4. Transfer about 20 mL (+0.02 mL) of the HCl to the flask from the acid buret located on the reagent bench. Record the molarity of the HCl and the initial and final volume readings from the buret (+0.02 mL).…
Titrate the contents of the conical flask by adding to it 0.100 mole dm3 hydrochloric acid from the burette. Add the solution slowly. Swire the flask gently to mix the contents at the end indicator turns as define red colour. This is the end point of the titration. Record the final burette reading in your table of result. Repeat the titration to obtain several sets of results or until you obtain two results which are concordant. You should always carry out at least three titrations. Record all of the results that you obtain. Calculate and record the average (mean) titre volume of hydrochloric acid solution. Remember…
get the mass of a evaporating dish, put a sample of the hydrate onto the evaporating dish and mass the dish with hydrate.…
Find the mass of a clean crucible and lid. USE THE SAME BALANCE DURING THE ENTIRE EXPERIMENT.…
During my observation I noticed that when 10mg of magnesium metal was added to the beaker a shaded area appeared on the bottom of the beaker. When the bubbles stopped and the shaded area in the beaker disappeared it showed that the magnesium has been consumed.…
When holding test tube inverted over heptane flame, condensation formed against top walls of the test tube. When the burning splint was added the walls of the test tube became less foggy from the condensation formed from the heptane flame.…
Purpose: The purpose of this lab is to find the limiting reactant, also to find the percentage yield and percentage purity of the reaction that happens between Calcium Chloride and Sodium Carbonate. The other purpose was to know how the reaction can be balanced and created.…
A hydrated ionic compound is an ionic compound that has a well-defined amount of water trapped within the crystalline solid. The water associated with the compound is called the water of…
5. Select the distilled water in the beaker and add 25mL to the graduated cylinder.…
The Law of Definite Proportions states that a chemical compound contains the same element in exactly the same proportions by mass regardless of the size of the sample or source of the compound. This relates to the magnesium oxide lab because we tested out this theory to see if it is true that the law of definite proportions says that a chemical compound contains the same element in exactly the same proportions by mass regardless of the size of the sample or source of the compound.…
In this lab, we used Bunsen burners to heat up a hydrated salt in order to determine the percentage of water inside of this hydrated salt. We heated up the salt in order to boil off the water, which allowed us to find the weight of the CuSO4 by itself. By comparing this final weight with the original weight and subtracting the difference, we were able to compile data about how much the weight of the hydrated salt decreased as the water gradually boiled away. In doing so, we were able to find the total weight of the water in the hydrated salt by subtracting the final weight weight from the original weight of the hydrated salt, allowing us to calculate the percentage of water in the hydrated salt by dividing the weight of the water by the original…
Procedure: 1. Cut the strip of magnesium into 10 mm pieces with the scissors/knife and then hold them in the beaker. 2. Measure out 5 mL of HCl (.5 molarity) with the dropper into the graduated cylinder. 3. Pour HCl (.5) from the graduated cylinder into the test tube. 4. Put a piece of magnesium into the test tube filled with HCl. 5. Start stopwatch when the magnesium is placed into the test tube filled with HCl (.5) and stop it when the magnesium has dissolved (flick the bottom of the test tube periodically to make sure that the magnesium mixes properly with the HCl). 6. Record your data and then dump out the HCl and wash your materials. 7. Repeat steps 2-6 with .5 molarity until you have completed 5 trials with it. 8. Get a new test tube. 9. Repeat steps 2-6 with 1 molarity. 10. Repeat steps 2-6 with 1 molarity until you completed 5 trials with it. 11. Get a new test tube. 12.…
Measure out approximately 100 mL of 0.50 M hydrochloric acid solution and 100 mL of 0.50 M sodium hydroxide solution. Record both volumes on your data table.…
5. Using the graduated cylinder label base, add 5ml of sodium hydroxide (NaOH) to tube 3.…
The decomposition of sodium carbonate is definitely, Na2CO3(s)+CO2(g)+H2O(g). The was the only equation that matched up exactly with my data in terms of percentage. To start off with, when I balanced out the equation, I got 2 NaHCO3→ 1 Na2CO3(s)+ 1 CO2(g)+ 1 H2O(g). Therefore when I set up my stoichiometry problem I got 3.2 grams NaHCO3 over 1 x 1 mol NaHCO3 over 84.007g NaHCO3 x 1mol Na2CO3 over 2 mol NaHCO3 x 105.987g Na2CO3 x 1 mol Na2CO3. Hence, I multiplied 3.2 x 1 x 1 x 105.987 and got 339.1584.…