Development of an Equation

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

You want to investigate a new wave of vitamin water is pH neutral. Results are: Three of the five samples turn a murky

8. The Tubes were observed for a final 5 minutes, noting any color changes in the solutions.

The Vitamin C turned to a red/orange color with no physical/chemical reaction. For the salt the solution turned to an orange color with no physical/chemical reaction. With the Alka-Seltzer, the solution turned to a brown color with no reaction as well. Last but not least, the Baking soda turned to an orange/brown color with no reaction.

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

Copper starts to dissolve and bubbling occurs when nitric acid was added. The solution became green and the beaker started to become orange/brown as gas was being released. Solution then became light blue when washed with water.

For this experiment, I added two chemicals K2CrO4 and HCl together which created an orange color. Then I added NaOH to revert the reaction, which changed the color of the solution back to yellow. I repeated the same procedure but didn’t add the NaOH the second time but added the solution to cold water then hot water for three minutes and observed the reaction. I did the same thing for K4Fe(CN)6 and Fe(NO3)3 except when I mixed them together it produced a dark blue with dark specks solution. I then added NaOH to revert back to the original solution but I got a yellow color with brown specks instead.

This information would be used in Part III to determine an unknown mixture with the results that were found in Part I. A singular drop of Pb(NO3)2 , Fe(NO3)3 , Ni(NO3)2 , AgNO3 , Ba(NO3)2 were added to the reagents: K2CrO4 , KSCN, NH4OH, DMG, HCl, H2SO4 inside of the glass spot plate. If a precipitate formed than the combination resulted in a change of color or appearance (results to these reactions are found in table 1.1). Part II included using the same procedure as done in Part III except this sample contained 1 mL of all five metal ions. This was meant to be a practice round to understand the different steps and procedures. Unfortunately, due to time concerns this trial was cut short at step 3.

The appearance of the precipitate was shown several ways during the experiment. In the 100mL beaker, after both chemicals were added, it was shown as a dotted solution. It was then shown as a solid and a white color in

Then there was the precipitation of the cupric hydroxide. For this step Sodium Hydroxide and water were added to the beaker with the solution until the precipitate settled down. When water and Sodium Hydroxide were added, the solution went from a green color to a dark sky blue color. The observations that were observed were also expected.

B. Looking at the household chemicals you tested with bromthymol blue, what can you deduce from the test results for each of the household chemicals?

* Next, I let the gas from the sodium and hydrogen peroxide go into some Bromthymol Blue. It turned yellow.

2.) Using examples in the last link, draw beakers showing atomic scale representations of aqueous solutions of the following compounds. Classify each as an electrolyte or nonelectrolyte.

After allowing the solution to sit undisturbed for 15 minutes, describe what you see. How does this differ compared with your initial observation?

When the light yellow iron (III) nitrate solution was added to the colorless potassium thiocyanate solution, the color of the final solution was red. To understand why this happens, the individual reactants must be examined. The potassium thiocyanate solution can be broken down as follows: KSCN(aq) ↔ K+(aq) + SCN–(aq). Both the potassium ions and thiocyanate ions are hydrated with water molecules.