Ionic Compound

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.

***Repeat steps 2-4 for each of the following: 5 mL of oil and 2 g each of cornstarch, sodium chloride, and sodium bicarbonate.

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The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube

There is a very easy way to find the empirical formula of a compound using the mass percentages found through elemental analysis. First, convert the mass percentages to a mass, assuming that the compound is 100g. Then convert each mass into moles using the molar masses. Then divide each of these moles by the element with the smallest amount of moles. That is the ratio of the empirical formula. Just make sure that the numbers are in whole numbers, if not, multiply by common denominators to get all of them to a whole number (3).

Upon finishing the experiment it was concluded that the the ability to determine whether or not the ore should be mined was successful. According to the data results it was determined that

As we learned before on how to determine the empirical formula of a compound based on the test and also chemical analysis on it. Hence this experiment is mainly goes around with how to determine the empirical formula of Magnesium Oxide following various tight procedures in order to get the knowledge and apply it onto another compounds. We are investigating the empirical formula of Magnesium Oxide in this experiment.

Crystals also formed on the bottom of the beaker as the concentration was not fully dissolved, settling to the bottom of the beaker. To improve the experiment, we could have used a better thermometer to record the appropriate data. We also should have heated the solution further to ensure the concentration of Copper Sulfate was

Introduction: The purpose of this lab is to find the unknown concentration of Cu+2 by comparing the solution to a set of standard concentrations, different known concentrations, which are prepared by diluting approximately 2.5 grams of copper (II) sulfate pentahydrate. A concentration is the amount of solute relative to the volume of a solution, the more solute the more concentrated the solution will be. Concentrations are reported using molarity (M) which is the moles of the solute by the volume of solution in liters.

E.g. Sodium chloride, NaCl, salt. The formula does NOT describe a molecule, but only gives the simplest ratio between the bonded atoms... This is the empirical formula Number of Moles in a Given Mass N=m/MM No.

In the final experiment we filled a dialysis bag with starch solution and tied off both ends of the bag so that it is water tight. We then filled a separate bag with sodium chloride and submerge both dialysis bags in two beakers of distilled water. We allowed the bags to sit in the water for 10 minutes. We then put silver nitrate into the water that held the dialysis bag filled with sodium chloride and recorded any changes in the water. We then added iodine to the water that held the dialysis bag of starch and observed any changes in the water.

The main goals of the experiment are to be aware of the ionic compound by comprehending of the principle of solubility. Then to be acquainted of the solubility rules because it’s important to design combination of a various compounds . After that, detach the solid product to see the final solution. However, in this experiment we have been used several material, such as, BaSO4, Zn(OH)2, Al(OH)3, and NaCl to discuss what will be the final compound. On the other hand, now we can define the Ionic compound, as a common, yet distinctive type of a chemical compound, and it’s a compound, which created by ions bonding with each other through electrostatic forces. However, the acid base reaction includes the transfer of hydrogen ions; in general, we

0.5% of copper sulphate solution was added by drop at a time and and the test tube was shaked continuously.

There are a few points of uncertainty---as mentioned above---in the lab procedure that could have led to varying results. For instance, the procedure was repeated multiple times for certain elements, but others were only tested twice. This is definitely a point of inconsistency, las it would have been better to test all of the elements multiple times if we were doing it to a select few.