Analysis of Sweets. Is it possible to find any of the substances(Starch,Gelatin, Sucrose/Glucose) in any of the different candy samples?
IB Chemistry: Analysis of Sweets IB Name: klassa andersen 6/9-11 Design: Aim: Is it possible to find any of the substances(Starch,Gelatin, Sucrose/Glucose) in any of the different candy samples? Variables: None Independent variable: None Controlled variable: None Dependant variable: None Materials: * Heater * Copper Sulfate (CuSO4 )(0,1M) * Sodium Hydroxide (NaOH) (2 M) * Beaker (25 ml) * Waterglass * Three different Candy samples(2: Gumdrops,4:Cola Straps,9:Winegum) * Iodide * Water (H2O) Method: . Cut the three different samples of candy into small pieces 2. Put small pieces of the different samples of the candies into three watchglasses 3. Put small amounts of H2O into the three watchglasses 4. Put small amounts of iodide into the three different samples containing small amounts of H2O 5. If the samples turn black then Starch can found in the samples of Candy. 6. To Find if there is any gelatin in any of the three samples of candy, you first cut the three different samples of candy into small pieces 7. Put the three different samples into three different beakers 8. Add small amounts of CuSO4 and then NaOH 9. Check to see if the samples have a purple color which means that the sample of the candy contains gelatin 0. To find out if the any of the three different samples of candy contain any Sucrose/glucose you put the samples containing
How many calories are in a timed burned frito chip?
Calorimetry-Fritos Anabel Castro Chemistry III IB Planning A Research question: How many calories are in a timed burned frito chip? Hypothesis: If a frito chip is burned for 3 minutes then it's calories will be more than that of a frito chip burned for a longer amount of time because there will be less calories in a burned chip than a non-burned chip because there will be less chip to measure. Variables(Independant): The amount of minutes the frito chip(s) will be burned for. (Dependant): Calories measured (Controlled): Type of can, amount of water in can, type of chips Planning B Materials: * 3 Frito chips * Tongs * 3 empty cans of soda * Lighter * Weighing plate * upright stand * timer Method: * Weigh 3 frito chips individually. Record masses of each chip * Fill a can half-way with water * Place the can on an upright stand * Using tongs to hold one frito chip under the soda can. Use the other hand to turn on the lighter and burn the one end of the chip at a resonable distance. Have timer ready! Burn chip for 3 minutes. * Let frito chip cool. Discard soda can. Once the frito chip is cooled, record the mass of the frito chip. * Repeat burning of frito chips for at least two more trials. Use a new can and frito chip for every trial. Add one minute of burning time for each new
charles law
Charles Law Anabel Castro Chemistry III IB Planning A Research question: Hypothesis: Variables (Independant): Temperature (Dependant): Volume of water in graduate cylinder (Controlled): glass beaker, graduate cylinder Planning B Materials: * Thermometer * 10.0 mL graduate cylinder * 500 mL beaker Method: Data Collection Temperature in Volume mL Celsius Degrees (+/- 0.01) Data Analysis
synthesis of aspirin
Synthesis of Aspirin Anabel Castro Chemistry III IB Planning A Research question: Which is more pure, salicylic acid, commerical aspirin, or home-made aspirin when tested with Ferric Chloride solution? Hypothesis: If the three substances are tested for purification by the addition of Ferric Chloride solution, then the purest substance will be salicylic acid then the home-made aspirin because Ferric chloride solution produces characteristic color changes when it reacts with certain organic compounds. In addition, the test tube containing the purest substance will have the smallest color change. Variables(Independant): The substances mixed with Ferric Chloride solution. (Dependant): Pureness (Controlled): amount of ferric chloride solution, amount of distilled water, clean test tubes. Planning B Chemicals: * Acetic anhydride * Salicylic acid * 85% phosphoric acid Materials: * 125 mL Erlenmeyer flask * 5 mL or 10 mL graduated cylinder * 600 mL beaker * 400 mL beaker * thermometer * burner * suction flask * buchner funnel * vertical upright * extension clamp with clamp holder * top loading balance * test tube with cork * split cork to hold thermometer Method: * Warning: Be careful when using Acetic Anhydride and Phosphoric Acid. Both chemicals can cause serious burns. Use gloves when handling and use in hood. * Using a top loading balance to
The Haber process involves reacting 1 mole of nitrogen gas with 3 moles of hydrogen gas to make 2 moles of ammonia.
