Sodium chloride Essays

Historic Background Sodium chloride is also known as salt. The molecular formula for sodium chloride is NaCl. NaCl has a molar mass of 58.443 grams. Sir Humphry Davy discovered sodium chloride in 1807. He was able to extract sodium from its compounds, which included sodium’s connection with chlorine. Sodium does not appear by itself naturally, so it was important that Sir Humphry Davy figured out how to get sodium by itself. The salinity in the ocean is in large part to sodium chloride. A physical description

The purpose of this report is determine if sodium chloride is a viable option as a deicer on winter roads. To determine this, one must compare a multitude of factors. In this lab, the freezing point depression of water, enthalpy of dissolution, cost, and environmental impact will be discussed. A large factor in how effective a substance is as a deicer is it’s ability to decrease the freezing point of water. If the freezing point of water can be lowered, the outside temperature must be much colder

Knowing the Interrelationship Between the Consolidation of Sodium Chloride Mixtures and Their Densities Chemistry 1A Lab 5pm Th, Department of Chemistry, California State University Fresno Professor Nimavat Experiment Conducted: 1/25/18 Report Submitted: February 15th, 2018 Alex Luna* and Ellen Introduction: Density is defined as the ratio between mass and volume or mass per unit volume. It is a measure of how much stuff an object has in a unit volume. This report discusses an experiment to find

concentration of Sodium Chloride (NaCl) solution affects the volume of the gases (Oxygen gas and Chlorine gas) at the anode during the electrolysis of sodium chloride solution. In my previous chemistry classes, I have learnt that concentration affects the majority of the gas produced at the anode. This made me wonder, how does the ratio of oxygen gas to chlorine gas produced at the anode vary at the electrodes. This made me formulate the research question: How does the concentration of Sodium Chloride solution

OBJECTIVE The objective was to determine the relationship between the reactants calcium chloride and sodium iodate their product calcium iodate. INTRODUCTION Experiment six was about the relationship between reactants and products. In this experiment the relationship of calcium chloride and sodium iodate in a reaction that produces calcium iodate. The calcium chloride and the sodium iodate undergo a precipitation reaction to produce calcium iodate. The goal is desirable for gaining understanding

alkalinity and increasing sodium chloride concentration had on the yield of lysozyme crystals through crystallization. The constants for this process were sodium acetate at a concertation 0.05 M for every well in both rows, along with the concentration of polyethylene glycol (PEG) being set at 10% for every well in both rows. The two rows of wells that were tested deviated in alkalinity, row A having a pH of 4.5 and row B having a pH of 4.8, along with the sodium chloride concentration of each well

substance “2” was proven to be Tin (II) Chloride and the Unidentified substance “4” turned out to be Sodium Chloride. The conclusion that substance “2” was Tin (II) chloride could be proven due to the fact that it reacted with Zinc and Sodium Hydroxide. When Tin (II) chloride reacted with Zinc, it began bubbling. This occurred because there was a single replacement reaction between Tin (II) Chloride and Zinc. Zinc is far more reactive than Tin (II) Chloride, making this a very likely conclusion. In

of each solution according to its concentration. Assuming that the density of each solution is approximately 1 g/mL, the mass of each solution will be 600 grams.(mass of solution=volume of solutiondensity of solution) In order to calculate the sodium chloride mass required for each solution use the following formula: mass of solution=mass of NaCl 100concentration of solution. For the solution of NaCl 5% are need 30 g NaCl and 570 mL water; for the solution of NaCl 8% are needed 48 g NaCl and 552 mL

one form into another, mixtures can be separated or made, and pure substances can be decomposed, but the total amount of mass remains constant. For example, from our experiment in the lab, we observed mass of the mixture of aqueous Sodium Sulfide and aqueous Zinc chloride turned white color. After the filtration, and all the water was evaporated, we measured the mass very close to what we had started at the beginning. The error in mass occurred because of the remained residue (solute) in the beaker

organic solvents, while if it were silicon dioxide it would fail both solubility tests for organic and aqueous solvents. When doing the flame test, if the flame colour of the substance is yellow then it is either sodium chloride or sodium carbonate. The difference between sodium chloride and sodium carbonate is that the first is pH neutral while the latter is basic, which means a pH test would need to be conducted to

of a copper (II) chloride and sodium chloride mixiture was attempted. The main aim was to separate the compounds from eachother while receiving as much of the original mass of both substances as possible - in perfect conditions the original mass will be received after seperation. Many techniques were considered but dissolution, filtration and evaporation proved to be easiest and most reliable in a school environment with school equipment. The copper (II) chloride and sodium chloride mixture was dissolved

