Using the 96 well plate I combined various chemicals together to observe the chemical changes that were created. After this step was completed I combined three different household cleaners with bromthymol blue to observe whether the cleaner was an acid or base. After a thorough cleanup of the chemicals and workspace I answered the appropriate questions related to this lab
iLab 1: Separation of a Saltwater Solution Devry University BIOS135 Professor Subbhalakshmi, Dhalladoo 11/01/14 Introduction The purpose of this lab experiment was, to practice using the scientific method and separate a mixture of salt and water based on the physical properties of each component. I will examine more closely the physical properties of matter. To do this procedure we must evaporate the water and leave behind the salt from the solution. In 103c the water evaporates and behind left is the salt. From this information, the percentage of salt verses water ions can be determined Ions are also produced in the liquid or solid state when salts interact with solvents (for example, water) to produce "solvated ions," which are more stable, for reasons involving a combination of energy and entropy changes as the ions move away from each other to interact with the liquid.
Chemistry Lab Types of Chemical Reactions OBSERVATION DATA TABLE Step|Name of Reactants|Description of Reactants|Description of reaction taking place (evidence of chemical reaction)|Description of Products| 1|Zn|Solid, small chunky bits, Silvery-grey, dull|As the Zinc and Sulfur heated up it expanded in the test tube and shot out Zinc Sulfide.-light and heat are produced|White powder was created and the leftovers of the reactions was a black powder.| |S|Solid, resembles powder, Off-yellowOpaque||| 2|KI|-dull yellow liquid-transparent|Instantaneously changed colour to a bright yellow.|-Bright yellow liquid-Opaque| |Pb(NO3)2|-liquid, transparent, very clear-bubbly||| 3|H2O2|-liquid-clear-transparent|A dark grey bubbling liquid was created. It got hotter as it reacted.gas test observations:The splint relit. Oxygen was present.|Oxygen gas was created and a dark grey opaque liquid was left behind in the test tube. | |MnO2|-solid-powder-black||| 4|AgNO3|A clear, transparent liquid.|As the copper reacted with the Silver Nitrate, the ball of Copper changed colour to grey and subsequently developed a ‘furry-like’ characteristic on its coating.|-Clear liquid-Copper changes to a grey colour, ‘furry-like’.| |Cu|-brown/red-solid-stringy||| 5|HCl|A clear, transparent liquid.|When the Magnesium was inserted the HCl liquid started to bubble and fizz releasing Hydrogen. The Magnesium strip dissolved in the process and the test tube got hotter.
Title: Heating Curves and Phase Diagrams Course: Chemistry 1412 – General Chemistry II Objective Activity One: In this experiment, the student will plot a vapor pressure vs. temperature graph and will discuss, interpret, and analyze it. Activity Two: In this experiment, a variety of values will be provided and the student is to recreate a phase diagram and interpret the meanings of the values. Activity Three: In this experiment, the temperature probe with start with a reading temperature that is well below the freezing point, and with that, the graph (Temp vs. Time) will be recorded and observed as time progresses in its natural direction. The Heating Curve will then be analyzed. Materials and Summary of Procedures Activity One: In this experiment you will need a Graphing Calculator and some Paper and Pencils.
When in flame it produces gas rapidly and bubbles. Liquid turns into gas quickly. When liquid disappears solution (now a solid) turns white | 4 | A Initial temperature is 15 degrees Celsius and the final temperature is 17 degrees Celsius. BThe blue hydrated copper sulphate turned white, evidence of condensation of a clear liquid present on the inside of the test tube.C concentrated sulphuric acid turns black on paper towel and is clear on the white cottonD Carbon pillar grows cause of air bubbles, it is brittle, it is both corrosive with a hole and there is evidence of carbon produced | 5 | No temperature change and iodine brown/yellow gas produced | Properties of Sulphuric acid results table Aim: To investigate and observe the properties of sulphuric acid through five different experiments where we will determine its extent of ionisation in aqueous solution, reaction of sulfate ions, action as a strong acid, affinity for water and action as an oxidising agent. Background: Sulfuric acid (H2SO4) is a diprotic acid (can donate 2 protons to a base).
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.
A 125mL Erlenmeyer Flask was used to combine (15mL) of concentrated aqueous ammonia and ammonium chloride (0.0467mol, 2.49g). The mixture was stirred till fully dissolved. Colbalt (II) chloride hexahydrate was ground (6.2g) and added in small amounts to the stirring solution (0.0210mol, 5.2g). As the mixture continued to stir (4mL) of 30% hydrogen peroxide was added drop wise to yield a dark warm slurry. After the effervescence, (15mL) of concentrated HCl was added drop wise to the solution.
4. Chlorine, Cl 2, is a strong oxidizing agent found in bleach. 10.0 cm3 of bleach solution was added to 25.0 cm3 of 0.4M Sn2+ solution acidified with sulphuric acid and made up to 100 cm3. 10.0 cm3 of the resulting solution containing the unreacted Sn2+ was titrated against 0.02M K2Cr2O7. Given that 11.40 cm3 of K2Cr2O7 was required for complete oxidation, a) Calculate the numbers of moles of Cr2O7- used.
* Gloves are to be worn whilst the experiment is in motion. * If an allergic reaction to iodine occurs, notify teacher immediately. Method: Room Temperature (23°C) : 1. Measure and pour 10cm3 of Iodine solution and 10cm3 of Starch solution into separate test tubes. 2.
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. The leaching technique will be used and precipitates formed via the addition of NaOH to the leach solution. The displacement of iron via zinc will also be utilized. As each metal precipitate forms in the solution, it will have to be separated from the remaining solution and the process repeated until all precipitates have been created and isolated. Next, each individual precipitate will be dissolved into an aqueous solution and ran through a spectrometer.