Molar Volume Lab Report

In the ADI Molarity Lab, the primary tasks was to use different values of moles of solute, volume of solvent, and molarity to find the mathematical relationships between them. To find these relationships, our group had to change the quantities of each of the variables and visually observe the molarity within the solution. For instance when using Cobalt (II) Nitrate to find the relationship between volume of the solution and the molarity of the solution; the group kept the amount of moles of the solute at a constant of 1.00 moles because if it would have changed it would have caused inaccurate data. We first set the volume of the solution to 0.2 liters. The molarity of the solution was 5.00 mol/L. Then we changed the volume of the solution

In this lab experiment our main focus was to get skillful in using tools such as the metric ruler, balances, thermometer, and graduated cylinder to capture measurements of length, mass, temperature and volume. Additionally, this lab helped us to become more familiar with the uncertainty of measurements, as well as becoming efficient with rounding our measurements to the correct numbers of significant figures. Our results are measured consistently with rounding to the closest answer we could possibly acquire as the data can tell you.

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

This experiment was done in order to understand both fractional distillations and gas chromatography. In addition, this experiment was done to separate and identify two liquids that made up an unknown mixture. Gas chromatography was used to figure out the ratio of these two liquids.

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.

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

Corresponding to the previous experiment, this week’s experiment measures the participants’ ability to conduct basic, fundamental laboratory procedures. These procedures revolve around scientific measurements of volume, mass, and density. Unlike last week’s activity, this week’s experiment had a few modifications. In addition to distilled water, saltwater and an unknown substance were added. There was a total of five substances to choose from; Hexane, Methanol, Ethyl acetate, Ethylene glycol, and Dichloromethane. Part C, the unknown liquid number was four, which the average density was 0.789 gmL-1, and from looking at the chart the unknown identity was methanol. Part A, the temperature of the water was 20 oC, which was in front of the class,

The mean voltage of the battery terminals while connected to the identification resistors is presented in Figure ‎4 12. These samples have been pulled out from the voltage sensor of the PEB panel. The voltage decreased as expected from 12.53 to 12.5 during first 20 seconds of connection to the

The purpose of this experiment is to determine the molar mass of an unknown volatile organic liquid, using methods such as, the Dumas method, and then state its identity.

The purpose of this lab was for my group, which was just Wendy Say and I, to use a graph to help measure density. We had to measure the mass and volume of several samples of pennies, and then create a graph to determine the pennies’ average density. We used seven materials, which were used in two different parts. In the first part we used a graduated cylinder, a scale, paper towels, a pencil and twenty-four pennies. The graduated cylinder was used to measure the volume of the pennies by water displacement, the scale was used to measure the mass of the pennies, the paper towel was used to dry pennies because we couldn’t reuse them, and the pennies were needed because we were getting their average density.

The purpose of this experiment is to identify an unknown substance by measuring the density and boiling point. I will be able to conclude which substance is my own from a list of known options stating what its real boiling point and density is.

To osmo- regulate properly in a marine habitat, physiological mechanisms intended to conserve fresh water and thus avoid dehydration are required. Marine mammals are well adapted to their hyper-osmotic environment. Their cells need to maintain both a water balance and an ion balance and life depends on the maintenance of the transmembrane potential. The concentration of potassium ions is higher in cells than on the extracellular fluid (ECF) and the concentration of sodium ions is higher in the extracellular fluid. Osmolarity is describes the total solute concentration.

In 1909 S.P.L. Sorensen published a paper in Biochem Z in which he discussed the effect of H1+ ions on the activity of enzymes. In the paper he invented the term pH to describe this effect and defined it as the -log[H1+ ]. In 1924 Sorensen realized that the pH of a solution is a function of the "activity" of the H1+ ion not the concentration and published a second paper on the subject. A better definition would be pH=-log[aH1+ ], where aH1+ denotes the activity of the H1+ ion. The activity of an ion is a function of many variables of which concentration is one. It is unfortunate that chemistry texts use a definition for pH that has been obsolete for over 50 years.

In this experiment, we experimented finding the fundamental quantities of length, mass, and time using many laboratory tools. We used a Vernier caliper, stopwatch, rulerm meter stick, wooden block, metal block, Dial-o-gram, different masses, and circular objects. We took into consideration the uncertainties of many different tools and objects into our experiment. The inherent uncertainties of different measurements and ways to propagate those uncertainties were learned during this experiment.