Chromite is iron magnesium chromium oxide. In some rare cases, magnesium is substituted for iron. Also aluminum and ferric ions can substitute chromium in a reaction. Hydrometallurgy is a form of extractive metallurgy that utilizes aqueous solution chemistry for the recovery of metals from salts, minerals, or ores. Extraction is a process in which metal is removed from an ore by dissolving the metal in a solvent, then recovering the metal from the solution (This is done by dissolving the metal into an acid or water).
Determining the Concentration of a Solution: Beer’s Law Purpose: The purpose of this lab was to measure absorbance value of standard solutions. And to find the relationship between absorbance and concentration. Then determine the concentration and the formula of the unknown CO(NO3)2*nH2O solution. Introduction: The reason we conducted this experiment was to determine the concentration and formula of an unknown solution. We used a calorimeter to monitor the light received by the photocell to determine the absorbance of different concentrations of cobalt chloride hexahydrate.
Introduction: Stoichiometry is the branch of chemistry concerned with measuring the proportions of elements that combine during chemical reactions (Bing). The mole ratio, which is the comparison of moles of a given reactant or product in an equation, is essential to the proper usage of stoichiometry. In the following experiments, stoichiometry and mole ratios were used to accurately predict and obtain missing proportions from the given equations. In the stoichiometry of a neutralization reaction experiment, the molarity and type of acid were predicted by the titration of an unknown acid using .1 molar (M) Sodium Hydroxide (NaOH). In the other, aluminum leftovers, the activity series was used to understand how and why the reaction took place and stoichiometry was used to predict the amount of aluminum that should have reacted in the following equation: 3CuCl2 * 2H2O (aq) + 2Al (s) 2AlCl3 (aq) + 3Cu (s) + 6H2O Stoichiometry’s importance in the laboratory is well defined in the results of the previously mentioned experiments.
Chose and Obtain Sulfate Solution will form aqueous compound as sulfate when combined with anything is aqueous · Is an anion 3. Chose and Obtain Nitrate Is an anion · Need another anion to test and see if order of reactivity is correct for each anion Solution will always form an aqueous compound according to Alchem Table 4. Chose and Obtain Copper Used by different lab partners whose data was observed Carrying Out The Reactions & Collecting Data How Why 5.Place 10ml of water in a test tube Done so aqueous solution may be made 6. Take magnesium nitrate and place 3 drops into test tube with water Done to have one part of the reaction 7. Repeat step 5 and 6 but replace magnesium with zinc Done so 2 metals can be tested at the same time 8.
Lab #3/Limiting Reagents Abstract The purpose of this laboratory experiment was to determine whether an unknown compound was sodium carbonate or sodium hydrogen carbonate by reacting a sample of it with hydrochloric acid and comparing the resulting yield of NaCl to the calculated values. The mass of an evaporating dish was taken at the start of the experiment. Then the unknown carbonate A was added in the amount of approximately one gram. The dish was weighed once more to find the definite mass of the unknown carbonate. Then, by means of a dropper bottle and stirring rod, hydrochloric acid was added until all of the unknown carbonate appeared to have reacted.
Then the content of the chloride in the original salt is then calculated using stoichiometry (Chemistry Department, 2014). Theory: Gravimetric analysis is the measurement of mass, which by definition is categorized into four types however the use of one is only necessary in this experiment, which is precipitation (Gravimetric Analysis, 2012). Therefore the goal is to determine the original amount of ion. This is by isolating the ion in solution by a precipitation reaction, filtering and washing the precipitate free of pollutants, then the conversion of that precipitate to a product of the unknown sample given (Gravimetric Analysis, 2012).Therefore determining the quantitative of that substance by the precipitation reaction. The equation of the precipitate proceeds as follow if followed by the criteria given.
What are the identities of the substances found after electrolysis and heating? The identities of the substances found were Iodine, Iodide ion (I-), Triodide ion(I3-), Zinc metal and Zinc ion(Zn2+) Post Lab questions: 1. What did this experiment convincingly show about the composition of the white solid? I put that the experiment showed us the white substance was comprised of Zinc ions and iodide ions, and that the two ions and be separated back into their respective elements 2. During the electrolysis, a gray solid formed on the negative wire of the battery and the dark red solution formed at the positive wire of the batter.
The Ksp of Magnesium Oxalate Abstract The Ksp for the acid catalyzed titration of the saturated oxalate is 1.8 x 10-3. Introduction In this experiment, the solubility equilibrium for the salt magnesium oxalate must be found in order to determine a solubility product constant. Solubility equilibrium is a type of dynamic equilibrium which exists when a chemical compound in the solid state is in chemical equilibrium with a solution of that compound. At the point of equilibrium the solution becomes saturated. The chemical reaction used to find this constant is as follows: MgC2O4 (s) ↔Mg(aq)2++ C2O4 (aq)2- Kc= Mg2+[C2O42-][MgC2O4] Ksp=Mg2+[C2O42-] The solid salt magnesium oxalate is prepared through the following precipitation reaction: Mg(SO4)(aq)+NaC2O4 (aq) → MgC2O4 (s)+NaSO4 (aq) Next, the concentration of the Mg2+ and C2O42- ions is found through a redox titration.
Percent Copper and Formula Weight of a Copper Compound Introduction: In many chemistry problems, you are asked to calculate the percent composition of each element in a compound. In this experiment a variation of this basic calculation will be employed. The amount of copper in a compound will be determined by dissolving the unknown compound in water. The copper ions in solution will be converted to metallic copper by reaction with magnesium metal. To ensure that all of the copper is removed from solution, an excess of magnesium will be used.