Flame Test Lab Report

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 titrations, gravity filtration, and distillation. General conclusions included

The hypothesis is correct. Potassium chloride mixed with silver nitrate creates a white precipitate. Barium

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 color of the solution was turning slightly into yellow and the color of the iron strip into white.

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

In a chemistry stockroom, a vial of an Unknown White Compound was found. In order to properly dispose of the substance, the substance has to be identified .The possible compounds has been limited to one of 15 different compounds. Also, approximately 5 grams of the Unknown White Compound (UWC) were available for testing. In order to determine the properties of the compound, a series of tests was conducted. These tests included a ph test, a conductivity test, a flame test, a sulfate test, a halide test, an ammonium test, a solubility test, and a carbonate test. Using the results of these experiments, it was hypothesized that the UWC is potassium chloride. To further confirm the hypothesis, a synthesis of potassium chloride was conducted.

10. Ba (NO3)2, barium nitrate produces pale precipitate when put in reaction with sulfuric acid.

In the first part of the experiment (identifying the chemical makeup of the unknown compound

then we know Ca2+ is involved in the solution. Next we add OH into the

Similar data have also found in 2B and 2C. These two groups of reaction both contain a similar element in the solution, so it might be the reason to cause the solid form in similar colors. The reaction of 1D also become a precipitate, but appeared in a different color. For 3C, the result was not clear enough to make sure if a precipitate was formed or not, but after a while, the solution turned slightly foggy. Solution 2D, 3D, and 4D had no color change, therefore no precipitation was formed.

The spot test came back positive for Barium which contradicts table 1.1 as a non-reaction. Regardless of what table 1.1 predicted, it was confirmed that the unknown solution contained Silver, Nickel, and

In this lab an attempt was made to determine the concentration of a Ba(OH)2 solution by using the conductimetrically determined equivalence point of the reaction between Ba(OH)2 and H2SO4 and by gravimetric determination. The molarity using the equivalence point was determined to be 0.076 M, with a percent error of 24% (actual value was 0.100 M). The molarity using gravimetric determination was 0.0835, an error of 17%. One possible error is the presence of bubbles in the buret. Bubbles would have caused the buret reading to be too high, resulting in a larger equivalence point. Another possible error deals with the colloidal nature of barium hydroxide due to its relatively low solubility. The colloidal barium hydroxide would make it

Recently, I learned how to make a lava lamp using a mason jar, vegetable oil, water, Alka-Seltzer and food coloring. I placed water and food coloring in a jar filled with vegetable oil. Because water is denser than vegetable oil, the water and water-based food coloring sank to the bottom of the jar. Once the Alka-Seltzer was placed in the jar and reacted with the water, carbon dioxide bubbles formed, creating colorful bubbles rising to the top of the jar. This experiment taught us about polar and nonpolar liquids and their immiscibility as well as liquid density. The colorful product of this experiment created an aesthetically-pleasing lava lamp, which we decorated our classroom with. This shows that science projects can not only be a learning

Ten cations were reacted with eleven anions and the results of the reactions were recorded; the reactions were performed so that the results could be used in the qualitative analysis of an unknown mixture containing a combination of the same ten cations. There are some distinct differences between the reactions that occurred and the reactions that were predicted to occur. The discrepancies can mostly be explained by contamination: the wells, where the reactions occurred may have been contaminated.

| White precipitate turn to yellow and then brown and finally black; white precipitate soluble in excess S2O32−.