how many mL of 0.5 NaOH solution is needed to react completely with all the copper (II) sulphate in solution. Then titrate ¼ of the estimated amount number of mL of NaOH needed to react with the sulphate solution. Then add 5 mL at a time NaOH until Cu(OH)2 precipitate does not form. Record the correct number off mL which forms to NaOH solution. Fold the filter paper and stick inside the funnel‚ and pour the solution of copper (II) hydroxide through the filter. The purpose of this experiment is to
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Question 1 (Limiting Reagent) 15.00 g aluminum sulfide & 10.00 g water react until the limiting reagent is used up. [Atomic mass: H = 1.008‚ Al = 26.98‚ S = 32.07‚ O = 16.00] Here is the balanced equation for the reaction: Al2S3 + 6 H2O ( 2 Al (OH)3 + 3 H2S (i) Which of the two reactants is the limiting reagent? (ii) What is the maximum mass of H2S which can be formed from these reagents? (iii) How much excess reagent remains after the reaction is complete
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BEAN BAG ISOTOPES:ABUNDANCE AND ATOMIC MASS LAB Prelab A new atomic theory‚ in which all atoms of the same element are identical to one another and equal in mass‚ was proposed by the scientist Dalton. Although the theory had its flaws and was simple‚ it was revolutionary. Scientists became able to study the actual structure and mass of atoms after the discovery of radioactivity. Soon‚ isotopes were discovered‚ as atoms of the same element which have been built up to have different masses. Purpose
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How effective were the Vietcong tactics of underground tunnels and booby traps in the Vietnam War? The Vietnam War was a war that started during the late 1950s and ended during the late 1970s. The Vietnam War ended in the Vietcong victory over America. I believe that this was due to the underground ‘labyrinth’ of tunnels and the vast usage of guerrilla warfare used by the Vietcong. Their usage of the tunnels and booby traps were in my opinion ingenious. The variety of the booby traps that were
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following from strongest oxidizing agent to weakest oxidizing agent: Ce4+ Ce3+ Fe2+ Fe3+ Mg2+ Mg Ni2+ Sn 17.3: Cell Potential and Equilibrium ∆G=-nFEº Example: Using the data in table 17.1‚ calculate ∆Gº for the reaction: Cu2+ (aq) + Fe(s) Cu(s) + Fe2+ (aq) 17.4: The Nernst Equation What happens when concentration and temperatures are not standard? Nernst Equation Sometimes written as: Assuming 25ºC Example 1: What is
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Test Dilute HCl Dilute NaOH Mg Silver N/A N/A Non soluble Bubbles Basic Hot/fizz N/A Cu Copper N/A Purple then turned black Non soluble N/A N/A N/A N/A Zn Silver N/A N/A Non Soluble N/A N/A Vaporized and fizzed N/A MgO White N/A Omits gas Hazy mix Boiled Rapidly Basic Got hot and fizzed Became thick or pasty CuCO3 Green N/A Turned black Hazy Green Became powdery Basic Dissolved and vaporized Turned blue and dissolved Cu(NO3)2 Blue N/A Turned green‚ became liquid Dissolved Boiled rapidly Acidic Turned
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water | .2 grams | Formula of anhydrous salt | Cu(SO4) – Copper Sulfate | Data Table Calculations 1. Mass of hydrate = 1.38 grams. Mass of anhydrous = 1.08 grams. Mass of water = .2 grams. 2. Ratio of anhydrous mass to hydrate mass is 5.4. 3. Moles of anhydrous salt: 1. 4. Moles of water are five moles. 5. Moles of water per mole of anhydrous salt was about 5.4/1 ratio but really is 5/1 6. Empirical formula for hydrate is Cu(SO4) * 5H2O Conclusion The mass of the anhydrous
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Multicomponent Phase Diagrams: Applications for Commercial Aluminium Alloys. Figure 1 Nikolay A. Belov‚ 2005. Multicomponent Phase Diagrams: Applications for Commercial Aluminium Alloys. The alloy is strengthened by the precipitation of hardening Mg and Cu rich phases‚ during ageing heat treatment. As a result the material can be up to 30% stronger‚ when the copper crystals are kept small forcing them to conform to the structure of the aluminium. Silicon is an influential element in the composition
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effect of concentration and temperature changes on equilibrium. 2. To predict the direction of the net reaction in an equilibrium system by Le Chatelier’s principle. Results: Part 1 (a): Effect of temperature changes on equilibrium Cu(NO3)2 (aq) Cu(NO3)2 (s) The color of the solution = dark blue with precipitate When placed in water bath 60oC When placed in ice bath The level of the solid Decreases Increases Color of the solution Dark blue with precipitate
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So‚ Pei and co-workers (Pei et al.‚ 2009) found that Cu increases CIP sorption on mineral components kaolinite and montmorillonite in a certain pH range‚ but Ross and Riley (Ross and Riley‚ 1992) showed that Cu increases the mobility and solubility of fluoroquinolones (Chen et al.‚ 2013). Although sediments 5 and 6 have the highest concentration of certain affordable microelements (Cu‚ Fe‚ Zn and Mn) show the lowest sorption potential to CIP‚ this contribution to sorption
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