Solubility and Stoichiometry I. Introduction The first purpose of this experiment is to apply solubility rules to choose two of eight given reactants to do a precipitation reaction. The second purpose is to use stoichiometry to calculate how much of a reactant will be used in a precipitation reaction‚ assuming that the amount of product is given‚ and to figure out the actual yield vs. the theoretical yield and to calculate the percent yield. The other purpose of this experiment is to practice the
Premium Solubility Stoichiometry Precipitation
NaOCl. One drop of HCl was then added. F) Two drops of KI and two drops of Pb(NO3)2. G) Two drops of NaOH and two drops of phenolphthalein. H) Two drops of HCI and two drops of phenolphthalein. B2) Two drops of NaOH and two drops of AgNO3. C2) Two drops of AgNO3 and two drops of NH4OH. This mixture was then absorbed into the corner of a paper towel and held in direct sunlight for approximately 5 minutes. D2) Two drops of NH4OH and two drops of CuSO4. 4. Each of the three
Premium Chemical reaction Chemical substance Solubility
Discussion for Experiment 1 (Basic Laboratory Operations and Identification of a compound : Chemical Properties) In the first experiment‚ the precision of instrument was studied by measuring the mass of water for several times. The result shows that the mass measurement of the balance is precise since the masses of water in six trials are somewhat close. The reason that the masses of water in each trial are not identical may come from the high sensitivity of the balance that keep fluctuating due
Premium Chlorine Ammonia Sodium chloride
CLASSIFICATION TESTS FOR ORGANIC HALIDES James Anand L. Regala‚ Sabrina Nicolle G. Sarte‚ Ann Michelle Siao‚ Michael Sibulo‚ Victoria Tan Group 8 2C Pharmacy Organic Chemistry Laboratory ABSTRACT This experiment is done to classify organic halides. Most organic halides are synthetic and are not flammable. One way to classify organic halides is by classifying its -carbon atom as primary‚ secondary or tertiary. If the -carbon is attached to one R group‚ it is then primary. If the -carbon is
Premium Sodium chloride Organic chemistry Iodine
purpose of this lab is to observe the reactions of halide ions with different reagents by mixing them together. Analyze data to determine characteristic reactions of each halide ion. Infer the identity of unknown solutions. Materials: * 0.1 M AgNo3 * 0.1 M NaCl * 0.1 M NaF * 0.2 M KBr * 0.2M Kl * 0.2 M Na2S2)3 * 0.5 M Ca(NO3)2 * 3% Starch solution * 5% NaOCl ( commercial bleach) * 12 test tubes‚ 18 mm X 150 mm test tube rack * Pipette Procedure: 1
Premium Chemistry Chemical reaction Hydrogen
and Calculations: Analysis of Unknown Chloride Molarity of Standard AgNo3 solution 0.02785M I II III Initial buret reading 0.00 mL 0.00 mL 0.10 mL Final buret reading 17.00 mL 16.40 mL 17.50 mL Volume of AgNo3 used to titrate sample 17.00 mL 16.40 mL 17.40 mL No. of moles of AgNo3 used to titrate sample mol=VxM mol=VxM mol=VxM
Premium Titration Laboratory Chemistry
The Chemistry of Latent Fingerprints KEY Chemical Reaction Silver nitrate (AgNO3) can react with the salt (NaCl) left from the perspiration on the friction ridge skin to form solid silver chloride (AgCl) and sodium nitrate. The silver chloride can then be converted to silver oxide (Ag2O)‚ which is dark in color and can be more easily seen. Challenge Suppose the fingerprint processing technique that uses silver nitrate to react with the salt from perspiration produced 5.8 x 10-2 grams of silver
Premium Fingerprint Ammonia Chemical reaction
Name : Dania Annuar Class : M11G Title : Determination of Chloride in Urine in Different Circumstances Aim: To determine the chloride content by titrating mixtures of urine against potassium thiocyanate under in different circumstances. Research Question: How do different conditions of urine samples collected affect its concentration of chloride which is measured by titrating the mixture of urine with potassium thiocyanate until it turns red? Hypothesis: The greater the consumption
Premium Urine Ion Standard deviation
the stock solution? 7. What mass of NaCl is required to precipitate all the Ag1+ ions from 20.0 mL of 0.100 M AgNO3 solution? 8. What mass of NaOH is required to precipitate all the Fe2+ ions from 50.0 mL of 0.200 M Fe(NO3)2 solution? 9. If 25.8 mL of AgNO3 solution is required to precipitate all of the Cl ions in a 0.785-g sample of KCl (forming AgCl)‚ what is the molarity of the AgNO3 solution? 10. If 55.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 0.544-g sample of Na2SO4
Premium Ammonia Concentration Sulfuric acid
• sodium hydroxide – NaOH copper sulfate – CuSO4 • sodium phosphate – Na2HPO4 copper sulfate – CuSO4 • sodium chloride – NaCl silver nitrate – AgNO3 • sodium hydroxide – NaOH silver nitrate – AgNO3 • sodium phosphate – Na2HPO4 silver nitrate – AgNO3 Answer: |Your Score |___ of 20 | (4 points) |Score | | | 3. In Part 1 Synthesis Reactions‚ the product of the
Premium Chemical reaction Sodium Sodium hydroxide