Chem 103 Project Lab Essay

In this Chemistry Lab the main objective is to perform accurate chemical analysis for the quantity of elements and compounds in a sample. There will be a compound made then synthesized. The methods used were acid-base titrations, redox titrations, gravity filtration, and distillation. General conclusions included

The mass percent of ascorbic acid in the sample is given by dividing the calculated mass of ascorbic acid (0.414060408 g) by the calculated mass of the sample (0.5500 g) and multiplying the quotient by 100%.

The empirical formula is base on the ratio of moles of silver and the moles of oxygen. The empirical formula needs to show the simplest integer number. For trial one the ratio between moles of silver and moles of oxygen is 5/4, and the ratio between the moles of oxygen and moles of oxygen is 1. According to the law of empirical formula, there can not be a fraction in the formula. So, the empirical formula is Ag5O4.

To calculate the percent by mass, we are to take the mass in grams of a particular salt and divide it by the mass in grams of the original sample, and then multiply it by 100.

pH was recorded every time 1.00 mL of NaOH was added to beaker. When the amount of NaOH added to the beaker was about 5.00 mL away from the expected end point, NaOH was added very slowly. Approximately 0.20 mL of NaOH was added until the pH made a jump. The pH was recorded until it reached ~12. This was repeated two more times. The pKa of each trial are determined using the graphs made on excel.

The proof (twice the % alcohol) starts at its maximum and goes down (as the alcohol evaporates). If we start with a high concentration of alcohol, we will get the azeotrope (95% alcohol, 5% water) for a while, then the concentration will decrease.

The luminous yellow flame is smoky because no air is entering the burner and hydrocarbon is converted into carbon dioxide

To begin Lab 7 of Chem 115, a clean and dry porcelain crucible and its cover were obtained. Next, an iron ring was attached to a ring stand. A clay triangle was placed on top to the ring and a Bunsen burner was placed under the ring. Following the setup for the experiment, the crucible and its cover were placed on the clay triangle and were heated for about five minutes. After, the burner was turned off and the crucible and cover were left to cool to room temperature. Once the crucible and its cover had reached room temperature, tongs were used to move them to a wire gauze. Using the wire guaze, the crucible and its cover were transported to an analytical scale to weigh and record the mass of it. Next, a strip of magnesium was obtained and

When the reaction was complete, we remove the aluminum and separated the copper from the solution to weigh the metal and calculate the number of moles of copper in the sample. After that, we found the mass of chlorine from subtracting the mass of copper from that of the dehydrated compound and determining the number of moles of chlorine. The mole ratio of Cu: Cl: H2O gives us the empirical formula of the

An aliquot (5 mL or 500 ml) of sample was filtered through a Whatman Anotop PTFE syringe filter (0.2 µm) and the concentrations of target PHCs were quantified using HPLC-MS/MS. Question: Why not preconcentration such as passing 200 ml through a cartridge to improve sensitivity? How does this method compare with published SPE techniques?

Purpose: In this lab, we will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate.

In this sample calculation, the percent error of the eutectic composition is calculated. Percent Error= Theoretical Value- Experimental ValueTheoretical Value100 % Error of Eutectic composition=0.45-0.5180.45100 % Error of Eutectic composition=15.11%

When it comes to chemistry, compounds will always more than one elements. These elements will always have a mixture of a certain proportion by mass for a given compound. When dealing with compounds it is important to find the empirical formula because it helps to show all the known elements of that compound and they display the smallest whole number of moles and the number of atoms each element contains. Empirical formulas are helpful for finding an

Advanced Placement Chemistry is a college course that students can take in high school. For some students Advanced Placement Chemistry is one of the most challenging classes, because it could help the student’s future career. Before taking Advanced Placement Chemistry, the student takes Chemistry, which is a summary of the scientific world. In Advanced Placement Chemistry it gets into more detail or takes another step into the scientific world. In Advanced Placement Chemistry students will learn more about the periodic table, chemical equations, and formulas.

This model approach the accurate method of estimating by grouping the element with same unit rates or common unit of measurement together in the standard elemental format. As the a basic set of