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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distillation Two liquids – immiscible liquids using a separating funnel - fractional distillation due to different boiling points H/W – P.18 Qu. 11-18 Identifying Pure Substances Colour – some substances have a characteristic colour‚ eg CuSO4 = blue. We can use this knowledge in a qualitative way to determine if a sample has impurities. Melting & Boiling Point – The mp & bp of a substance is a good indicator of its purity. A pure substance will have a sharp melting point and its mp &
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Chemistry F332 Notes Ions in solids and solutions: Structure of an ionic lattice (Sodium Chloride): * Consists of sodium ions (Na+) surrounded by six chloride ions (Cl-) * Chloride ions also surrounded by six sodium ions. * Held together by attraction of oppositely charged ions. * Giant ionic lattice. * Electrostatic bonds hold lattices together. * Structure is simple cubic. * Some ionic crystals contain water. * Known as water of crystallisation. * These crystals
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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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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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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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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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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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