Add 5 mL of copper (II) sulphate solution to a test tube. Add 5 mL of sodium carbonate in another test tube. Record the appearance. 2. Write a hypothesis on what you think will happen when mixed.
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.
Lesson written by Carolina Sylvestri Experiment: Reaction Between Ions in Aqueous Solutions The Monster Mash Background: Ionic solids dissolve in water to form aqueous solutions which conduct electricity. These solutions contain both positive and negative ions in such numbers that their net electric charge is zero. In this experiment, you will mix various ionic solutions, two at a time, to determine which combinations form precipitates. Knowing which ions are present makes it possible to deduce which of the possible ion combinations are responsible for the precipitates. From your data table, it will then be possible to generate a solubility table.
The test for Sodium Bicarbonate included mixing that with HCl. After doing this experiment bubbles would form in the solution. This was CO2 being released. This reaction is a way of testing for Sodium Bicarbonate. BACKGROUND: For these experiments a 96-well plate was used.
Alex Evans Sanders Dellinger Ryan Shockney Rashaad Williams October 18, 2010 Experiment 29 Procedure Proposal In this experiment, the experimenter will be given a one gram sample of Chromite. Chromite is defined as an Iron Magnesium Chromium Oxide. The objective of this lab is for the experimenter to determine if Iron, Magnesium, and Chromium are in the unknown sample, and from these conclusions, infer if the unknown sample is actually Chromite. In doing this, multiple laboratory skills are needed, along with general knowledge on the elements comprised in the experiment to be covered. As aforementioned, the main objective of this lab is to determine whether or not the unknown sample is in fact chromium.
How could it have been improved? (b) Based on your evidence, which anion could be used to precipitate most of the metal cations? (c) Which anion could be used to selectively remove silver ions from solution? Why? (d) What evidence suggests that nitrate compounds are soluble in water?
In the first part, five 100 mL flasks of 5 mL ligand solution, 5 mL 2 M sodium acetate, 4 mL 3 M NH2OH, and 1-5 mL Fe2+ solution are diluted with water. The absorption spectrum for varying concentrations of Fe2+ are measured using a spectrophotometer and the data is graphed in Excel. The slope of the line is ε in the Beer-Lambart equation A = εcl. In the second part of the experiment, eleven flasks containing diluted stock solutions of Fe2+ and ligand are mixed with 5 mL 2 M sodium acetate and 4 mL 3 M NH2OH and diluted with water. The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel.
Introduction In this experiment copper chloride and iron chloride are separately reacted with sodium hydroxide to determine what their charge is. The copper chloride can be either copper (I) or copper (II) chloride. The iron chloride can either be iron (II) or iron (III) chloride. By completing a double replacement reaction with the sodium hydroxide the formulas of the iron and copper chlorides can be found. Objective The objective of this lab is to find the formula of an ionic compound.
The purpose of the laboratory is to determine the number of waters of hydration in aluminum potassium sulfate as well as the purity of the Alum we produce. Experimental1: The procedure for this laboratory was followed closely from Professor Abrams’ lab manual. In Part 1 of this laboratory an aluminum soda can was cut apart and the paint and lacquer was rubbed off with steel wool. Next, the aluminum can was rinsed off with tap H2O and then cut into small pieces. Using the analytical balance 1.0537 g of the aluminum can was weighed out.
· There are numerous measures of the amount of solute in solvent. Try this exercise. Exercise 1. Devise a measure of solute concentration that you would place on the label for the following case: You weigh out 2.56 g of zinc iodide: You put the solid zinc iodide in a 500 mL flask and fill the flask with water to ttie 500-ml nia'rk. You now have sao mL of a zinc iodide aqueous solution.