AP Chemistry P2 Experiment 2: Formula of a Hydrate 9/24/2013 Purpose: Calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate. Procedure: 1) Set up ring stand with ring clamp, clay triangle, crucible with lid, and burner. Adjust the height of the ring stand. 2) Dehydrating Procedures: 3. Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid.
Observe the color change while it is being heated. After observing the color change, find the mass and moles of the hydrate. Then find the mass and moles of the water eliminated. And lastly find the mole ratio of water to hydrate. For part 2, do the same thing as part 1 except use an unknown hydrate and calculate the percent mass of water in an unknown hydrate.
3. Set up the ring stand, iron ring, and clay triangle to support a crucible over the Bunsen burner. 4. Place the clean and empty crucible with its cover on the clay triangle. Turn the Bunsen burner on and ignite it.
Introduction A titration was carried out in this experiment to find the concentration of hydrochloric acid is an unknown solution. The aim of this experiment is to determine the number of moles of sodium hydroxide in hydrochloric acid and then to determine the number of moles of sodium hydroxide present in gastric juices. Titration, or volumetric analysis, is a common laboratory procedure for the analysis of substances and solutions. In a titration, the analyst determines the volume of a solution, called a titrant, that reacts exactly with a known weight or volume of another substance. This reaction is carried out by adding a solution of reactant hydrochloric acid from a burette to a solution of sodium hydroxide until just sufficient of hydrochloric acid has been added to react with all of the sodium hydroxide.
Nathan Bahn Beer’s Law Study Lab Introduction: In this lab, we used a spectrometer to observe the transmittance of light at a certain wave length. We experimented to see if the molarity of a solution changes the transmittance of light and the absorbance of that light by the solution. By observing the percent transmittance and the amount of light absorbed, we can calculate the amount of color absorbing components in the solution. Through this process is how we are able to discover the amount of copper in the solution. Experimental Procedure: 250 mL of the copper solution was made by creating 100 mL of the solution, reacting CuO with HNO3, and then diluting to the mark of 250 mL.
Gravimetric Determination of Sulfate Purpose The purpose of this lab is to determine the percentage of sulfate in the hydrate by precipitating the sulfate as barium sulfate. Materials Filler paper Sodium sulfate Graduated cylinder Bunsen burner Watch glass Beakers (250 mL, 400 mL) Rubber bulb Graduated pipette Beaker tongs Funnel Filter Paper Sodium Sulfate Drying oven Wash bottle Stirring rod Silver nitrate Hydrochloric acid Distilled water Small test tube Procedures First, .4861 grams of sodium sulfate was placed into a clean 400mL beaker. Exactly 200mL of water and 1mL of HCl was added to the same beaker. A watch glass was placed on the beaker and the solution was heated using the Bunsen burner to a gentle boil. The watch glass was removed with the beaker tongs.
The calorimeter was designed in 1780 by a chemist named Antoine Lavoisier with help from a mathematician by the name of Pierre Simon de Laplace. Now a widespread tool, we will be using the calorimeter, and our knowledge of equations to find the specific heat of zinc and aluminum. OBJECTIVE/GOAL In this experiment we will Measure the mass and temperature of water in a calorimeter Heat a metal sample of a known mass to a specific temperature Calculate the change in water temperature caused by adding the hot metal sample Calculate the specific heat of the metal using your mass and temperature data PROCEDURE 1. Prepare a data table as directed in the Analysis. Safety goggles and lab apron must be worn for the experiment.
The term Cp is the specific heat of the material (at constant atmospheric pressure). Different materials have different specific heat values. The units of specific heat are : Joules/gram deg – C. In this lab we will find the specific heat value of Zinc and compare it to accepted values.This will do by heating a mass of Zinc up to the temperature of boiling water and placing the hot metal into a cup of cold water. The thermal energy that the zinc loses goes into heating up the water in the cup. By knowing the starting temperatures and the final temperature of the water and the zinc, the specific heat of Zinc may be easily obtained.
In this experiment we are going to measure the solubility of KNO3 in water at various temperatures. Results can be reported in different ways ranging from grams or salt dissolving in a milliliter of water to grams of salt in 100 mL of H2O In general, systems tend to go to a state of disorder or to a state of greater entropy. During the dissolving process, the particles of the solid become randomly distributed through the solvent in sharp contrast to their orderly arrangement in the solid state. Ion the solid state there are strong forces holding these particles together. In order to dissolve the solid, energy must be expended to overcome these forces.
The consecutive evaporations and condensations allow for the separation and purification of compounds with similar boiling points. Boiling points are directly proportional to pressure; therefore as the pressure is decreased the boiling point will also decrease. Compounds with very high boiling points can be distilled much easier if a vacuum is applied. Vacuum distillation is a common technique which allows for the distillation of high boiling compounds under mild conditions. Both the simple and fractional distillation apparatus can be performed under vacuum by attaching the vacuum line to the fume hood vented adapter near the collection