Haber process essay Background In a chemical change new substances are made. Chemical bonds are broken and reformed. These processes require energy. Chemical changes are usually irreversible. Some chemical changes are reversible, however. For example, in the change of hydrated copper sulphate to the anhydrous form, the water of crystallization is removed and the blue hydrated form becomes the white anhydrous form. The reaction can be reversed by adding back the water. Another reversible chemical change occurs in the Haber process. The Haber process involves reacting 1 mole of nitrogen gas with 3 moles of hydrogen gas to make 2 moles of ammonia. The nitrogen is obtained from the fractional distillation of liquid air and the hydrogen from heating steam with methane. Heat is given out during the reaction to make ammonia heat is produced. This is called an exothermic reaction. As the reaction making ammonia is reversible, adding heat causes the back reaction to be favoured. This means that if ammonia is required (that is, the forward reaction is to be favoured) then a lower temperature should be used. Temperature in the Haber process Although the forward reaction is favoured by a lower temperature, too low a temperature means that the rate of the forward reaction is too slow. The particles have very little kinetic energy at low temperatures so do not move a great deal and
Hous Process for producing Sodium Carbonate
Hou's Process for Sodium Carbonate Introduction: Hou's process is developed based on Solvay process by Chinese chemist Debang Hou in 1930s; the first few steps are the same as the Solvay process. However, instead of treating the remaining solution with calcium carbonate (CaCO3), carbon dioxide (CO2) and ammonia (NH3) are pumped into the solution, then sodium chloride (NaCl) is added until the solution saturates at 40 °C. Next, the solution is cooled to 10 °C. Ammonium chloride (NH4Cl) precipitates and is removed by filtration, and the solution is recycled to produce more sodium carbonate (Na2CO3). (Source 2.) The equation of Hou's process is: (1)NH3+H2O+CO2=NH4HCO3 (2)NH4HCO3+NaCl=NH4Cl+NaHCO3v (3)2NaHCO3=Na2CO3+H2O+CO2ˆ NaCl (saturation) +NH3+H2O+CO2=NH4Cl+NaHCO3v 2NaHCO3==Na2CO3+H2O+CO2ˆ Compare the Solvay process and Hou's process: (source 1.) The advantage of Hou's process is: Hou's process kept the advantage of the Solvay process, but increased the yield from 90% to 96%. The Product ammonium chloride (NH4Cl) can be used as fertilizer, and can also be united with the production of ammonium. Hou's process uses carbon monoxide (CO) to produce the required carbon dioxide (CO2) instead of using calcium carbonate (CaCO3). This eliminates the by-product calcium chloride (CaCl2) which is produced from the calcium carbonate (CaCO3) in the Solvay process.
How does the change in temperature affect the rate of reaction?
