What Is The Use Of Measure In Relation To Acid-Base Balances Lab Report

Purpose: To learn about the international system of units (SI), to become familiar with common lab equipment and techniques, to gain proficiency in determining volume, mass, length, and temperature of a variety of items using common laboratory measurement devices, to learn to combine units to determine density and concentration, and to use laboratory equipment to create serial dilutions and determine the density and concentration of each dilution.

We calibrate a volumetric pipet and flask. We also calibrated a beaker and 50 mL buret. We also calculate the difference between the expected density and density obtained by our team.

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.

9. The accepted value for the density of water is 1 g/mL and the accepted density for isopropyl alcohol is 0.786 g/mL. Determine the percent error between your calculated densities and the accepted values for both water and isopropyl alcohol. Record the percent error in Data Table 4.

For each of 3 acceptable trials, enter the mass of your bleach sample in GRAMS. Your mass precision should

Weight 10 dry post-82 pennies which get 77.12g, using 30ml initial volume measuring the volume of 10 pennies, record the data 9.1ml. Using equation Density= Mass/Volume, get the density of the pre-82 pennies is 8.47g/ml. Then calculate the error%=0.04%, and the deviation%=7.13%.

There were three different runs in order to have comparable data and to increase the validity of the experiment. The first run gave 39% of Sodium Bicarbonate. The second run gave 34% of Sodium Bicarbonate while the third one gave 39%, which is the same as the first run. The average percentage was 37% which is much lower than the manufacturer's percentage of 59%. The percent error came out to be -37%.

Abstract: The objective of the lab is to determine the volumes of the polystyrene spheres with three different measuring tools: Water Displacement, Analytical Scale, and Triple Beam Balance Scale. The experiment is meant to help understand the concept and application of precision and accuracy in experimental measurements. Accuracy is a measure of how closely the results of repeated measurements are to the true value of what is being measured. Precision is the variability in the results from the repeated measurements, and how close the repeated measurements were to one another. In this lab, the method for measuring the volume of the polystyrene spheres is done with the previously stated tools: Water Displacement, Analytical Scale, and Triple Beam Balance Scale. The standard deviation for the entire classes volumes and masses are recorded to determine the densities.

Spectrophotometers are quite precise instruments allowing for five significant figures to be obtained. The major source of error in this lab is how small the concentration of the reagents are.

This lab was not repeated to examine for consistent results, which may result in data where precision and accuracy are compromised. In this investigation,

Calculate the percent error for your result. Show all work. State and explain at least two sources of error for this experiment. How might you change the experiment to reduce the error from one of those sources?

Through this experiment, we were look for a relationship between a gas’ atomic mass and its mass. In doing so, we were paying very close attention to two other central ideas of chemistry: accuracy and precision. Accuracy is how close a measured value is to the actual true value, while precision is how close the measured values are to each other. The most appropriate calculation for testing accuracy is % Error. Through this calculation, you are actually comparing your value to the literature value, or those values found in the

This experiment shall be repeated twice or more to enhance accuracy of the results obtained. Besides detecting systematic errors, this experiment would aid on the technique and understandings to the correct use of these equipments.

The density of water is its mass divided by its volume. In this case, the mass of water was determined by subtracting the final mass of the glassware with water by the initial mass of the glassware without water. The volume was determined by observing closely which line (marked on the sides of each glassware) the water reached and reporting the most precise measurement. Based on the class data, the average densities of water and its standard deviations were: 50-mL beaker – avg: 0.90 g/mL, stand dev: 0.12, 10-mL graduated cylinder – avg: 0.980 g/mL, stand dev: 0.0600, 10-mL volumetric pipette– avg: 0.9800 g/mL, stand. dev: 0.06499, 50-mL burette– avg: 0.969 g/mL, stand. dev: 0.140. The average density of water compares our experimental value to the true value. This means that the closer our values are to the true density of water, which is approximately 0.998 g/mL at 18.89°C, the more accurate our data is. Furthermore, the standard deviation measures how precise our results are with one another.

Furthermore, the measurements from a wooden block and a metal object were taken to calculate their volume and density. In this case, the calculations were more precise but due to other sources of errors, which may be systematic, random or personal, the data was not 100% accurate. There are always certain uncertainties associated with any type of measurement and it is important to know that no measurement will be one hundred percent correct.