Analysis Of The Seven Numbered Solutions Through Chemical Reactions Lab Report

In addition, my hypothesis for this lab is the cornstarch and water will make a liquid-solid substance. The Investigating Mixtures Lab objective is to observe that not all liquids behave the same way when mixed with other liquids. Also, my hypothesis for this lab is the vegetable oil will not mix with the water. Conclusion/Analysis:

This means that all of the elements in the same group have a main aspect in common, except for a few exceptions. These elements react with the same specific compounds. This was used to identify the order of the groups from left to right and to determine which elements go under which group. Some research was conducted to identify all the names of the groups ranging from element number one to element number 20. Once all group names were recorded, it was researched which groups react with which compounds that are given on the element cards.

Untested Victims Bailey Votto 4/19/16 Margaret Oakes Paper 4 Draft #2 When the two solutions, sodium chloride (NaCl) and silver nitrate (AgNO3) react, a soluble sodium nitrate (NaNO3) and a precipitate silver chloride (AgCl) form. While this reaction is not a common occurrence for most of us in our daily life and work, it is in a forensic science lab. This chemical reaction is just one of the many techniques used to unveil fingerprints in a crime scene. Unfortunately, fingerprints are not always left or able to be found. In that case, new chemical procedures must take place.

When the substance reacted with the solution it turned from its initial color yellow/brown to its final color lilac/violet. The experiment went by easily flowing nicely, although one or two things went wrong, none had any effect on the experiment. It is very important to know what foods are composed of because, knowing what is inside our food is essential for our health. We need to be aware of what things we are consuming and what we should be consuming for our bodies to function properly.

One of the reactions you observed resulted in this product: NaCl + H2O + CO2 (g)? What well did this reaction occur in? Describe how the observations for this reaction support your answer. B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript70 Words A reaction I observed in number 1.)

There are however some aspects of the experiment that could be changed with little to no effect on the color of the solution or the calculated molar masses. For instance, if the amount of deionized water used were to be doubled, there would be no change in the results of the titration calculations. This is the reason that the amount of DI water used in this experiment was not measured nor

Each reaction was composed of two compounds as the reactants and two compounds as the products. The metal in each of the reactants bonded with the opposite compound’s nonmetal and created a new product. For example, barium chloride and silver nitrate reacted and yielded barium nitrate and silver chloride. The ionic salt products could be dissolved in water. When this occurred, H20 weakened the bond between the ions and surrounds the two ions individually because of an attraction to create a solution.

They occur when two ionic compounds are used as reactants and the anions and cations switch places between the two. This type of reaction will proceed provided that the reactions do not have the same cation or anion as explained in discussion question #3. Also, the products of the reactants must have at least one solid to indicate a precipitate is made. If all products are aqueous then the reaction did not take place as shown by the fourth reaction presented in discussion question #5.

This lab consisted of determining whether a certain liquid was an acid or base and experimenting with the pH of various substances when either acid or base was added to them. The lab was executed by using two different types of indicators as well as a titration in the end. The first indicator used was litmus paper. Through litmus paper, it is possible to decide whether a liquid is an acid or a base. By placing one slip of red litmus paper by one slip of blue litmus paper and dropping beads of the liquid on each, determining whether the liquid was a base or an acid was possible.

The system had an increase in the concentration of the product. So, when the ice bath was put in place the reaction was reactant

Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.

The reactants, hydrogen and boron, are among the most abundant elements on earth. These elements can be used in excess without any repercussion. (Ruggiero

pH means “hydrogen potential”. (The carbon dioxide comes from the lungs during exhalation. Carbonic acid is a weak acid and is therefore in equilibrium with bicarbonate in solution. When sig- nificant amounts of both carbonic acid and bicarbonate are present, a buffer is formed, because they neutralize each other.) Under normal circumstances, there’s much more bicarbonate present than car- bonic acid (the ratio is about 20:1).

TABLE 1 - Particle Size Range (micrometers).5 3. RESULTS AND DISCUSSIONS Experiment A shows that the compound present in the dust sample is Sodium Nitrate. Experiment B shows the dust is inhalable and can directly get to the lungs. From the oxidation state of nitrogen, Nitrate is the most oxidized form of nitrogen present in the environment.

If anything is added out of order, then the experiment will not react as needed. The experiment was held in two parts. The titrant was prepared first because it was what was going to be used in mass amounts for both parts. The preparation of the analyte and indicator needed to be done precisely. If anything was added out of order the color change would not happen.