Calculations involving the Mole, Avogadro’s Number, Molar Mass, Mole-Mole and Mass-Mole calculations in chemical equations. Combustion analysis and calculation of empirical and molecular formulas from composition analysis. Electrolytes and non-electrolytes. Precipitation reactions and solubility rules. Writing balanced molecular equations and net ionic equations.
What are the identities of the substances found after electrolysis and heating? The identities of the substances found were Iodine, Iodide ion (I-), Triodide ion(I3-), Zinc metal and Zinc ion(Zn2+) Post Lab questions: 1. What did this experiment convincingly show about the composition of the white solid? I put that the experiment showed us the white substance was comprised of Zinc ions and iodide ions, and that the two ions and be separated back into their respective elements 2. During the electrolysis, a gray solid formed on the negative wire of the battery and the dark red solution formed at the positive wire of the batter.
½ mark 10 Outline the reaction pathway to produce propanoic acid from propane. Write the chemical reactions (using chemical structures) indicating reactants and any special conditions. 2 marks 11 Name all the chemical species in Q10 using the IUPAC system. 1 mark 12 If you put the product formed in Q10 in a basic solution, what would the resulting ion look like? 1 mark 13a Indicate the chemical equation when your product from question 10 undergoes a
Identify the acid-base reactions from the reactions shown on this worksheet. 23. Think about the reactions for which we have written ionic equations. Which category of reactions would they best fit in to? Explain your answer.
This was the solution that was used in order to obtain the absorption spectrum for each of the different iron (II) ligand examples different flasks. Each of the five flasks were
Write a hypothesis on what you think will happen when mixed. 3. Combine the substances; record observations. Hydrochloric Acid and Magnesium 1. Add hydrochloric acid to a test tube.
Aim: To determine the presence of the cations Na+, K+, NH4+, Ag+, Cu2+ and Bi3+ in the solution under analysis. Procedure: Please refer to page 26-27 of CHM152/154/2252 Laboratory Manual. Results: Procedure No and Ion Test Reagent or Technique Evidence of Chemical Change Chemical(s) Responsible for Observation Equation(s) for Observed Reaction 1. Na+ Perform flame test by dipping a test loop in test solution and putting in Bunsen flame after cleaning the loop with HCl(aq) A brilliant yellow persistent flame occurs Presence of sodium in the test solution - 2. K+ Perform flame test by dipping a test loop in test solution and putting in Bunsen flame after cleaning the loop with HCl(aq).
This will help determine the types of ions present in the water sample. Ions also absorb light differently according to the concentration of the ions in the solution. Using absorption spectroscopy the absorption rate is used to determine which ions are present in the solution and at what concentration. The equation m1v1=m2v2 will be need where m1 and v1 are the initial concentration and volume, and m2 and v2 and the final concentration and volume. Experimental: List of Chemicals 0.5 M NaCl solution 0.5 M LiCl solution 0.5 M KCl solution 0.5 M CaCl2 solution 0.5 M SrCl2 solution Fe/Cu solution containing 400 ppm Cu2+ and 20 ppm Fe3+ in SCN- solution 20 M iron(III) nitrate solution
Observations of Chemical Changes Purpose: To examine the reactions of chemicals and see what types of changes can occur. Procedure: I used a 96-well plate and the following chemicals to document the chemical changes that occur: Ammonia, Bromthymol Blue, Copper (II) Sulfate, FDC Blue dye #-1, Hydrochloric Acid, Lead (II) Nitrate, Phenolphthalein Solution, Silver Nitrate, Sodium Bicarbonate, Sodium Hydroxide, Sodium Hypochlorite, and Starch Solution. Data Tables: Well #/Question | Chemicals | Reaction | A | NaHCO3 and HCl – CO2 | Bubbles formed | B | HCl and BTB | Turns a yellow/orange color | C | NH3 and BTB | Turned to orange | D | HCl and Blue Dye | Turns green | E | Blue Dye and NaOCL | Stayed blue | F | Kl and Pb(NO3)2 |
Purpose of the Experiment: To produce diphenylmethanol from the reduction of benzophenone by using sodium borohydride as a reducing agent. To check purity of a product by using thin layer chromatography (TLC) and by performing a melting point. Introduction: The key step in the reduction of a carbonyl compound by either lithium aluminium hydride or sodium borohydride is the transfer of a hydride ion from the metal to the carbonyl carbon. In this transfer the hydride ion acts as nucleophile. The mechanism for the reduction of a ketone by sodium borohydride: (1) Method (Based on Chemistry Laboratory Manual): 1.