Now add ~ 0.35 g of zinc powder to the solution and stir until the solution becomes clear. Dissolve the excess zinc with more sulfuric acid. Decant the liquid with a stirring rod, retaining only the copper. Rinse the copper with distilled water and steam dry. Weigh the mass.
In an acid base titration you may have an acid that you don't know the concentration of, and a base whose concentration you do know. The technique is to measure out accurately a volume of the alkali of unknown concentration into a flask, and fill up a burette with the acid. Add some indicator solution to the acid in the flask, so that when all the acid has reacted with the base, there will be a colour change. The burette is graduated. You then open the tap on the burette and let the acid run into the flask.
Controlled variables • Concentration of base • Temperature of chemicals • Same indicator used • Chemicals obtained from the same bottles • Same measuring apparatus used Apparatus • 2x burette • 2x retort stand • 2x clamp • 6x conical flask • 2x round bottom flask • 2x pipette • 1x measuring cylinder • 1x spatula • 1x electronic scale • 2x beaker • 1x Erlenmeyer flask • 4x 250ml volumetric flask • 10ml Bromothymol blue • 3x oxalic acid crystals • 3x Sodium hydroxide pellets • 1 Bottle Hydrochloric acid solution • 1x Thermometer • 1x video camera • 1x dropper Diagram Method Safety precautions 1. Plugging the beakers containing chemicals 2. Using tongs to pour chemicals 3. Keeping eyes and nose away from the opening of the beakers 4. Standing away from the work table when not working on the experiment 5.
Lab Report on Volumetric Determination of Iron with Potassium Permanganate Principle: This experiment consists of titrating the ferrous ion with permanganate ion to study the oxidation-reduction reaction. The ions react in acidic solution to give ferric ion and a reduced ionic form of manganese. All the reactants and products except permanganate ion are weakly colored, whereas permanganate is a very intensely colored ion. Then a solution of permanganate is removed as long as there is a ferrous ion present to react with it. But as soon as the entire ferrous ion has been oxidized, the next small portion of added permanganate colors the solution.
The objective for the second part is to compute for the percent composition of the potassium chlorate in a mixture correctly. Stoichiometry is the branch of chemistry and chemical engineering that deals with the quantities of substances that enter into, and are produced by, chemical reactions. It is the accounting, or math behind, behind chemistry. Given adequate information, Stoichiometry can be used to calculate masses, moles, and percents within a chemical equation. Methodology A test tube containing 0.2 gram of manganese dioxide was weighed.
Purpose The whole purpose of this experiment is to determine wether or not the amount of the zinc and or hydrochloric acid effects the out coming percent of the solution after under going chemical reaction. Procedure $ 1. Weigh the zinc metal pieces and place them in a test tube $ 2. Pour some hydrochloric acid over the zinc pieces. Observe $ 3.
As you can see from the diagram in one tube there was limewater that was to test for the carbon dioxide, and in the other was copper carbonate. If there were carbon dioxide present, the limewater would turn cloudy (white in colour). When I was observing what happened I could see that there was carbon dioxide present because the limewater turned cloudy. Secondary Experiment This experiment was to compare the rates of decomposition of several metal carbonates. Several metal carbonates were placed in a test tube and linked to a syringe that measured the amount of carbon dioxide gas when the metal carbonates were heated.
4. Put approximately 2 mL of 1.0 M copper (II) nitrate in an adjacent well. Polish small strips of zinc and copper metal, and place the metal in the appropriate well containing the solution of the ions of that metal. 5. Take a small strip of filter paper that has been soaked in potassium nitration solution, and drape it across the wells so that one end dips in the solution in each well.
Giving us a slightly inaccurate measurements. This can be avoided by getting used to the burettes release mechanism and knowing how to control the flow of the Sodium Hydroxide to the Acid. Conclusion: To conclude this lab, we learned how to calculate the mass volume percent of acetic acid in a vinegar solution using stoichiometry learned in unit 2 and how to conduct a proper titration lab.
The Concentration of Odium Hydroxide Solution by Titration Against the Primary Standard Ethanedioic Acid-2-Water Introduction Titration is a method of analysis that to determine the precise endpoint of a reaction. In a titration, solution was run from a burette into a definite volume of another solution in a conical flask. 1 or 2 drops od suitable indicator (phenolphthalein) is added to indicate the end point. The end point is the stage at which two solutions have just reacted completely. The accuracy of titration results depends very much on the correct detection of the end point.