What Is The Concentration Of Cocl2 Through The Precipitate Titration

Deborah Bell April 17, 2012 Chemistry 1212K Lab Synthesis Report Introduction In this Chemistry Lab the main objective is to perform accurate chemical analysis for the quantity of elements and compounds in a sample. There will be a compound made then synthesized. The methods used were acid-base titrations, redox

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

Determination of the Composition of Cobalt Oxalate Hydrate Experiment 12 Robbie Kinsey Partner: Debnil Chowdhury Chem. 1312-D TA’s: Russell Dondero & Sylvester Mosley February 9, 2000 Purpose The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O.

Yes, because the solution seen was still blue meaning that not all the copper chloride was extracted from the beaker.

Copper-Iron Stoichiometry Lab Report 10/3/12 Abstract: The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the

Finding the concentration of an unknown sample of copper sulphate using colorimetry. In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution

Purpose The purpose of this experiment is to study ionic reactions, to be able to write balanced equations, and to be able to write net ionic equations for precipitation reactions.

(Hint the concentration of calcium ions in well 12 is 4.9 x 10-5 M.) Place 5 drops of 0.10 M NaOH in each of the wells 1 through 12. When the NaOH is added to each well, the initial concentrations of the reactants are halved, as each solution dilutes the other. Use an empty pipet to mix each of these combined solutions by drawing each solution up into the pipet and squirting it back into the well. (Hint the concentration of Ca2 ions in well 12 is 2.4 x 10-5 M.) Allow three or four minutes for the precipitates to form, then observe the pattern of precipitation. At one point the concentration of both ions becomes too low to have any precipitate form. We will assume that the first well with no precipitate represents a saturated solution. Part B NaOH varies, Ca(NO3)2 held constant To check your results, repeat the procedure but use a serial dilution of the NaOH. In a different row, put 5 drops of 0.10-M NaOH in well 1. Put 5 drops of distilled water in wells 2 through 12. Add 5 drops of the 0.10-M NaOH solution to well 2. Use an empty pipet to mix the solution by pulling the solution into the pipet and then squirting it back several times. The solution in this well, 2, is now 0.050 M in OH- ion. Continue this serial dilution to well 12, and then remove 5 drops from well 12. Add 5 drops of 0.10 M Ca(NO3)2 to each of the wells, and mix each with an empty pipet or stirrer. Again, determine the well where no more precipitate appears. Cleanup

Ocean County College Department of Chemistry Ionic Reactions Submitted by Erin Walsh Date Submitted:   July 24, 2013 Date Performed:  July 24, 2013 Lab Section: Chem-181-DL1 Course Instructor: Amal Bassa Purpose To study the nature of ionic reactions, write balanced equations, and write net ionic equations for precipitation reactions.

The wet, crude product was placed into the 50 mL Erlenmeyer flask. Small amounts of CaCl2 were added to dry the solution. The flask was sealed and the mixture was swirled and left to settle. Once

Task 1: M1 Vacuum Filtration: Vacuum filtration is the method of separating a solid product from a liquid or solution mixture. The mixture is poured through a Buchner funnel containing filter paper. The filter paper holds the solid particles and the liquid draws through the funnel into the flask below. • In order to

As a group, we obtained our salt mixture of calcium chloride and potassium oxalate, and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution, leaving the precipitate. Once the precipitate was dried overnight, it was weighed and the mass was measured. Then we calculated the moles of the precipitate.

           Experiment #10 & #11 The Synthesis of Cobalt Oxalate Hydrate The Synthesis of a Nitrite Complex   February 5, 2012   Chemistry 1211L - 146 - Spring 2012   Procedure The Synthesis of Cobalt Oxalate Hydrate Place 100 ml of distilled water in a 250-ml (or 400-ml) beaker. Add 1.26g of oxalic acid dihydrate (H2C2O4.2H2O) and 1 ml of concentrated

We then proceeded in testing for excess Ca2+ by adding two drops of .5 M K2C2O4 to test tube two and attentively observed to see if a precipitate formed, which it did. This meant that Ca2+ was in excess and C2O42- was the limiting reactant in the original salt mixture. We then cleaned up. Upon returning to our next class, we took the filter paper, with the precipitate on it, and took its mass.

The reaction characteristics of basic copper carbonate 〖mCuCO〗_3⋅n〖Cu(OH)〗_2 were observed by changing the reaction mole ratio. The reaction mole ratio of sodium carbonate to copper chloride (II) was controlled from 1.08 to 1.68. Fig. 1 shows the XRD patterns of copper carbonate powder. At a reaction ratio of 1.08, paratacamite