Specific Heat of a Metal Michael Diaz Ms. Zhort Performed: October 3, 2013 Due: October 24, 2013 Period: 1 Lab Partner: Rocco & Asha Objective: This lab was meant to teach us how to find the specific heat of a metal sample. Materials: * Specific heat set * Balance * Thermometer * Tap Water * Hot plate * Polystyrene cup and a lid * Stirring rod * 250 mL beaker * String (about 15 cm) Procedure: 1. Fill a 250 mL beaker approximately half full of water. Place the beaker of water on a hot plate. Begin heating the water to the boiling point.
Sodium Hydroxide + Hydrochloric Acid Sodium Chloride + Water NaOH(aq) + HClaq → NaCl(aq) + H2O(l) Variables Independent The independent variable of the experiment was the amount of sodium hydroxide that we added to the acid. To keep the variable controlled we would measure 1 ml of the sodium hydroxide and pouring that to the hydrochloric acid. Dependent The dependent variables of the experiment were the temperature and the pH number of the mixture. To control the pH and temperature use the electronic probe and data logger. Controlled The controlled variables of the experiment were: A.
Gently stir the pellets until the acid is dissolved by shaking the the apparatus. Lift the calorimeter lid and wash out its contents and the thermometer. Repeat this experiment using 50.0 mL of 1.0M acetic acid. Repeat experiment using 25.0 mL of each 2.0M sodium hydroxide and 2.0M acetic acid. Data Table(s): Reaction equation Mass of solid NaOH Initial Temp.
PURPOSE/INTRODUCTION The purpose of this experiment is to produce visible emissions from heating different metal fluorides with a Bunsen burner. The hypothesis is that by warming the different metal chlorides, the different elements found in each chloride will produce a different color when placed in the flame. We will also produce a table of our findings with our information we recorded from the results gathered in this lab. In the preceding discussion, we will be testing different metal chloride reactions when a flame is introduced to them. MATERIALS * One Bunsen burner * 1 gram of Sodium Chloride * 1 gram of Potassium Chloride * 1 gram of Lithium Chloride * 1 gram of Barium Chloride * Nichrome wire (wire with a loop) * 0.4 grams of water * Protective eyewear * Lab gloves Barium is a toxic metal, be sure to wear gloves and goggles when handling this material, also if using a Bunsen burner be sure to turn of the gas.
Matter and Chemical Reactions Pre-Lab Preparation: Purpose: The reason we are doing this lab is because we are trying to see what will happen. When you put copper and silver nitrate together. Also after that I will see if any elements reacted and if so which ones and what is the name of the compound they formed. Hypothesis: If I put the copper into the silver nitrate, then it will make some type of solid. Materials: copper wire AgNO3 solution Sandpaper Stirring Rod 50-mL Graduated Cylinder 50-mL Beaker Funnel Filter Paper 250-mL Erlenmeyer Flask Ring Stand Small Iron Ring Plastic Petri Dish Paper Clip Bunsen Burner Tongs Pre-Lab Questions: 1.)
A melting point will be ran on the aspirin when completely dry. A capillary tube containing the dry aspirin will be placed into the melting-point apparatus. This process is to determine the melting point range of aspirin. First, a hot water bath was created with a 400. mL beaker on a hot plate. The temperature was raised to 70 degrees Celsius and 4.419 g of salicylic acid was measured out on a balance and transferred into a 125. mL Erlenmeyer flask.
It is called the heat of solution of solid NaOH. From our calculation it known that ∆H3 is -58.6 kJ/mol. When ionic solid dissolves in water, heat was librated. Reaction 1: Dissolving solid sodium hydroxide in water. NaOH(s) ---> Na+(aq) + OH-(aq) + heat Reaction 2: Reaction of sodium hydroxide solution with dilute hydrochloric acid.
Halogens Aim: To find the difference in appearance, reactivity and solubility of Halogen elements. Materials: * Chlorine * Bromine * Iodine * Chlorine solution in water * Bromine solution in water * Iodine solution in water * Test-tubes * Rubber bungs * Potassium chloride solution * Potassium bromide solution * Potassium iodide solution * Silver nitrate solution * Cyclohexane Method: Experiment 1- Appearances and solubilities of halogen elements 1. Observe the elements: Iodine, Bromine and Chlorine at room temperature and record their physical state and color. 2. Boil or sublimate (if necessary) to observe each element in gaseous state, record color of vapor.
1ml of concentrated H2SO4 was then added to the tube and the solution was continuously stirred to dissolve all the triphenylmethanol. Using a Pasteur pipette, the sulfuric acid solution was then transferred to 2ml of ice cold methanol. Crystallization was induced by scratching the tube with a glass rod. The crystals were collected by vacuum filtration on a Hirsch funnel. After filtration, the crystals collected were washed thoroughly with water and then dried with filter paper.
In this electrolytic cell both electrodes are copper and the electrolyte is 0.5 M H2SO4. During electrolysis, the copper electrode (anode) connected to the positive pin of the power supply loses mass as the copper atoms are converted to copper ions. The loss of mass may be visible as pitting of the surface of the metal electrode. Also, the copper ions pass into the water solution and tint it blue. At the other electrode (cathode), hydrogen gas is liberated at the surface through the reduction of hydrogen ions in the aqueous sulfuric acid solution.