-Use the titrations of the following chemical reactions: NaHCO3 + HCl (aq) NaCl (aq) + H2O (l) + CO2 (g) 2HCl (aq) + Na2CO3 (s) 2NaCl (aq) + H2O (l) + CO2 (g) Experimental procedure- Two Erlenmeyer flask must be labeled “unknown 1 and unknown 2”. Assure that all containers used are dried and cleaned properly. Two bigger flask are labeled “waste” according to each unknown. A pipette is set up and primed with HCl. The two unknown solids are weighed to a mass of 0.15g each.
Resolution of Matter into Pure Substances – Paper Chromatography Abstract The purpose of this laboratory was to determine how different substances have different solubilities in a given solvent. This was accomplished using the method of chromatography. The solubility of each substance was first determined by dropping a drop or two of each on a line drawn 2 inches above the bottom of a piece of paper. Then the paper was lightly bent in order to tape both sides of the paper leaving about a 4 centimeter gap so that the sides of the paper are not touching. The paper was then put into a beaker of a hydrochloric acid, ethanol, and butanol mixture, being sure that the paper does not touch the sides of the beaker, and then topped.
Using a Buchner funnel, a hose, and a suction flask we created a vacuum filtrator which we used to help remove the remaining liquid on the copper so that we may make a more precise measurement of the mass of the remaining copper. Our final mass of copper was .7951 grams. Results and Discussion: Initial Mass of Cu: .25 grams When we mixed the 5 ml of 6 molar HNO3 the copper had disappeared, indicating it had been used in the reaction. The copper had undergone a single replacement reaction and a decomposition reaction. Initial equation: Cu(s) + HNO3(aq) -> Cu(NO3)2(aq) + NO2(g) +H2O(l) Balanced: Cu(s) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) The copper had replaced the Hydrogen in the HNO3 and the NO3 had also broken down into NO2 and O2- allowing the H+ to bond with it and create
While the soil is soaking, add dispersing agent into the control cylinder (Sodium Hexametaphosphate 125ml) and fill it with water to the mark. 3. Shake the cylinder in such a way that the contents are mixed thoroughly. Insert the hydrometer and thermometer into the control cylinder and record temperature. 4.
Allow the mixture to cool for a few minutes then filter it, using either gravity or vacuum filtration. (We shall be using vacuum filtration.) Wash the residue in the funnel once with a little water and collect all the filtrate. 4. Pour all the filtrate and washings into a 250cm3 volumetric flask.
Let’s experiment and observe Whether these ions will have a reaction or indeed soluble in water. Experimental Procedure Let’s begin this experiment by obtaining a 100ml beaker from our equipment tool bar list, then we are going to add 50ml(s) of Potassium Chromate 1M solution to that beaker, The next step we are going to add another ionic compound of 50ml of Lead (11) nitrate 1M into the same beaker as the Potassium Chromate. As we observe the beaker, we notice a reaction has occurred and a precipitate has formed and settled on the bottom of the beaker. The next step is we are going to filter the resulting precipitate into a 250 ml Erlenmeyer Flask with a Buchner funnel. Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight.
Stoichiometry of Reactions in Solution I. Introduction: Stoichiometry of reactions in solution applied stoichiometry and the idea of a limiting reactant to a reaction in solution. This experiment involved performing aqueous acid and base titrations to determine the mole ratios of four different acid base reactions. Titration is one compound added to a known amount of another compound quantitatively and reacted together to completion (the solution turn pink at the end point). The end point is also called the neutralization point, which means that all the acid has reacted completely with the base and the solution has been neutralized.
Enzymes Amylase: | Tracing the Breakdown of Starch | Rashaud Pickering, Ashley Bagnis, Stephanie Alvarado, Elbany Angulo 3614098 Section U-14 | Signature___________________ Abstract An experiment was conducted to find out what the optimal temperature for amylase to break down starch was. An Iodine test was used to find evidence of starch formation. Three drops of iodine were dropped into two sets of spot plates. There were four test tubes that contained human amylase and four test tubes that contained fungal amylase. These specimens were all tested before being placed into their respective ice or water baths.
Determine what your group’s hypothesis will be and write it as an “if, then” statement on your lab report. 2. Label each petri dish with the 4 different amounts of salt using the grease pencil: (control (0%), 1%, 2% and 3%) 3. To make salt concentrations of 1%, 2% and 3%: -Place 100 mL of water in beaker -To make a concentration of 1%, add 1 gram of salt (for
Title Page Experiment Title: Experiment 4: Qualitative Analysis of Cations III – Mg2+, Ca2+, Fe3+, Ba2+. Aim To determine the presence of the cation II , Mn2+, Ni2+, Fe3+, (Fe2+), Al3+, Zn2+ by using separation method to confirm the presence of cation II in the test solution. Procedure Please refer to the laboratory manual page 30-31. Results Procedure Number and Ion | Test Reagent or Technique | Evidence of Chemical Change | Chemical(s) Responsible for Observation | Equation(s) for Observed Reaction | 1 | Centrifuge the solution. | A brown precipitate was formed.