Chemical Reaction Lab Report

In part 1, the precipitate that forms is a aluminum hydroxide and in part 2 it is magnesium hydroxide. A precipitate is an insoluble solid that emerges from a liquid solution. When the emergence of the insoluble solid from solution happens, it is called precipitation. The property change in the reactants of the lab are when the water, alum, ammonia, react and create the aluminum hydroxide. When the precipitate is formed, it is an endothermic reaction because the change in the product, aluminum hydroxide, decreases in temperature. This is a chemical reaction because different elements rearrange themselves to form a new substance and while they do so, they either absorb heat or give it

The collected and washed precipitate was allowed to air dry and was then transferred and weighed. At the end, a collection of small,

Once, the precipitate was ready to be placed in the oven there was not enough time to allow for it to dry for 10 minutes. The precipitate was only in the oven for about 5 minutes, therefore, when weighed there was excess liquid in the precipitate. The final weight of the precipitate was .45 g which was more than the amount that was started with. From this end weight, it can be deduced that there was excess liquid in the end result.

The precipitate was Calcium Sulfate. The reaction occurred immediately upon mixture of the two reactants. There was a total of 4.3 grams of Calcium Sulfate left in the filter

HCl is an acid and would react with the base, either silver or lead, and once they reacted, a precipitate would form.1 The Sample was heated in step 5 to dissolve the precipitate into the liquid. Heat caused the precipitate to dissolve by breaking apart the molecules into cations and anions. In step 12.

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

Co: Co2+ (aq) + 6NH3 (aq) < ==> [Co(NH3)6]2+, which has a blue/red precipitate. Cu: Cu2+(aq) + 2NH3(aq) + 3H2O(l) < ==> Cu(OH)2(s)

The precipitate was AgCl (Silver Chloride). The color of the precipitate was white. Copper Dichloride + Lead Dinitrate formed a precipitate. The precipitate was PbCl2 (Lead Dichloride) and the color of this was blue. Ammonium Sulfate + Lead Dinitrate also formed a precipitate.

The result is water and a salt. A __salt__ is an ionic compound, which is the result of a combination between a cation and an anion. *__Example__: Reaction between NaOH (base) and HCl (acid) The precipitate formed is AgCl, as indicated by the subscript (s).

We added 5 ml of lead(II) nitrate to 5 ml of potassium iodide in a small beaker. We had to observe the precipitate formed. All of our data is shown in figure 1.

Vinegar is a non-toxic chemical made from acetic acid, water, salt and other chemicals. Sodium Bicarbonate also known as baking soda is a salt composed of sodium ions and bicarbonate ions. Vinegar and sodium bicarbonate cannot be mixed with each other which causes a chemical reaction. There are two chemical reactions that take place in the whole process. Firstly, a double displacement reaction occurs where acetic acid in the vinegar reacts with the sodium bicarbonate to form sodium acetate and carbonic acid: NaHCO3 + HC2H3O2 → NaC2H3O2 + H2CO3.

Precipitates: When Do They Form? Background Information What would happen if two aqueous solutions of different ionic compounds were mixed?

Precipitate also began to form in many of the substances. When the precipitate was formed, it means that a complex ion was not formed and the iron did not remain in the solution. 4. The substances that will have the greatest bioavailability will also have the least amount of precipitate. The more precipitate present, the smaller the chance the iron has to be absorbed.

Medium amount of precipitate became present; solution then became opaque and turned medium blue in

Lab Experiment 4 was an experiment where we determined whether two double-exchange reactions that we performed would be a precipitation reaction, then we had to identify the precipitates formed if any . Precipitation reactions are double-exchange reactions that combine two reactants that are both soluble, or aqueous to produce an aqueous solution and an insoluble solid, aka the precipitate. To figure out whether a solution is soluble we have a set of rules that we must follow, which are: the solution must contain an alkali metal, or sodium, potassium, ammonium, and nitrate. Though, if the two aqueous reactants form two aqueous solutions than no reaction was made. Our group had to perform two reactions, which were: Na2SO4(aq)+LiCl(aq), and NaOH(aq)+ZnSO4