Investigating The Mass Rate Of Sodium Hypochlorite

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

thiosulfate anion needed to react with each mole of hypochlorite anion in the bleach sample.

The topic is: The cleanest cleaner. In this experiment, the scientists will be testing which brand of detergents cause a better cleaning effect on one stain on multiple white shirts. The independent variable in this experiment consists of the different detergents, while the dependent variable consists of the amount by which the stain faded (using the purple light scale), and or removed, others include the white t shirts, washing cycle, and drying cycle, staining agent, and cycle of drying and washing. The control variable in this experiment will be the 1 trial run with water only per experiment. The unit while measuring the amount of detergent is mL, and a scale which the is going to use to measure the amount of stain faded.

The errors in the lab which could best explain the slight disparity between the measure of the experimental and theoretical masses would be pouring the limiting reagent into the excess reagent, and the inability to completely gather the precipitate into the filter paper. However, since copper(II) sulfate was present on our the filter paper, it would add to the mass, therefore, the mass lost would have to be slightly greater than that gained as to create the slight disparity between the experimental and theoretical masses. Stoichiometric predictions are valid as long as errors in the experimental trial are taken into consideration. Furthermore, the experimental mass could be more similar to stoichiometric predictions if the excess reagent was poured into the limiting reagent, and if more than one trial were conducted. Additionally, the results of this lab, as well as any other lab, would be more thorough and conclusive if it was conducted more

The problem that was trying to be solved in this study deals with analyzing unknown solutions. In this particular case, a chemical company has several unknown solutions and to correctly dispose of them they need to know their properties. To figure out the properties several qualitative tests were performed throughout the study (Cooper 2012).

was to determine the percentage by mass of acetic acid in vinegar using acid/base titration. The

When the concentrations were changed so did the rate of reaction. When the concentration was changed to 0.265M the rate of reaction dropped by a factor of 0.5 (50%) below the control value. Furthermore when 60mL of water was added to the bleach dropping the concentration too 0.132M the rate dropped by a factor of 0.7 (70%).

For the concentration experiment three different concentrations were made of the KMnO4. Three test tubes were filled with 4 ml of water. The first test tube had 1 ml of the 500 KmnO4 added to it. Then the second test tube had 1 ml from test tube one and 4 mL of water. For test tube 3, 1ml was taken from test tube two. Each concentration was placed into a dialysis tubing using the strings to tie off one end and the clamp to close off the other end. Before the dialysis tubing was placed in the beaker, 1ml of a sample was placed in a cuvette to blank the spectrophometer. Each stir plate was set on a low speed and the dialysis was hung in the water by a string. Every 5 minutes that passed a sample of 1 ml was taken and put into a cuvette. The cuvettes were placed in the spectrophometer to measure the absorbance of each solution. The measuremnts were then recorded in lab notebook. Once the measurements were documented, the average of absorbance and concentration was recorded.

The purpose of this lab was to determine the limiting reactant in a mixture of to soluble salts and the percent composition of each substance in a salt mixture.

The purpose of this lab is to determine the percent of water in a hydrate. I learned that copper sulfate hydrate is blue on its own but, when heat is added it will change color to a dim gray. One error that may have occurred is the failure to zero the scale which would ultimately change the math in the equation. Another error that may occur in this lab is forgetting to wait the recommended amount of cooling time, which would change the mass of the elements. At the end if the lab when we look to the questions, it is also beneficial to look at the notes for the lab because it helps with the setup of equations that may come with the questions, also it is very helpful

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

The purpose of this experiment is to determine an unknown concentration of acid (hydrochloric acid) with a standard solution of a base (sodium carbonate) using titration method.

2. To titrate a hydrochloric acid solution of “known” concentration with standardized 0.5M sodium hydroxide.

The purpose of this lab was to use process titration to find concentration of an aqueous solution of Hcl(aq) , using KOH(aq) as the titrant.

In this experiment, a redox reaction occurred. An oxidation-reduction reaction (redox) is a type of chemical reaction that involves a transfer of electrons between two solutions. The chemical being oxidized is losing electrons and the chemical being reduced is gaining electrons. In this case KMnO4 is losing electrons and Oxalic Acid is gaining electrons. KMnO4 can titrate a or reduce Oxalic acid. Titration is the technique used to find the unknown concentration of one solution based on the concentration of a known solution. In equation 2, the molar relationship between the 2 is shown, it is 2 KMnO4 to 5 Oxalic Acid. The molar ratio relationship is useful because it shows how much of a certain product is needed to help a reaction occur and which chemical is limiting reagent. The experiment was started by preparing a titrating strength KMnO4 solution from stock to a less concentrated KMnO4. Equation one shows how this was done. The KMnO4 needed to be diluted, if it had not been diluted, then it would be way too hard to get an accurate reading of the Oxalic Acid used. Without being diluted the Oxalic Acid would be strong. The next step was to standardize the KMnO4 solution. It was calculated that 37.5 mL of Oxalic Acid could titrate 15 mL of KMnO4. To determine the exact molarity of a solution a standardization needs to happen. In this experiment the standardization found how much Oxalic acid was needed. Through the controlled variable, the fact that 37.5 Oxalic acid could be titrated by 15 mL of KMnO4, the percent of the