Ionic Reaction Lab Report

Ionic compounds are soluble in water to a certain point depending on the compound. The level of solubility changes among different compounds. Some ionic compounds can completely dissolve in water and appear to be a homogeneous mixture. Although, some ionic compounds dissolve very little, and could be considered insoluble, since it does not dissolve fully. Depending on the compound, the level of solubility can be high or low. However, ionic compounds could dissolve to a certain degree. If the solution appears to be a heterogeneous mixture, many may assume through visual representation that it may be insoluble. As stated previously, the smallest amount of solubility should be considered. To confirm whether or not the substance is soluble, observe the efficiency when conducting electricity. Due to practical reasons, the slightest solubility could be considered insoluble by people.

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

In this lab we performed four test. Using these test we discovered how the chemicals compounds Citric Acid, Calcium Chloride, Sucrose, Potassium Iodine, Phenyl Salicylate , and Sodium Chloride reacted to heat and many solutions. We also noticed that Phenyl salicylate was the least reactive out of all chemical compounds. Using the information discovered from the lab we were able to separate the chemical compounds into two groups. In group one were the chemical compounds Calcium chloride, Citric acid, Potassium iodide, Sodium chloride, and Sucrose these chemical compounds reacted to three of the four test. Group two was just Phenyl salicylate which reacted to only one of the four test. We also were able to state that group one was a covalent compound group and, group two was an ionic compound

As a result of this lab experiment, the hypothesis is attested to be precise as the ionic compounds did go through a double displacement reaction. The purpose of this experiment was to establish what occurs when two pairs of compounds react with one another. The information collected while doing the lab has allowed more knowledge to be obtained, as one can visibly see the changes happening and different signs of chemical changes. The cations and anions in the ionic compounds have successfully exchanged places with one another, creating the compounds with the different properties evident in the observation given. For example, precipitates were visible in almost all reactions in this experiment. Therefore, this lab experiment was held to demonstrate

Is A+C a chemical reaction? Yes, because of serval chemical changes happening to the solution before and after. I came to this conclusion by using three pieces of evidence. The three pieces of evidence were a ph imbalance, a dramatic density rise, and a change in electroconductivity.

We discovered that the acetic acid reacted only with baking soda and sample #2. The acetic acid did not react with the sucrose or the table salt. During the conductivity test, the conductivity meter showed that the aqueous form of each substance, sample 2 included, conducted electricity. As the conductivity test produced no conclusive data, we based our determination of sample 2’s nature on the reaction with acetic acid. Sample 2’s reaction was only comparable to that of baking soda, leading us to believe sample 2 is indeed baking

At station A when zinc and hydrochloric acid react with each other it is a chemical change because it creates gas bubbles and temperature change. At station B where NaOH solution and phenolphthalein react with each other it is a chemical change because it changed to the colour purple and the change looked difficult to reverse. Station C in which sulfuric acid and magnesium were to react with each other is a chemical change because it formed gas bubbles and changed colour. Station D where hydrochloric acid and Bromothymol blue were the materials is a chemical change because it changed to the colour yellow and looked difficult to reverse. In Station E where NaCl solution and AgNO3 solution were the materials is a chemical change because the reaction

The purpose of this lab was to find out how gaviscon reacted with different salt solutions. Sodium Alginate is a compound that forms with the Gaviscon and forms a “raft” and blocks all the stomach acid from traveling up the esophagus.

Conclusion The mass of the recovered copper was 5.22g, much greater than the initial mass of copper, 2.09. The number of moles of the recovered copper was calculated to be 0.0821mol while the number of moles of the initial copper was calculated to be 0.0329mol. The percent of copper recovered was calculated to be 250.%, and the percent error of copper recovered was calculated to be 150.%. From what seems to have been an increase in copper from the initial mass to the recovered mass, it can be assumed that the copper solid recovered at the end of the lab contained compounds other than the expected copper, as there was no way for additional copper to be introduced into the reactions.