Temperature affecting Reaction Rates * Guiding Question: How does the change in temperature affect the rate of reaction? * Objectives: The objective of this experiment is to see how temperature affects reaction rates. * Hypothesis: We think that temperature increases the rate of reaction because the increase in temperature increases the energy of the particles and therefore overcomes faster the activation energy. * Variables: . Independent: Temperature (°C) 2. Dependents: Time (s) and rate of reaction (s -1) 3. Control: Volume (ml) and concentration (M) of HCl and Na2S2O3. * Procedure: a) Transfer 50 ml 0.0400 M sodium thiosulfate solution into a 50 ml flask. b) With a marker make a black cross in a paper and put it below the flask. c) At room temperature quickly pour 5ml HCl of a 2M solution d) Measure the time needed for the black cross to disappeared. e) Repeat this procedure and then place the flask in a hot plate using a thermometer and vary the temperature to 30 °C, 40 °C, 50 °C and 60 °C. f) Repeat the experiment twice for each temperature and find the average. * Materials: i. 2 measuring cylinder (50 ml) ii. Thermometer 10 °C - 110 °C iii. Chronometer iv. 2 flasks (250 mL) v. 60 ml of a 2M solution of HCl vi. 600 ml of a 0.04 M solution of Na2S2O3 * Observation: Sodium Thiosulfate ions (0.04 M) with different temperatures ºC mL HCL
How Temperature affects the Rate of Dissolving Lab
How Temperature affects the Rate of Dissolving Question: What is effect does temperature have on the rate of dissolving sugar in water? Hypothesis: If the temperature increases then the sugar will dissolve faster in the water since in a warmer solvent the particles are moving faster, therefore allowing the particles of the solute to mix with the particles of the solvent quicker. Variables: Independent variable is the temperature of the water Dependent variable is the rate of dissolving measured by time. Controlled variables: Variables How to Control The amount of water to dissolve the sugar in Measure the water with a cylinder beforehand The amount of sugar added to the water Measure the mass of the sugar before adding Type of liquid Tap water Container for dissolving Beaker of same size and shape Required Materials: - 4 beakers (250ml.) - 100 grams of sugar - 1 thermometer - I Bunsen burner - 1 Tripod - 1 Metal Gauze - 4 Stopwatches - 1 Graduated Cylinder Procedure: . Measure 200ml. of tap water with a graduated cylinder and pour it into a beaker. Measure and record the temperature, with a thermometer, of the water. 2. Then add 25 grams of sugar to the water and measure the time with a stopwatch, record the time it takes to completely dissolve. Stir every 5 minutes for saving more time. 3. While the first beaker is dissolving, set up the heating
Equilibrium Changes
Qualitatively Investigating Changes in Equilibrium Research Topic: In this lab we will be observing the qualitative changes in equilibrium by changing known concentrations of reactants: iron and thiocyanate ions, and finding its effect on the position of equilibrium. We will be using a colorimeter to find the absorbance of the solutions with known concentrations and we will plot a graph of absorbency vs. concentration which will allow us to quantitatively track the changes in equilibrium of a solution. I will be using iron nitrate and potassium thiocyanate in order to give us ironthiocyanate. Fe3+(aq) + SCN-(aq) FeSCN2+ . Variables Chart Independent variable The variable I will be manipulating is concentrations of the FSCN2+ (ironthiocyanate). Dependent variable(s) Position of equilibrium shown through equilibrium constant Kc. Control Variables - the variables that must be kept constant during the experiment How variables affect experiment How the method compensates for experiment Metal ions Without the reactants including metal ions, the solution would be colourless and thus there would be no way of measuring absorbency and thus of finding concentration. I will keep this constant by using metal ions (Fe3+) and using that same reactant throughout all of my trials. Colorimeter Different colorimeters may have different absorbency ratings. As well using
The purpose of this experiment is to to prepare a solution of primary standard of potassium hydrogenphthalate C8H5O4K, which can be used to standardise water-soluble bases such as sodium hydroxide solution.
Preparing a solution of primary standard. Purpose The purpose of this experiment is to to prepare a solution of primary standard of potassium hydrogenphthalate C8H5O4K, which can be used to standardise water-soluble bases such as sodium hydroxide solution. Formula: n= m/M and c= n/V Theory Many common reagents are supplied in an impure state or they can easily pick up moisture from the atmosphere, or may be supplied as concentrated solutions of an uncertain concentration. As a consequence, solutions made from such substances must be stanardised against a substance of known purity. We call them primary standards. Chemicals • Potassium hydrogenphthalate (C8H5O4K) Apparatus • top loading balance (weighing scale) • weighing bottle • beaker • volumetric flask Procedure • We started by weighing 5 g of potassium hydrogenphthalate accurately in a weighing bottle. • I poured the content of the weighing bottle into a beaker and i reweighed the the weighing bottle. I also made sure that no residue of the chemical was left in the weighing bottle. • I added about 100 ml of distilled water to the beaker and stired it until it dissolved the hydrogenphthalate. • I transferred the solution from the beaker to a 250 cm3 voumetric flask. i washed the beaker several times and poured the content into the volumetric flask just to make sure that no residue