ADI Molarity Lab Report

My results yielded a high Average Molarity .270M . The ideal would be around 1.000M . Deviation was ± 1.20

Stoichiometry is a very important part of chemistry. Stoichiometry refers to calculating the masses of molecules and their products . The reactants are usually given and stoichiometry is used to find the products of the equations as well balancing the equation. An example of this would be sodium chloride (NaCl). Stoichiometry will say that if there are ten thousand atoms of sodium and one atom of chlorine, only one molecule of sodium chloride can be made and that fact can never be changed.

From the excel chart of Molarity vs. Density, what was the relationship between the molarity of the sugar solution and the

In the experiment I performed it was proven that, the moles of a solute, the volume of the solvent, and the molarity of an aqueous solution share a mathematical relationship. Solutions, solutes and molarity are all terms that are crucial to chemistry. A solution is defined as a liquid mixture in which the solute is distributed into the major component, and a solute is defined as the minor component within a solution. The molarity of a solution is the number of moles of solute per liter of solution and it is used to express the concentration of a solution. Both the solute amount and the solution volume can be determined in experiments to aid finding the solution concentration or molarity of a substance that they are included in. I state confidently

The results showed the molarity of the NaOH solution. This experiment was completed twice and a new average molarity

One of the most important skills to have in the chemistry lab is the understanding of how chemicals will react. Knowing for example, how a chemical will react with a metal, is an excellent way of determining the amount of a particular metal in a deposit. This knowledge was used in this lab to determine the amount of copper in an unknown sample mixture. It is also known that the determination of the percent concentration of a certain solution, will directly effect the percent transmission and absorption of a solution, dependent upon its dilution. By first testing known concentrations of a solution, and plotting this information graphically, a line is formed

Our purpose in this lab was to create four solutions of the same components and different concentration. I found the concentration in Molarity (mol/liter). I would dilute a solution to create new solutions, using the formula M1xV1=M2xV2 where M=molarity and V=volume. In this lab, there were four solutions, Solution A, Solution B, Solution C, and Solution D. The solute or substance that dissolves was sugar and the solvent or substance that the solute dissolves in was water. For Solution A, I weighed 3.42 g sugar and diluted to 100 mL to get a concentration of 0.10 M and the color of bright red. For Solution B, I weighed 0.342 g sugar and diluted to 100 mL to get a concentration of 0.010 M and the color of pink. For Solution C, I measured 10

Molarity – the concentration of a solution expressed in moles of solute per liter of solution

In the third stage of this experiment, the density of a liquid was determined and compared to known standards. A 100ml beaker was filled to about half-full with room-temperature distilled water. The temperature of the water in ◦C was recorded in order to compare to known standards later. A 50ml beaker was then weighed on a scale in order to determine mass and recorded. A sample of the distilled water with an exact volume of 10ml was then placed in the 50ml beaker using a volumetric pipette. The 50ml beaker with the 10ml of water was then weighed again and the initial mass of the beaker was subtracted from this mass to obtain the mass of the 10ml of water. With the volume and the mass of the water now known, density was calculated using d = m/V and recorded in g/ml. This process was then repeated to check for precision and compared to standard values to check for accuracy. Standard values were obtained from CRC Handbook, 88th Ed.

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.

Lab 1 also teaches us the importance of molecular weight of a substance and how to use that to find the amount of moles of that substance in a solution. For example; in exercise 3 we were asked to weigh 8 grams of sugar and then calculate how many moles of sugar it really was. Using the molecular weight of sugar (C = 12.01 grams/mol, H = 1.008 grams/mole, O = 15.00 grams/mole). We were then able to use this molecular mass of the sugar that we then had to use to calculate and determine the molarity of the sugar

For lab eight, the molarity of the NaOH solution is 0.07823 M. For lab nine, the molarity of the NaOH solution is 0.4224 M. The molarity of the NaOH solution for both lab eight and nine was not accurate because the solution did not turn the color to pink. Some source of error in this lab is oxalic acid is not completely moved from the plastic lab tray to the beaker. There is a small amount of substance left in the plastic lab tray that cause the mass of the beaker with NaOH solution to have less mass than I measured previously. Another source of error is not all the base was delivered from the burette to the beaker with oxalic acid. Some base remained on the side of burette instead of fully going into the beaker. This leftover base would change

In conclusion when the molarity level was at 0 and at .2 the potatoes had gained mass so therefore they were placed in a hypotonic environments. When the molarity level was .4 and above the potatoes loss mass so therefore they were placed in hypertonic environments. So the different in concentrations does change the mass of the potatoes because they determine the osmosis environments.

Molar Consentration or Molarity: Concentration of a solution measured as the number of moles of solute per liter of solution. For example, a 6 M HCl solution contains 6 moles of HCl per liter of solution.

The purpose of this lab was to find and compare the saturating concentration of Sodium Chloride (NaCl) and Sucrose. By making solutions of NaCl in water at different concentration, we found that the saturating concentration NaCl is between 0.375g/ml and 0.500g/ml. Using the same method, we found that the saturating concentration of sucrose is 0.750g/ml. Moreover, to further our understanding of density, we created a discontinuous density gradient using different concentration of sucrose solutions. When we placed the solutions in the test tube according to their relative density, we found that the solution with highest concentration sinks at bottom and the solution with lowest concentration stays on top. Therefore, we concluded that the higher the density of a solution is, the lower it will sink in a mixture.