Copper sulphate

Materials: Metals: • 15 pieces of Cu(s) (copper) • 7 pieces of Mg(s) (magnesium) • 7 pieces of Zn(s) (zinc) Solutions: • H2O(l) distilled water • HCl(aq) hydrochloric acid • CuSO4(aq) copper (II) sulphate • ZnSO4(aq) zinc sulphate • MgSO4(aq) magnesium sulphate • SnCl2(aq) tin (II) chloride • ZnSO4(aq) zinc sulphate • FeSO4(aq) iron (II) sulphate • • Tweezers • Two Spot Plates • Distilled Water Bottle • Safety Glasses • 1 piece of paper • Pen / Pencil Procedure: 1. Gathered all the required

Introduction By using a spectrophotometer, we were able to measure the absorbance of Copper (II) sulphate with increasing dilutions. From this we were able to create a graph showing the concentration as well as the absorbance. The Beer Lambert Law is the linear relationship between the absorbance and concentration. This has a connection with the light behaviour as well because light behaviour effects the concentration and absorbance. The more concentrated that a solution is, the less light passes

Determining the amount of Water of Crystallization Hydrated to Copper Sulphate Daniel Benda October 11th 2014 Hl Chemistry Block: H Word Count: 1354   Data Collection and Processing: Raw Data: Table 1: Raw data of Trials vs Mass of crucible and contents before and after heating Trials Empty mass of crucible (±0.001g) Initial filled mass of crucible (±0.001g) Final Filled weight of crucible (±0.001g) T1 36.093 43.516 40.783 T2 48.160 56.218 53.143 T3 31.503 44.537 39.705 T4 34.345 38.677 37.082

sample of copper sulphate using colorimetry. In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate

solubility of my solutes. My decided solutes are sugar, salt and copper sulphate pentahydrate. I decided I would be using 100mL of water as my solvent due to the abundance of solutes available and that fact that 100mL is a nice, easy number to work with. I also spoke to Mrs Rach and she informed me she has a surplus of copper sulphate so I don’t have to be careful with how much I use. She also gave me some measurements on how much copper sulphate should dissolve into 100mL of water at varying degrees. It’s

Task 7:  Titrations: Method: 1. Firstly you need to need to measure accurately 0.50g of your copper sulphate solution into a 100cm³ beaker 2. Then add about 50cm³ of distilled water ensuring you continue to stir until crystals have dissolved. Then transfer the solution into a 100cm³ volumetric flask 3. Next rinse out the beaker with small amounts of distilled water and transfer the washings to the volumetric flask to ensure none of the solution is wasted affecting the end result. 4. Once the beaker

Concentration of the acid The denser the solution, the slower the reaction. The slower the reaction, the less copper is deposited in the given time period. Everyone used the same amount of copper sulphate solution Current passed through the circuit If it wasn’t constant then the time, intervals wouldn’t be equal. If the current is larger, there will be more electrons flowing around the circuit and more copper will be deposited. The use of a ammeter tells you the current stayed constant Power Supply Effects

Completion Date: Introduction We are studying the reaction between zinc and sulphuric acid, the reaction is catalysed by copper sulphate and this experiment is to test whether the amount of drops effect the rate of reaction. Word Equation Zinc(s) + Sulphuric acid(aq) à Hydrogen(g) + Zinc Sulphate(aq) Symbol Equation Zn + H2SO4 à H + ZnSO4 This reaction is catalysed by Copper sulphate (CuSO4) Ionic Equation - Cancel Spectator ion (SO42-) Zn + 2H+ à Zn2+ + H2 For this reaction to work there must

Copper is one of the most used metals in the world. Copper or Cu has an atomic number of 29 and an atomic mass of 63.546. It has 29 protons, 29 electrons and has two stable isotopes Cu63 and Cu65. Copper is one of the most used metals since ancient times. It is estimate that copper was first discovered in the year 8,000 B.C by men and was one of the first metals discovered by men. Copper can be found in nature as a pure element and that is why it was one of the first metals to be worked on. Research

In the lab, copper underwent a process of reactions that lead the chemical to change into a multitude of forms. Furthermore, the copper shifted its state quite a few time, initially as a solid rod, to gelatinous form, and even liquid. In this lab, common techniques were applied such as decanting, measuring in with an analytical balance and filtration. the attempt on recovering the original mass of solid copper was a failure as our percent recovery was 252.35%. The initial mass that was weighted