Investigate the Rate of Electroplating a Met

In the hood, place the copper wire in 10mL of nitric acid and wait for it to dissolve. Afterwards, add 100mL of deionized water to the solution and boil the solution, so all the nitrogen oxides are removed. Place the solution to a 250.0mL volumetric flask and add deionized water to the flask until the solution is 250.0mL. When the solution in the flask is at 250.0mL place the solution in a clean plastic bottle. Now cut a penny into four pieces, and measure the mass of all the pieces together. Go back to the hood, and place the pieces of the penny into a 250mL beaker. Afterwards, add 20mL of concentrated hydrochloric acid. Wait for the hydrochloric acid to dissolve the zinc core. When the zinc has dissolved, filter the solution through the filter paper, and place the copper metal pieces into a clean 150mL beaker. In the hood, place 4mL of concentrated nitric acid in the beaker, and when the copper dissolves add, one drop at a time, 30mL of 6 M ammonium hydroxide to neutralize the nitric acid. Transfer the copper/ammonia solution to a 100.00mL volumetric flask. Prepare four different calibration

The content of this section depends to a large extend on the nature of the experiment. Topics here should include a section labelled:

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 crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

Then in the last test tube fill it up with 5ml of sodium sulphate. Then after that carefully pour the sodium carbonate solution into the test tube labelled copper chloride solution examining the result and recording appropriately.

The materials needed for this experiment included test tubes, a test tube holder, the unknown compound #202, 35mL beakers, gloves, safety goggles, ethanol (to clean equipment), stirrer (to mix solutions), the 15 possible compounds that are provided, pH strips, distilled water, wooden splints, spatula to get out unknown compound #202, waste bucket, Bunsen burner, graduated cylinder, 500mL beaker for the waste, plastic dishes to measure out compound and the scale.

This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor.

The first experiment begun by filling a 600-ml beaker, almost to the top, with water. Next, a 10-ml graduated cylinder was filled to the top with water. Once water was added to the beaker and graduated cylinder, a thumb was placed over the top of the graduated cylinder. This would ensure that no water was let out and no bubbles were let into the graduated cylinder. Next, it was turned upside down and fully submerged into the beaker. Then, a U-shaped glass tube was attained. The short end of the glass tube was placed into the beaker with the tip inside of the graduated cylinder. Next, a 50-ml Erlenmeyer flask was received. After, 10-ml of substrate concentration and 10-ml of catalase/buffer solution were placed into the flask. A rubber stopper was then placed on the opening of the flask. After adding these, the flask was held at the neck and spun softly

Students: These are some hints about the requirements of a high quality Extended Experimental Investigation for the Queensland Senior Chemistry Syllabus. Guidelines given to you by your teacher should take precedence if there is any doubt. They are addressing a Year 12 EEI but will still guide you for Year 11. They refer to a hypothesis-testing EEI. What’s the purpose of an EEI? You‟ll do an EEI to research a question you have about some chemistry-related phenomena you have come across. In the process you gain a better understanding of the concepts. It does not matter that your experiment has been done a thousand times before or that your teacher already knows the results. What matters is that you don

Problem: How does the electronegativity of 1.25 mol/L of hydrochloric acid, 1.25 mol/L of sulphuric acid, and 1.25 mol/L of nitric acid, affect the rate at which magnesium will react at room temperature(21°C)? Background: A chemical reaction is the rate at which a substance goes through a change and it is transformed into another substance that has different compositions as well as properties.1 The rate at which a chemical reaction occurs depends on many factors, some of which include the concentration of a reactant2, temperature2, collision theory and electronegativity3. Concentration of a reactant effects the rate of reactivity.

First we began by doing an inventory of the supplies in our lab drawer. We then inspected the glassware in the drawer for any cracks or chips. Next we identified

The purpose of the experiment was to identify the concentration of an unknown solution by performing a serial dilution to provide reference for comparison. Serial dilutions are extremely useful for identifying unknown substances as the gradual discolouration of the solution allows for simple comparison. Although serial dilutions are extremely helpful for chemists, they are often used to help microbiologists reliably count the number of bacteria living in a host or an environment. Blodgett states that serial dilutions can help estimate the concentration of target microbes in a sample; this estimation is useful when counting the bacteria for low concentrations of organisms (Blodgett, 2013). Having an estimate of the concentration of bacteria

0.5% of copper sulphate solution was added by drop at a time and and the test tube was shaked continuously.

Electrolysis is the means of breaking down a solution or a liquid compound by having an electric current go through it. Electrolysis is utilized in removing impurities in copper, tin, silver, and gold, and for acquiring sodium, magnesium, aluminum, and other metals derived from their ores. Electroplating is when you utilize electrolysis to cover a metallic item with a slim coating of a different metal. Anodizing is the utilization of electrolysis to cover a metallic item with a slim coating of oxide for conservation against deteriorating and damage. Electrolysis is additionally utilized for the yielding of caustic soda, chlorine, oxygen, hydrogen, and other substances.

Electroplating is a plating process that uses electrical current to reduce cat ions of a desired material from a solution and coat a conductive object with a thin layer of the material, such as a metal. Electroplating is primarily used for depositing a layer of material to bestow a desired property (e.g., abrasion and wear resistance, corrosion protection, lubricity, aesthetic qualities, etc.) to a surface that otherwise lacks that property. Another application uses electroplating to build up thickness on undersized parts.