equation for it. Then using the A‚ B symbols‚ write a general equation for a single-displacement reaction. Here are the chemical formulas of the reactants for each reaction: • zinc – Zn copper sulfate – CuSO4 • aluminum – Al copper sulfate – CuSO4 • zinc – Zn silver nitrate – Ag(NO3) • copper – Cu silver nitrate – Ag(NO3) Answer: (8 points) |Score | | | 2. For Part 3: Double-Displacement Reactions:
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empirical formula of the hydrate and its percentage by mass of water. Hypothesis: If the hydrated form of CuSO4 is heated then it will remove the water turning it to the anhydrous form then it will change from blue to white. Materials: * Balance * Crucible and Cover * Crucible and tongs * Distilled water * Spatula * Stirring rod‚ glass * Bunsen burner * CuSO4‚ hydrate crystals * Desiccator gauze * Dropper or micropet * Ring Stand * Ring and pipe-stem
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solution of 7.25 M MgCl2 from 4.89 moles of MgCl2? (A: 0.674 L) 6. What is the molarity of a solution prepared by adding 58.5 g of NaCl to 230 ml of H2O? (A: 4.3 M NaCl) 7. What is the molarity of a KNO3 solution prepared by adding 151.5g of KNO3 to 300ml of H2O? (A: 5.00 M KNO3) 8. How many grams of NaOH are required to prepare 2.0 liters of 2.5 M NaOH solution in water? (A: 200g NaOH) 9. What is the molarity of a soltuion prepared by dissolving 5.68 g of NaOH in enough water
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Mike Morrison – SCH3U Types of Chemical Reactions Lab Intro/Purpose The purpose of this lab is to determine types of reactions with only the reactants and through observation. Through observing the experiments‚ one is able to see a visual of each type of reaction taking place and it gives them a better understanding of how chemical reactions work and what products they may form. Materials & Procedure Materials: * Wood Splints - Copper Sulfate * Sodium Sulfate - Copper
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calculations. Data: |Mass of Empty Beaker(g) | | |Mass of Beaker & CuSO4 . nH2O (g) | | |Mass of Beaker and CuSO4 (g) | | Calculations: You must show all work for complete credit. Determine
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The Dehydration of a Bluestone February.28.2008 Purpose • To determine the value of X in CuSO4 • xH2O. Materials • Crucible • Blue Stone • Bunsen Burner • Bunsen Lighter • Test Tube • Water • Rheostat • Clay Triangle • Electronic Balance Procedure A clean crucible was taken and weighed on an electronic balance. The mass was then written down. 2g of bluestone was placed in the crucible and weighed. The mass of the blue solid was written down. The crucible was placed on a clay
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pentahydrate is CuSO4 · 5 H2O The dot indicates that the molecules of water are attached to the ions in CuSO4 by weak bonds. We can drive off the water of hydration by heating the hydrate. If blue CuSO4 · 5 H2O is heated‚ the water of hydration is released as water vapor‚ and solid white anhydrous CuSO4 remains.
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In this lab‚ we used Bunsen burners to heat up a hydrated salt in order to determine the percentage of water inside of this hydrated salt. We heated up the salt in order to boil off the water‚ which allowed us to find the weight of the CuSO4 by itself. By comparing this final weight with the original weight and subtracting the difference‚ we were able to compile data about how much the weight of the hydrated salt decreased as the water gradually boiled away. In doing so‚ we were able to find the
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(II) Sulfate‚ CuSO4‚ mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:- CuSO4(aq) + Fe(s)
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ACADEMY Aim The aim of this investigation is to determine the formula of the complex ion formed from copper (II) ions and ammonia through colorimetry. Results Raw Data Table 1: The Effect of CuSO4:NH3 Volume Ratio (cm³) (±0.05) on Absorbance (±0.01) Independent Variable: Volume (cm³) (±0.05) CuSO4 NH3 0.00 0.00 1.00 9.00 1.50 8.50 2.00 8.00 2.50 7.50 3.00 7.00 4.00 6.00 5.00 5.00 Dependent Variable: Absorbance (±0.01) Trial 1 0.00 0.14 0.22 0.23 0.10 0.10 0.09
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