First, put on safety goggles to protect the eyes from the chemicals used in this experiment. To begin the lab, label one 100-mL beaker “HCl” using a beaker marker and add 30 mL of 1.0 M Hydrochloric acid solution to this beaker. Next, label the other 100-mL beaker “Na2S2O3” and pour 30 mL of 0.30 M Sodium thiosulfate solution. Finally, label the 250-mL beaker “H2O” and add 25 mL of Distilled or deionized water into this beaker. After all the beakers have been labeled and filled with their set solutions, place a sheet of white paper underneath the six-well reaction plate and using the black sharpie, draw a “X” under each of the wells. Before beginning the lab, place the six-well reaction plate over the sheet and verify that the six “X’s” can be seen through the plate. …show more content…
Make sure that there are no air bubbles in the syringe as that will affect the results of the experiment. After it is checked to make sure there are no air bubbles empty the syringe into Well #1 of the six-well reaction plate. For Well #2, submerge the 5-mL syringe in the 100-mL beaker labeled “Na2S2O3” (be sure that the syringes are not being mixed in different syringes) and draw 1.5 mL of the Na2S2O3 solution into the syringe. Then, fill the 5-mL syringe up to the 1.5-mL mark with distilled or deionized water by submerging the syringe in the 250-mL labeled “water” beaker by drawing water into the syringe. For Well #3, fill the 5-mL syringe up to the 2-mL mark with distilled or deionized water by submerging the syringe in the 250-mL labeled “water” beaker by drawing water into the syringe. Next, submerge the next 5-mL syringe in the 100-mL beaker labeled “Na2S2O3” and draw 1 mL of the Na2S2O3 solution into the syringe. Empty both solutions into Well #3 of the six-well reaction
For this experiment, you will add the measured amount of the first sample to the measured amount of the second sample into its respectively labeled test tube then observe if a reaction occurs. In your Data Table, record the samples added to each test tube, describe the reaction observed, if any, and whether or not a chemical reaction took place.
Repeat for each trial. Rinse volumetric pipette with vinegar and drain into the waste beaker. Weigh and record the mass of each 200mL beaker. Add 10.00mL of vinegar into each beaker and weigh them and record their again. Add 50mL of de-ionized water to the beakers and place them under the drop counter on top of a stir plate, submerging the pH meter into the solution. Place the stir bar into the beaker and carefully turn on the stir plate so that the stir bar spins without splashing or hitting the sides of the beaker or the pH
the chances of collisions increase thus giving a faster rate of reaction. Then the s Apparatus:. Beaker Hydrochloric acid Distilled water Measuring cylinder Pipette Test tubes Test tube rack Diagram:.. [ IMAGE] Method: The.. Measure out 10cm3 of hydrochloric acid, as the concentration requires. for each concentration its composition is.
reaction is the rate of loss of a reactant or the rate of formation of
Rates of Reaction - The concentration of hydrochloric acid and the rate of reaction with sodium theosulphate
Experiment is to investigate the rate of reaction between hydrochloric acid and calcium carbonate Hydrochloric acid + Calcium Carbonate Þ Calcium Chloride + Water + Carbon Dioxide 2HCl (aq) CaCo3 (s) CaCl2(s) H2O (aq) CO2 (g) There are a number of variables in this experiment and these are listed below as input variables and outcome variables.
from 10cm to 50cm to make it easier to see the difference in a graph.
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
To make sure it was a fair test. i had to constantly keep cleaning and
In this the experiment the amount of Sodium Thiosulphate is varied each time in comparison to the amount of water used, the solution will always add up to 45cm3. There will always be 5cm3 of hydrochloric acid used. The experiment was performed at room temperature as this made the experiment easy to perform, as no heating or cooling devises were necessary.
My aim in this piece of work is to see the effect of temperature on the rate of a reaction in a solution of hydrochloric acid containing sodium thiosulphate.
The temperature at which the reaction is carried out Use of a catalyst Reaction equation is mentioned above but rate equation can only be decided by doing experiments. So, the following procedure can be used to carry out the experiment. Plan Equipment 2 Measuring cylinders Beaker Stopwatch Paper with black cross on it Sodium Thiosulphate (different concentrations) Hydrochloric acid (same concentration each time) Water (different concentrations) Pipette. Prediction I predict that the greater the concentration of sodium thiosulphate solution, the faster the chemical reaction will take place.
Effect of Temperature on the Rate of Reaction between Sodium Thiosulphate and Hydrochloric Acid Investigation Chemical reactions are used in our everyday life, they literally keep us alive. They are used in food, respiration and everywhere else in the environment. A chemical reaction mainly occurs when reactants react together to produce a new product. The speed at which this reaction takes place is called the rate of reaction. The product produced has a number of particles in the solution that has formed from the reactants.
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).
The Effect of Acid Concentration on the Rate of Reaction Introduction: We are going to investigate the effect of Acid Concentration on the Rate of Chemical Reaction. We are going to use the combination of Hydrochloric Acid and Calcium Carbonate as the reactants: [IMAGE][IMAGE] [IMAGE]Calcium Carbonate + Hydrochloric Acid Calcium Chloride + Water + Carbon Dioxide Prediction I predict that the greater the concentration of acid the greater the rate of chemical reaction i.e. the rate of reaction will be directly proportional to the concentration of acid. This means that if I were to double the concentration of acid the rate of reaction would also double, halving the time taken. In order to generate a more accurate picture I have constructed a series of graphs highlighting my above statements. I have used a relative scale, following my prediction, in order to calculate the rate and therefore time taken.