Abstract: Voltommetric Behavior was examined in two different environments: unstirred and stirred. It was confirmed that a stirred solution of electrolytes produces a more stable and efficient current in a voltaic cell. This was concluded due to the average current of the unstirred solution being 8.9265*10-6A which is 3.8435*10-6A less than that of the stirred solution that was 1.277*10-5A. The Randles-Sevcik behavior helped to conclude this and then was verified when varying the scan rate while
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bonded by dative coordinate bonds from the oxygen atom of the water. Therefore‚ Water of crystallization is water that is stoichiometrically bound into a crystal. Crystal salts containing water of crystallization are called hydrates. * Eg. CuSO4·5H2O cyrstals (copper(II) sulfate pentahydrate) Hypothesis In the hydrate copper (II) sulfate one mole of salt is believed to be combined with five moles of water. Bearing this in mind the following hypothesis was made: If the hydrate is heated
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Zn + CuSo4 mol ratio | Observations | .01/.09 | Clear‚ light gray zinc | .02/.08 | Clear‚ medium gray zinc | .03/.07 | Milky‚ dark gray zinc | .04/.06 | Light blue liquid‚ black zinc | .05/.05 | Light/medium blue‚ brown zinc | .06/.04 | Medium blue‚ dark brown zinc | .07/.03 | Dark blue‚ brownish black zinc | .08/.02 | Bright darker blue‚ medium brown zinc | .09/.01 | Bright darker blue‚ lighter brown zinc | Quantitative Data: Group # | Moles Zn | Moles CuSo4 | 3rd Hour
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Qualitative Observations of Double Displacement Reactions Lab Table 1.0 Qualitative Observation of Products Formed |Balanced Chemical Equations |Qualitative Observations | |BaCl2 (aq) + 2NaOH (aq)( BaOH2(aq) + 2NaCl(s) |An aqueous solution formed | | |Precipitate
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measured and weighed. It was found in the experiment that the yield of copper hydroxide in 40%. Introduction: The copper (II) sulphate is then placed in 100 mL of distilled water. Then 20 mL of CuSO4 is measured and placed 100 mL of distilled water. This can later be weighed to determine the mol of CuSO4 and the mol/L concentration. Then this was used to find out 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
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opposite ions that attract to one another. In this lab research‚ I learned that the following reaction will happen: lead nitrate + potassium chromate à potassium nitrate + lead chromate‚ the balanced chemical reaction is: Pb (NO3)2 + K2CrO4 --> 2 KNO3 + PbCrO4 Procedure Materials: - (1) 100ml Beaker - (1) 50 ml(s) of potassium chromate 1M solution - (1) 50 ml of lead (II) nitrate 1M - (1) 250 mL Erlenmeyer flask - (1) Buchner funnel - (1) Test tube Procedure: 1. Gather required
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A: Ba(NO3)2 B: AgNO3 C: CuSO4 D) CuCl2 E) KCl Description how to identify solution: _ We have two blue solution which are CuSO4 and CuCl2 or C and D‚ according to chemical reaction experiment‚ C didn’t have any reaction with other solution like B and D beside A‚ so if we look at the solubility chart‚ SO2- have only one precipitation with Ba2-. So we come to conclusion that C is CuSO4 and A is Ba(NO3)2 _ So now that we know C is CuSO4‚ other blue solution must be CuCl2
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single-displacement reaction | Fe + CuSO4(aq) --> FeSO4 + Cu | 5. PbSO4 (milk white) | double-displacement reaction | Pb(NO3 )2(aq) + H2SO4(aq) --> PbSO4 + 2HNO3 | 6. CaCO3 (s) appears to dissolve and lot of bubbles comes off out of container. | double-displacement reaction | CaCO3 (s) + 2 HCl(aq) --> CaCl2(aq) + CO2(g) + H2O(l) | 7. When copper sulfate hydrate was heated‚ we can see some white precipitate. | decomposition reactions | CuSO4·5H2O(s) → CuSO4(s) + 5H2O(g) | 8. Red
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Formula of a Hydrate Lab Wednesday October 29‚ 2014 Chemistry Honors Purpose This lab was done to determine the percentage of water in a hydrate‚ which was CuSO4 ?H20. Not only the percentage of water can be found‚ the moles of water can be found per one mole of anhydrous salt. An anhydrous salt is a hydrate that lost its water. Using various lab equipment such as burners‚ crucible‚ and balance‚ and techniques such as the mass-to-mole ratio and mass to percentage‚ the percentage of water in a hydrate
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|the MgCl was added | | | | |(+) There is a black tint to|(+) there was black spotting|(-) no reaction |(-) no reaction | |CuSO4 |the Zinc and the edges are |on the magnesium and the | |
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