Potassium And Sodium Lab Report

When calcium chloride, sodium bicarbonate, and phenol red are put into a bag and mixed up the type of reaction that occurs is a chemical reaction for the following reasons. Things that indicate that a chemical reaction has occurred are color change, formation of precipitate, formation of gas, and energy transfer in which three of them took place in the reaction of calcium chloride, sodium bicarbonate, and phenol red. The three indicators in this experiment were: a color change, formation of gas, and an energy transfer

Sodium bicarbonate has a molar mass of 84.0 g/mol. It has a melting point of 50°C and can be an irritant.

The purpose of this experiment was to mix Alka-Seltzer with Hydrochloric acid in order to analyze Sodium Bicarbonate as an active ingredient in the Alka-Seltzer. The mixture will contain hydrochloric acid to only see the composition of Sodium Bicarbonate in the tablet once it reacts. The amount that reacted allowed us to determine how much of it is present in the tablet. The amount of sodium bicarbonate will be measure by using the ideal gas law PV=nRT. The experiment will be conducted in the lab, therefore we are going to use room temperature which ranges from 15 to 26 degrees celsius. At room temperature pressure ranges from 12.8 to 25.0 millimeters mercury according to its corresponding room temperature.In the ideal gas equation R is 0.08206latm/mol k which is a constant. Once we have those values we can calculates the number of moles that reacted in the mixture by solving for the missing value. With the number of moles we are able to find the mass in grams which is what will potentially tell us the composition of Sodium Bicarbonate in a tablet of Alka-Seltzer.

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.

The previous steps were repeated for the remaining known salts and also the two unknown salts. 9. All flame colours were observed and recorded. 10.

In a test tube, 0.5mL of the sample will be added with 0.5 mL of water and shaken vigorously. Take note for its solubility by parts (0.5mL is one part). Keep adding parts of the solvent until the sample is soluble. If not, add until ten parts of the solvent and determine its solubility. To separate test tubes, water will be replaced with ethanol, chloroform, ether, and acetone as solvents. Same procedures were

The purposes of this experiment were to model a bimolecular nucleophilic substitution reaction between potassium hydroxide (KOH) with 1-bromopropane and determine whether it follows a second-order rate law mechanism. A rate constant of 0.0684 M-1 min-1 was obtained for this reaction at 45.1°C, which was determined through equilibrating the reaction and performing titrations of 0.390 M KOH with 0.1000 M hydrochloric acid (HCl). The activation energy calculated from class data was 50.188 kJ/mol, which deviated largely from the literature range value of 72.80–83.76 kJ/mol. It was concluded that the reaction was consistent with the predicted SN2 mechanism, based on the regression of a trendline.

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

An error that occurred during within this lab experiment was not weighing the beaker at the same, tampering with the results. There was chaos within the first beaker it could not be be put on the plastic balance. Making a quick decision that was not in the procedure, which was wait 3 and half mins before weighing the becker instead of 1 min after boiling out water and the cardondixode gas out. this caused the lab experiment to had a later start time. The time of weighing the sodium acetate was effect within this error caused the results to be different.

CH 204 – Introduction to Chemical Practice Experiment 1- Qualitative Analysis of Cations Anusia Mansukhani Andrea Martinez TA: Joseph Guerrera September 28th,2017 RESULTS & DISCUSSION The purpose of this lab was perform qualitative analysis an unknown solution and determine if the unknown cation. It was a combination of either lead and calcium, lead and barium, silver and calcium or silver barium. This experiment was divided into three parts.

he Stream Team tested the nitrate levels, air temperature, dissolved oxygen, pH, turbidity, and phosphate in the stream. The Nitrate test the average of all the tests taken where .25 mg/L.The air temperature of the day the test was taken was 11.7 degrees Celsius. The dissolved oxygen levels of the stream the day of testing were 5 mg/L.The average pH levels were 7.85. The turbidity of the stream the day we tested was 10 NTU.The phosphate level for the was not available because all tests performed showed there was no phosphate in the stream. The stream tested was Cole Camp Creek.Beginning at 0857.All of the tests were taken from circulating water.

General Chemistry Lab: Lab report For the materials list and procedure, see attached. The purpose of this lab is to understand the difference between chemical and physical changes and apply the knowledge to different labs to figure out what the change is whether it be physical or chemical. Practicing lab safety, goggles taking precautions with hot materials, etc. For each of all six of the experiments it was concluded for each one whether or not it was chemical or physical, for the first lab, copper sulfate and water were mixed , the mixture was then left to dry and formed larger, glass-like crystals, this was concluded as a physical change because there was no change in molecular structure to make it a chemical change.

Stoichiometry has many uses in the real world. In the chemical industry and in professional scientific experiments, scientists use stoichiometry to save money. Scientists use stoichiometric calculations to determine the amount of a substance they need to purchase for a specific reaction. There are four possible reactions that can occur when sodium bicarbonate thermally decomposes. In this lab, stoichiometry was used to find out which balanced chemical equation out the four best represents the thermal decomposition of sodium bicarbonate.

In this experiment, the laboratory instructor prepared an unknown mixture containing soda ash. Soda ash or Crude Sodium Carbonate with a molecular formula of Na2CO3 is a mixture that is frequently used as commercial neutralizing agent. Titration using standardized acid (HCl) to the Bromocresol

The purpose of this lab was to separate a mixture of iron, sand, and salt into each of its individual compounds or elements. The iron had a magnetic property so the group was able to separate the iron shavings from the mixture using a magnet. Then the group used filtration to separate the sand and salt. When the mixture was filtered, salt water went through the filter and the sand stayed in the funnel, this lead to the conclusion that particles of sand are larger than particles of salt and water. Then the group distilled the salt water mixture so that the water evaporated and the salt was left, this lead to the conclusion that the boiling point of water is lower than the boiling point of salt. The group had hypothesized that the mixture could