The synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride. The synthesized compound formed was used to perform another flame test and the chloride anion test, which further solidified the identification of NaCl as the ionic compound. Introduction The purpose of the experiment was to identify unknown ionic compound
The purpose of this lab is to focus on how to make zinc iodide in a different way using compounds instead of elements, which are barium iodide and zinc sulfate. We will see if the reaction between these two compounds will occur and make a prediction by writing a chemical equation. The procedures for this lab are to place a small test tube inside a 50mL beaker and weigh it. Then, using a spatula, add 0.45±0.03 g of zinc sulfate heptahydrate into the small test tube and record the mass. After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid.
1. 15.8 g of KCl is dissolved in 225 mL of water. Calculate the molarity. 2. Calculate the mass of KCl required to prepare 250. mL of 0.250 M solution.
0.00079 moles EDTA4- c. 0.00079 moles ZnI2 d. 0.0517 grams of ZnI2 are in the sample e. 0.0517/0.237= 21.8% f. Error Is 6.34% Lab Report: Part 1: In this lab we used the following supplies: * Zinc Iodide * Na2H2EDTA(s) * Calmagite indicator solution * pH 10 buffer solution * 6M Acetic Acid * Unknown Zinc Compound The main purpose for this part of the lab was to determine the amount of zinc ion in a sample of ZnI2 by titration. The two types of zinc: * Zinc iodide made by zinc and iodine * Commercially purchased zinc iodide (the
To make the clay, 250 mL of distilled water was heated in a 600 mL beaker to 70° to be used as a hot water bath for the Erlenmeyer flask. 40 mL of distilled water was added to the flask along with .80 g of FeCl3, .40 g of FeSO4-, and .30 g of Bentonite. Using tongs, the flask was stirred in the hot water bath to disperse the iron compounds and the clay. The flask was then taken out of the hot water bath and 20 mL of NaOH was added drop-wise. After it was properly cooled, the solution was equally distributed to four centrifuge tubes and centrifuged for 5 minutes.
The test for Sodium Bicarbonate included mixing that with HCl. After doing this experiment bubbles would form in the solution. This was CO2 being released. This reaction is a way of testing for Sodium Bicarbonate. BACKGROUND: For these experiments a 96-well plate was used.
(4 points) q = m × c × Δt Given: q=? m = 34.720g c = 4.18 j/(g x °C) Δt = 41.6°C - 25.2°C = 16.4°C q = (34.720g) (4.18 j/(g x °C) (16.4°C) q = 2380.13j You are trying to figure out the energy change of the water which is the surroundings in the lab. To do that you must take the mass of the metal, which for me was Aluminum, and multiply it by the heat capacity of the water, which was given, then multiply that by the change in temperature, which is the final temperature of the mixture
iLab 1: Separation of a Saltwater Solution Devry University BIOS135 Professor Subbhalakshmi, Dhalladoo 11/01/14 Introduction The purpose of this lab experiment was, to practice using the scientific method and separate a mixture of salt and water based on the physical properties of each component. I will examine more closely the physical properties of matter. To do this procedure we must evaporate the water and leave behind the salt from the solution. In 103c the water evaporates and behind left is the salt. From this information, the percentage of salt verses water ions can be determined Ions are also produced in the liquid or solid state when salts interact with solvents (for example, water) to produce "solvated ions," which are more stable, for reasons involving a combination of energy and entropy changes as the ions move away from each other to interact with the liquid.
Ally Emerson Lab Report H. Chem. Period 3 1-11-15 How does mixing distilled water, iron, and copper (II) sulfate and then boiling the mixture help us determine the theoretical and percent yield of copper after the chemical reaction? Partner: Naomi Purpose: To determine the theoretical and percent yield of copper after a chemical reaction between distilled water, iron, and copper (II) sulfate. Hypothesis: There will be around 2 grams of copper left, which will equal a 89% yield. Materials: scale, filter paper, weighing paper, distilled water, copper (II) sulfate, iron, beaker, tongs, drip, and a funnel.
Record several points of pH and NaOH added (especially near equivalence point) to be use later to prepare a titration curve. Observations and Results Part I: Solution | pH | 0.1 M HCl | .70 | 0.1 M NaOH | 13.30 | Part II: Volume of 0.1 M NaOH at equivalence point: 35mL pH at equivalence point: 11.45 Molarity of the Unknown Acid A (HCl): 2.0 x 10-4 Discussion In this lab, we found out that water self ionizes itself into hydrogen ion and hydroxide ion naturally to a very small extent. An indicator, in an acid base reaction, is a substance whose color changes over a particular pH range. Phenolphthalein is an example of an indicator which changes from colorless to pink as pH goes from 8 to 10. We plotted the pH against the amount of base added producing a