To understand this lab there is knowledge prior to the lab that was taught. A physical change is a change affecting the form of a chemical substance but not its chemical composition. Physical changes can be used to separate mixtures into their component compounds. An example of a physical change is a popsicle freezing in the freezer. A chemical change is any change that results in a new formation of chemical substances. An example of a chemical change is when rust forms on nail. The signs to look for to see if there is a chemical change are color change, odor change, production of bubbles and gas, production of heat and light, and production of a precipitate. If any of these signs happen in the lab it is a chemical change. The question for

In the previous lab, it was found that ionic substances are soluble in water due to the dipole-dipole attraction between the partially negative oxygen and partially positive hydrogen within the water molecule to the ions within the ionic compound. It is also a conductor in water due to the dissociated, free-floating ions that create charges within the solution. Also, they have a melting point above 5000C due to the magnitude of the bonds held between atoms. Lastly, they react with .1M NaOH which is a strong base since ionic compounds are formed by an acid-base reaction. While conducting the various tests to determine the type of bond for the chemical in container 5, it was shown that it meets all of the requirements for it to contain ionic bonding. It was soluble in water, acted as a conductor in water, had a melting point above 5000C, and reacted with .1M NaOH. This reaction between the substance and NaOH was shown when the solution became cloudy which indicated that a solid precipitate was in

Meaning, compounds with the same type of bonding tend to be soluble with one another. Polar substances would dissolve in polar solvents such as water, however, would not dissolve in non-polar solvents. Non-polar substances dissolve in non-polar solvents but do not dissolve in polar ones. Most ionic compounds are able to be dissolved in water as the water molecules hydrate ions. For an ionic compound to be dissolved, the water molecules must stabilize the ions, which thus would result in the separation of the ionic bond to form a solution. Water is a polar molecule, it has a permanent dipole. The oxygen atom has a partial negative charge whilst the hydrogen atom has a partial positive charge. When an ionic substance is placed in to the water, the water molecules would quickly attract the charged ions from the substance. They then become free to move about. However, this only occurs when the attractive forces between the water molecules and ions are stronger than the attractive forces within the ionic compound. CaOH is a slightly insoluble compound, the solubility of CaOH is approximately 0.189 g/100 mL of water at 20. A more soluble ionic compounds solubility such as NaCl is only 35.7 g/100 mL of water at 20°C. CaOH is only slightly insoluble as calcium and oxygen are +2 and -2 ions in

In this lab section we talked about how elements on a periodic table are organized by increasing atomic number and we focus on six metals which are called Lithium,sodium,potassium,rubidium,cesium and francium. In which we observed how each metals reacted inside the water. To add on this lab focused on electrons and valence electrons. In which we learned that in a period table left to right it decreases and from top to bottom it increases. Before doing the lab we watched a video based on the lab we did. Then we wrote the observation we saw in video which were:

In our first Chemistry lab, I was tasked with using volumetric tools and devices in order to find the density of water, a sugar solution and determining the amount of beads within a container while maintain the appropriate significant figures. The main skill goal of the experiment was to gain knowledge on the use of volumetric measuring tools such as beakers, graduated cylinders and volumetric pipets. This experiment was designed for us to learn how chemistry lab equipment is used and maintained, while also giving us the opportunity to use this equipment in several uniquely designed experiments. This makes the experiment very useful in our knowledge of how scientific labs operate and how chemistry experiments are conducted through the proper

Ionic-It was just like any other day when Maggy and Nesa spotted a sulfur atom that hadn't been bonded with. The sulfur was a perfect home for Maggy and Nesa because it would satisfy the octet rule, the ultimate goal of every atom(with a few exceptions). They remembered learning about the lewis dot diagram in biology class which showed how the process was possible. From that class they also learned that magnesium usually has an ionic bond with a non metal as well[3,4,7,9]. So, when it came time to interact with he sulfur atom, the interior electrons kicked out Maggy and Nesa. With the twins gone, the two atoms bonded due to their charges being opposite[10]. This ionic bonding gave properties to both of the atoms that they would have never