of 0.100mol/dm3 hydrochloric acid was added to form solution X. (i) Calculate the number of moles of hydroxide ions formed when the potassium was added to water. (ii) Calculate the
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large quantity of solute in a given amount of solvent. Dilute solutions contain relatively little solute in a given amount of solvent. There are two specifics term to express concentration‚ which molarity and percent by mass. Molarity is the number of moles of solute per liter of solution. Percent by mass is the mass in grams of solute per 100 grams of solution. Vinegar is a dilute solution of acetic acid. The molecular formula for acetic acid is CH3COOH. Both molarity and percent by mass of acetic
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the volume of one mole of hydrogen gas at STP (standard temperature and pressure). In the experiment‚ a magnesium ribbon was placed at the bottom of an eudiometer tube and allowed to react with 2M hydrochloric acid. The volume of hydrochloric displacement was measured and calculations determined the molar volume of hydrogen gas produced inside the eudiometer tube. After performing and taking the average data of two trials‚ it was concluded that the calculated value of one mole of hydrogen gas at
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CHAPTER 4 REVISION 1. How many moles of silver atoms are in 0.780 grams of silver? a) 0.78 moles b) 0.00723 moles c) 84.2 moles d) 0.522 moles 2. What is the molar mass of Mg(BrO4)2? a) 312 g mol-1 b) 232 g mol-1 c) 168.2 g mol-1 d) 477 g mol-1 3. What mass of the compound FeWO4 contains 50.0 grams of tungsten (atomic symbol W‚ atomic number = 74)? a) 30.0 g FeWO4 b) 304 g FeWO4 c) 82.6 g FeWO4 d) 188 g FeWO4 d) FeSO4 4. A compound contains 20.2%
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of moles and grams of urea and the amount of urea used originally used in the experiment‚ so the ammonium chloride will be primarily compared to the corrected amount of urea to make sure that the amount of solvent is equal. Graph 1 and 5 and Data Table 2 show that the mass of solutes were overall very similar: 8.735 grams of ammonium chloride and 8.99 grams of urea. Overall‚ this experiment proved that the freezing point depression is a colligative property that depends on the number of moles of
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12. The salt solution will turn into salt crystals when it is heated. NaOH + HCl = NaCl + H2O NaOH + HNO3 = NaNO3 NaOH + H2SO4 = Na2SO4 + 2H2O Observations: Alkali | Acid | Moles | Observation | NaOH | HCL | 1 Mole | Took 4 ml to neutralize. No further experiment was made. | NaOH | HCL | 0.1 Mole | Took 31 ml to neutralize. 2.30 minutes until pink salt crystals were formed. | NaOH | HNO3 | 1
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Factors Affecting Reactions I. Factors Affecting Reactions [545] • Every chemical proceeds at its own rate. • By changing the conditions of the reaction‚ the rate of almost any reaction can be modified. • The rate of a chemical reaction depends upon: o Temperature o Concentration o Particle Size[SA] o Catalyst A. Temperature [545] • Increasing the temperature causes molecules to move faster‚ so there’s an increased chance of them colliding
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