Nacl2 Lab Report

Introduction The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

Ankur Sindhu Sep 20, 2011 CHEM 182-DL1 Prof.: Dr. Nidhal Marashi Lab 1: Colligative Properties & Osmotic Pressure Purpose: The purpose of this laboratory was to gain an understanding of the differences between the freezing points of pure solvent to that of a solvent in a solution with a nonvolatile solute, and to compare the two.

We did Lab 2 part 1, first we found the weight of the graduated cylinder and 10 ml of water. Then we found the weight of the graduated cylinder. After that we found the we found the weight of the 10 ml of water by subtracting the weight of the

Results & Discussion Day One Results Trial | Volume H2O(ml) | Grams NaCl | Molarity of Solution | Final Freezing temperature(C) | Theoretical Change in Temperature(C) | 1 | 10 | 0.255 | 0.436 | -1.5 | -0.45 | 2 | 10 | 0.255 | 0.436 | -1.2 | -0.45 | 3 | 10 | 0.250 | 0.428 | -1.2 | -0.44 | 1 | 9.9 | 0.502 | 0.868 | -3.6 | -0.89 | 2 | 9.9 | 0.499 | 0.863 | -3.2 | -0.88 | 3 | 10 | 0.503 | 0.861 | -3.3 | -0.88 | Calculations for Day One Tf=(mass solute)(i)(molarity of solution) Sample Calc: (.512)(2)(.863)=.8837 Molality=mols solute/kg of solution Sample Calc: 0.499gNaCl/mm NaCl (58.44g)=.00854mol=> .00854mol/.0099kg=.863M Analysis Day One Through our data acquisition on day one our predicted values for the change in temperature of our NaCl solution in water was slightly off. This was most likely due to recording the freezing temperature sometime after the precise moment of the solution freezing. However, we predicted that as we doubled our concentration of NaCl in solution the freezing point depression would also double which is consistent with our results. Through our day one experiments we were able to better understand the ability of NaCl as a deicer by understanding how the freezing point depression changes based on concentration. We could further test these results by testing with different concentrations of NaCl.

Base 8.93 Pastel green A Neutral 7.14 Very Pale Pink B Acid/Base/Neutral pH Reading Color of Extract Solution Acid 4.26 Light Pink C Acid 2.22 Pink D Base 10.05 Light green E 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.

Deicer Analysis of MgCl2 Dalena Khothsombath *† Group Members: James Deringer, Jeff Tanaka, and Yang Zhao Group 3 “I pledge that this report, the data in it, and interpretations are my work, except where referenced. I have neither obtained nor given aid on this assignment outside of data discussions with my lab team. “

The first part of the lab began by one lab member adding 10.0 mL of DI water to a test tube while another lab member obtained a beaker full of ice and salt. After both these steps were complete the test tube was put in the beaker full of ice. Immediately following the test tube be being placed in the beaker, a temperature probe was inserted into the test tube. The initial temperature was recorded and after the temperature was recorded in 30 second increments. Once the water exhibited supercooling and then remained consistent at .1 °C for 3 readings it was determined that the water had froze and formed crystals. Evidence that crystals formed allowed for it to be confirmed that the water actually hit freezing point at .0

Question 2. The freezing point depression constant for water that was experimentally determined in this analysis was 0.0479 °C/m, which was derived from the slope of the trend line in Figure 4. This is significantly lower than the constant stated in the literature of 1.86 °C/m.1 The freezing point temperature determined via cryoscopy should have been much lower in the high sucrose concentration solutions.

The wet, crude product was placed into the 50 mL Erlenmeyer flask. Small amounts of CaCl2 were added to dry the solution. The flask was sealed and the mixture was swirled and left to settle. Once

2. (5 pts) List and explain the names and affiliations of the various characters/stakeholders in this story – I’m looking for us to use the story to map out the complexities that are generally associated with solving public health puzzles – the stakeholders you list and explain here should apply to many of the cases we consider going forward.

Introduction/Purpose: The purpose of this lab was to find out how gaviscon reacted with different salt solutions. Sodium Alginate is a compound that forms with the Gaviscon and forms a “raft” and blocks all the stomach acid from traveling up the esophagus.

Method As stated, our solvent in this lab will be tert-butanol. We start by recording the freezing point of this substance without anything added. Then, we add various

Experiment #1: Determination of the Solid-Liquid Phase Diagram for Napthalene-Biphenyl Using Thermal Analysis Objective To apply thermal analysis to the two-component system, naphthalene-biphenyl at atmospheric temperature. The analysis will be represented by a solid-liquid phase diagram (freezing point diagram). Theoretical Principles Phase Equilibria and the Gibbs Phase Rule This experiment is conducted in order to

This experiment has been split into several mini-experiments and procedures with the whole purpose serving to teach basic laboratory techniques. To begin, the first experiment requires the use of a meter stick or ruler which is then used to measure a lab notebook’s width and length in both inches and

The amount of NaOH used for each trial run was compared to one another. The three closest trials with the difference of ± 0.10 mL of each other were used to average the amount of NaOH dispensed for the HCl and Alkalak solution to turn slightly basic. The phenolphthalein (acid-base indicator)