Stoichiometry/Percent Yield Lab Purpose: to predict the amount of product generated from a double displacement reaction. In class, you have learned how to use stoichiometry to determine the amount of a product generated from a chemical reaction. We call this the theoretical yield. In this lab, sodium bicarbonate (NaHCO3, a.k.a. baking soda) will be mixed with acetic acid (HC2H3O2, a.k.a.
Halogens Aim: To find the difference in appearance, reactivity and solubility of Halogen elements. Materials: * Chlorine * Bromine * Iodine * Chlorine solution in water * Bromine solution in water * Iodine solution in water * Test-tubes * Rubber bungs * Potassium chloride solution * Potassium bromide solution * Potassium iodide solution * Silver nitrate solution * Cyclohexane Method: Experiment 1- Appearances and solubilities of halogen elements 1. Observe the elements: Iodine, Bromine and Chlorine at room temperature and record their physical state and color. 2. Boil or sublimate (if necessary) to observe each element in gaseous state, record color of vapor.
Lab #5 – Exp #2: Evidence for Chemical Change Name: Period: 2 Date Due: 1/27/12 Lab Partners: ______________________ Objective: • To observe the types of evidence that indicate a chemical change has taken place. • Infer from the observation of chemical change that a new substance has been formed. Procedures: 1. In the 250ml beaker, make a water bath by heating until boiling approximately 125 ml of water. 2.
=n (mol)/v (dm3) Whereby c=concentration, n=number of moles and v=volume used. (JOHN GREEN AND SADRU DAMJI, PG 27.THIRD EDITION) Volume=0.1dm3 Concentration of acid =0.0048996mol/0.1dm3 =0.049moldm⁻3 Also, to calculate for the average titre volume of the acid used, I summed up the three consistent values from my experiment and divided it by 3(sarps series, 2009) thus Average Titre volume= (19.60+19.60+19.60) 3 =19.60cm3 Also, to calculate for the concentration of sodium hydroxide, I used The dilution factor, C₁v₁=C₂v₂ (JOHN GREEN AND SADRU DAMJI pg28, third edition) whereby C₁=concentration of the acid used=0.049moldm⁻3 v₁=volume of acid used (titre volume) =19.60cm3 C₂=concentration of the base, v₂=volume of the base used=10cm3 Therefore C₂=
Once the solution of sodium thiosulfate had been standardized the molarity of the solution was known and sodium thiosulfate could be used to titrate tap water and an iodine solution to determine the amount of chlorine in the tap water and iodine in the iodine solution. Procedure/ Observations: The first step of the experiment was to standardize the sodium thiosulfate solution. This was done by cleaning a 50 mL buret and rinsing it three times with sodium thiosulfate solution to ensure the surface of the buret was consistent with the sodium thiosulfate throughout. The buret was then filled with the sodium thiosulfate solution. The buret was monitored to ensure that the solution extended to the tip of the buret and that no air bubbles were present because both would cause an inaccurate titration.
Stoichiometry is a section of chemistry that involves using the relationships between reactants or products in a chemical reaction to determine the desired quantitive data. 4. Using the balanced chemical reaction between Sodium carbonate and Calcium Carbonate given in page 92 of your lab manual (first paragraph of procedure), find the mass of Sodium Carbonate (in grams) needed in reaction? Na2CO3(aq)+CaCl22H20(aq)-CaCO3(s)+2NaCl(aq)+2H2O Date:_____3/30/2015____________ Name______Chloe Flake______________ 1. Title: 1pt Stoichiometry Of A Precipitation Reaction 2.
Ocean County College Department of Chemistry [Observations of Chemical Changes] Submitted by Andrew Grimm Date Submitted: 5/31/14 Date Performed: 5/31/14 Lab Section: Chem-181DL2 Course Instructor: Amal Bassa Purpose The main goal in this experiment is to observe the properties of simple chemical reactions, and relating their chemical properties to household products. Procedure To begin this experiment I placed two drops of NaHCO3 into well A1 of the 96-well plate, and then added two drops of HCl into well A1. Next I placed two drops of HCl into well B2, and added two drops of BTB, and observed the color. Then I placed two drops of NH3 into well C1 and added one drop of BTB, and observed the color. Next I added two drops of HCl into well D1, and then added two drops of blue dye, and recorded what I saw.
CHEMISTRY HL Investigation 1.2 Standardizing a solution of hydrochloric acid using a standard solution of Sodium Carbonate Candidate name: Amjad Al-Jafari 11 IBDP 1/2/2013 Preparing a standard solution of Sodium Carbonate (A) • Data Collection and Processing: 1. Data Collection: -Mass of Sodium Carbone which is the solute in this solution: 1.26 ± 0.01 grams. -Volume of distilled water which is the solvent in this solution : 250 ± 0.3 cm3 = 0.250 dm3 -Molar Mass of Sodium Carbonate: 2 Na + 1 C + 3 O = 105.99 Observations: Before beginning the experiment we observed that: • Sodium Carbonate is solid powder that has a white color, • Distilled Water is colorless. During the experiment we observed that: • As we started to add the solution of Sodium Carbonate to water its particles started to dissolve in the solvent as we are stirring until all particles are dissolved in the solvent (water). After the experiment we observed that: • However a white solid powder of Sodium Carbonate has been added to water no color change occurred, it stayed colorless, still all particles of Sodium Carbonate has dissolved in water.
Riya Singh Banita Sathpathy Period 1 Analysis of a Commercial Bleach Purpose The purpose of this experiment is to determine the amount of sodium hypochlorite in commercial bleach by reacting the bleach with sodium thiosulfate. Procedure In this experiment a solution of sodium thiosulfate of known concentration will be added to the bleach using a buret in a titration procedure. The disappearance of the dark blue color of the starch- iodine complex will signal the end point. Data Trial 1 Trial 2 Trial 3 Initial Reading (ml) 0 0 0 Final Reading (ml) 35.7 36.0 36.6 Volume of Na2S2O3 35.7 ml 36.0 ml 36.6 ml Calculations and Analysis 2 S2O3-2 = I3- = I2 = ClO- Therefore looking at the equation above, we can conclude that for every mole of sodium thiosulfate we need half a mole of sodium hypochlorite. (35.7+36+36.6)/3=36.1 ml is the average volume of the Na2S2O3.
Then the content of the chloride in the original salt is then calculated using stoichiometry (Chemistry Department, 2014). Theory: Gravimetric analysis is the measurement of mass, which by definition is categorized into four types however the use of one is only necessary in this experiment, which is precipitation (Gravimetric Analysis, 2012). Therefore the goal is to determine the original amount of ion. This is by isolating the ion in solution by a precipitation reaction, filtering and washing the precipitate free of pollutants, then the conversion of that precipitate to a product of the unknown sample given (Gravimetric Analysis, 2012).Therefore determining the quantitative of that substance by the precipitation reaction. The equation of the precipitate proceeds as follow if followed by the criteria given.