Copper sulphate solution

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 is sufficiently washed

compounds (sulphates) were combined, they will react according to the Activity Series of metals. In our experiment we hypothesized that when magnesium metal and copper sulphate combines, it will produce an aqueous solution of magnesium sulphate and copper metal. When zinc metal and iron sulphate are combined, an aqueous solution of zinc sulphate and iron metal is produced. When iron and tin chloride are combined, iron chloride and tin are formed. When tin is combined with copper sulphate, an aqueous

Determining an enthalpy change of a displacement reaction Aim: To determine the enthalpy change for the displacement reaction between zinc powder and copper (II) sulphate solution. Zn (s) + Cu2+ (aq) → Cu2+ (s) + Zn2+ (aq) Theory: For the displacement reaction, an excess amount of zinc powder is added to the measured amount of aqueous copper (II) sulphate. The temperature change over a period of time has to be measured and thus, the enthalpy change for the reaction can be measured. The equation of

variable was controlled 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

Chemistry Title: voltaic cell experiment a voltaic cell is a device made from connecting two different metals together and immersing the combined piece into some sort of solution that creates conductive atmosphere , the general purpose of a voltaic cell is to convert the chemical reaction between the metals and the solution into an electrical charge , Hypothesis: the voltage produced by magnesium and cupper = the sum of the voltage produced by magnasium and iron ; and iron and cupper Variables:

electrochemical cell, invented in 1836 by a British chemist, Frederic Daniel. The cell produces electricity through a redox reaction. The combined electric potentials of two metals in the metal sulphate solution of the electrolyte generate voltage. If the concentration of one of the electrolyte solutions is increased, the number of cations and anions increase (depending on which electrolyte you increase), which increases the overall voltage potential of the cell. Equilibrium conditions are not achieved

Will it Precipitate? Precipitation occurs when two aqueous (soluble solids) solutions are combined and the reaction forms an insoluble solid. When insoluble solids are formed the process is known as a precipitation. An insoluble solid is a solid that cannot dissolve unlike a soluble solid. Therefore only insoluble solids can form precipitates. In the following experiment six solutions were mixed with each other (groups of twos) in test tubes to test which reaction will result in an insoluble solid

To find the molecular formula of a certain hydrate of Copper (II) Sulphate, CuSO4, XH2O Apparatus • Ceramic Evaporating Dish • Electronic Balance • Bunsen burner • Clay Triangle • Glass stirring rod • Spatula • Crucible tongs • Copper (II) Sulphate hydrate crystals Method 1. Before doing the whole experiment, make sure that you weigh: • The evaporating dish • The evaporating dish + the hydrate • The evaporating dish + the anhydrous solution (this is after the experiment, don’t worry about it now)

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

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