Hydrochloric Acid and Sodium Carbonate because it was the only reaction that produced a gas release. Unknown A and C produced the only yellow, brown precipitate just as the reaction between Sodium Carbonate and Silver Nitrate had previously. This led to the conclusion that A is Sodium

was burned, a bright, vibrant orange flame color resulted. According to the lab manual chart, a compound that lets off an orange colored flame contains sodium (1). To confirm that the compound did in fact contain sodium, 4 additional flame tests were performed: sodium, potassium, magnesium and calcium. As seen in Table 2, both the unknown and sodium produced a consistent orange flame. Potassium omitted purple light, magnesium showed no change in color, and calcium produced a red light. When heated

was completed, it was found that the identity of the white compound was Sodium Nitrate. 1. Introduction The objective of the experiments was to determine the identity of an unknown compound in order to properly dispose it. The process of disposal is very important when dealing with chemicals. Some chemicals are very

sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted. This shows that these substances conduct electricity as a solid. The next test was conductivity as a solution. From our findings, sucrose had poor conductivity, while ascorbic acid and sodium chloride had good conductivity. Ascorbic acid conducts

I. INTRODUCTION This report discusses an experiment, the objective of which was to determine the classification of six known chemicals: sodium nitrate, barium chloride, silicon carbide, naphthalene, urea, and antimony and two unknown chemicals XIa and XIb. Since each type of chemical (ionic, molecular, macromolecular and metallic) has its own set of properties, by testing these properties and finding them out for each chemical, it was possible to classify them. The properties tested during this

DESCRIPTION  A simple reaction, followed by isolation of the desired product from the solution, will illustrate a typical application of extraction.  Some organic acids are liquid and are soluble in water as indicated. The sodium salts of these acids are ionic compounds that are also very soluble in water. If an aqueous solution of one such salt is acidified with a strong mineral acid, the much weaker organic acid is produced.  The weak organic acid is largely un-ionized in the aqueous solution

1305-008 07 August 2017 Sodium (Na) Sodium has an atomic number of 11 and an atomic mass of about 23. It has a symbol on the periodic table of Na. It is a silvery-white metal found under the alkaline metals. Sodium is the “sixth most common element on earth and makes up about 2.6% of earth’s crust,” (RSC 1). It is usually found in compounds, including salt, sodium chloride (NaCl) or more commonly known as table salt. It is also used in baking soda, sodium bicarbonate (NaHCO3). Sodium is used to “de-ice

5-aminotetrazole monohydrate: In a 250 ml round-bottom flask equipped with a condenser for refluxing (90 °C) and a magnetic stirring bar, 5.00 g (5.95 mmol) dicyandiamide (three times crystallized), 7.47 g (11.9 mmol) sodium azide and 11.00 g (17.8 mmol) boric acid and 100 ml of water is added and allowed to reflux for 24 hours, after the completion of the reaction, until the solution pH to about 2 to 3 as hydrochloric acid 37% is added (about 12 ml) Then the reaction mixture was cooled in a refrigerator

Before the water reach to the consumer 70% of the permeate water goes to potabilization or remineralization while 30% goes the demineralization. In potabilization plant four chemicals are added which are: Sodium hypochlorite It is added for final disinfection of treated water Sodium fluoride This chemical must be existed in the potable water because when it dissociate fluoride is produced as shown in the chemical reaction: NaF → 〖Na〗^++ F^- The fluoride used to protect the teeth in two ways: