Nacl2 Lab Report

In order to fulfil the labs purpose, the lab was split into two parts. The first part consisted of measuring and determining the freezing point depression of the solution water. The second part consisted of measuring and determining the freezing point depression of a solution that consisted of water and an unknown solute.

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.

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.

The freezing point constant (Kf) of water is 1.86 °C m-1. Each mass amount and Van’t Hoff factor was calculated then analyzed in a table.

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

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.

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

Results were recorded after every five minute interval up to twenty minutes. For 0g and 2g of sodium bicarbonate dissolved in water, there were zero leaf chads floating. However, in the solution containing 1g of sodium bicarbonate, there were 2 leaves floating after 5 minutes, 4 leaves floating after 10 and 15 minutes, and the remaining leaf adding up to a total of five leaves floated after 20 minutes. There is a trend in the table for 1g of sodium bicarbonate due to the increase in leaves floating. The results from the lab was plotted on a scatterplot, which contains a trend line.

Many solutions can be used to lower the freezing point of water. They use salt to decrease the freezing point of water to keep roads clear of ice or other things that require decrease in waters freezing point. The colligative properties can be helpful in finding the molar masses of anonymous compounds. For low concentrations of substances that cannot be turned to gas readily, the freezing point depression of the solvent can be given in the

Student added solutions of 0.9% of sodium chlorine, 10% of sodium chlorine and distilled water to individual slides containing a drop of blood, then placed under the microscope, the following observation listed below took place, and were compared to the original slide number one. Slide#1 with one drop of sheep’s blood. The first slide was placed under the microscope under the magnification of 40x, and a thick red layer appeared with a white streak on the side. There was little air bubble spread on the layer, which looked like a piece of meat with lean on it.

Next is to calibrate a thermometer through various reading and the discovery of the true temperature of the boiling point. First, fill a beaker with approximately 50 mL of ice, then cover the ice with water. Attack it to a ring hold with a

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.

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.

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

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.