Let’s experiment and observe Whether these ions will have a reaction or indeed soluble in water. Experimental Procedure Let’s begin this experiment by obtaining a 100ml beaker from our equipment tool bar list, then we are going to add 50ml(s) of Potassium Chromate 1M solution to that beaker, The next step we are going to add another ionic compound of 50ml of Lead (11) nitrate 1M into the same beaker as the Potassium Chromate. As we observe the beaker, we notice a reaction has occurred and a precipitate has formed and settled on the bottom of the beaker. The next step is we are going to filter the resulting precipitate into a 250 ml Erlenmeyer Flask with a Buchner funnel. Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight.
This colour can be used to determine which ion is being burnt as each ion emits a certain specific combination of wavelengths which correspond to specific colours. Variables: Independent Variable: Metal Salt Dependent Variable: Colour of the flame Controlled Variable: Quantity of the metal salt taken. Apparatus: * Safety goggles * Latex gloves * Nichrome wire * Bunsen burner * Hydrochloric acid * Wash bottle(with distilled water) * some metal salts > sodium chloride > sodium carbonate > sodium sulphate > lithium chloride > potassium chloride > potassium sulphate > strontium chloride > calcium sulphate > calcium carbonate > calcium chloride > copper carbonate > copper chloride * Spectroscope * Cobalt glass Safety Precautions:- * Safety goggles and latex gloves must be worn. * Hydrochloric acid is corrosive and can cause severe injury. If you spill acid on yourself, immediately flush the affected area with water for 2-3 minutes and notify the teacher.
We are looking to find wether the reaction is exothermic or endothermic. Experiment 2: the aim for this experiment is to record the pH level of a sodium hydroxide and hydrochloric acid reaction. Then record it into the graph, it should resemble the standard neutralization curve, as shown under the introduction. Materials: what you will need for both experiments: Experiment 1: ➢ 20g baking soda ➢ 20g citric acid ➢ 2 cm strip of magnesium ➢ 50 ml of 5M HCl acid ➢ 50 ml measuring cylinder ➢
Introduction A titration was carried out in this experiment to find the concentration of hydrochloric acid is an unknown solution. The aim of this experiment is to determine the number of moles of sodium hydroxide in hydrochloric acid and then to determine the number of moles of sodium hydroxide present in gastric juices. Titration, or volumetric analysis, is a common laboratory procedure for the analysis of substances and solutions. In a titration, the analyst determines the volume of a solution, called a titrant, that reacts exactly with a known weight or volume of another substance. This reaction is carried out by adding a solution of reactant hydrochloric acid from a burette to a solution of sodium hydroxide until just sufficient of hydrochloric acid has been added to react with all of the sodium hydroxide.
Chemical Bonding, structure and Quantity Aim To investigating a range of compound which include metallic, covalent molecular, covalent giant and ionic giant Materials used and list of apparatus Google Bunsen burner Test tube Power supply Spatula Tongs Mats Method To discover the characteristic physical properties of the substances six tests were done. These were tests of appearance, melting point, conductivity of solid, solubility in water, conductivity of solution and hardness. Test 1: Appearance. This was to note whether the substance was shiny, dull, with colour etc. Test 2: Melting point.
Also, the chromium in chromite may sometimes be replaced by aluminum and ferrous ions. Hydrometallurgy is a way to separate the different elements making up ores and isolate the metals from each other. In order for this to occur, the ore must be melted down into a solution. After the metals of the ore have been dissolved, they may be separated from each other by many different processes, some of the most popular are leaching and precipitating the metal from the solution via electrolysis or chemical means. In this experiment the team of students must determine exactly what is in chromite sample, and also confirm the existence of all such metals that should be in the sample of chromite.
These impurities include vanadium, arsenic, zirconium, iron, silicon, and magnesium. Therefore, impure titanium tetrachloride is then cleaned of all these impurities for the purpose of gaining a pure titanium tetrachloride. The cleaning process is initiated by allowing the former mixture to settle, where the undissolved particles are removed as dirt or mud. Afterwards, the liquid that contains several chlorides is passed through a distillation column and is chemically treated with hydrogen sulfide or mineral oil to eliminate vanadium oxychloride, which is a chloride that boils at the same temperature as titanium tetrachloride. Finally, it is redistilled again to further purify the titanium tetrachloride produced.
TITRATION OF SULPHURIC ACID WITH SODIUM HYDROXIDE Modified: November 3, 2002 INTRODUCTION A TITRATION is a process in which a measured amount of a solution is reacted with a known volume of another solution (one of the solutions has an unknown concentration) until a desired end point is reached. (The “end point” of a titration is the point in the titration at which an indicator dye just changes colour to signal the stopping point of the titration.) In this experiment, you will use a PIPETTE to measure some sulphuric acid into a beaker. The sulphuric acid has an unknown concentration. Then you will fill a BURETTE with sodium hydroxide (a base) that has a known concentration.
Clean the nichrome wire by dipping it into the acid and heating the loop to get rid of any excess chemicals. Dip the wire into one of the sample solutions and place into the hottest part of the flame. Repeat the dip into the salt solution if necessary to see the flame test colour. Write the colour of each metal salt when it is put into the flame into a results table. Repeat this procedure with the other known solutions to record the
About 3mL of the wash water is collected in a small test tube. A few drops of 0.1M silver nitrate solution is added to the water to test for the presences of Cl- ions. Lastly the filter paper was placed in the dry oven to dry completely and then weighted. Calculations and observations were made and recorded. Observations The