The dissolving process involves a consideration of the relative strength of three intermolecular attractive forces. The type of forces between solute-solute molecules and solvent-solvent molecules must be considered. These intermolecular attractions must be broken before new solute-solvent attractive forces can become effective. A solute will dissolve in a solvent
First obtain 2 crucibles and lids. Label them #1 and #2. Make sure to clean the crucibles thoroughly. Now for part 1; weigh the crucible without the hydrate before heating. Then weigh the crucible without the hydrate after heating.
Computer Additivity of Heats of Reaction: Hess’s Law 18 (1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. (2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous solution of sodium chloride. NaOH(s) + H+(aq) ) + Cl–(aq) → H2O(l) + Na+(aq) + Cl–(aq) ∆H2 = ? OBJECTIVES • • • • In this experiment, you will Combine equations for two reactions to obtain the equation for a third reaction. Use a calorimeter to measure the temperature change in each of three reactions.
Objective The objective of this lab is to find the formula of an ionic compound. Materials: Copper Chloride Iron Chloride Sodium Hydroxide Well plate Indicator Toothpicks safety goggles pipets Procedures - collect materials label pipets according to the solutions inside. (CuCl, FeCl, NaOH, and the indicator) Using the pipet with the CuCl place 5 drops in the 5 wells in the well plate. Place one drop of indicator in those 5 wells. Starting on the 1st well place one drop of the NaOH at a time and mix with a toothpick until the NaOH has dissolved.
2) Predict which of the following in each set of compounds will have the highest water solubility. Which will have the lowest? Explain your answers. 3) Show how you could separate the components of the following mixtures. a) + O OH 1) dissolve in organic solvent like Et2O or CH2Cl2 2) add water solution of NaOH + O H2O layer O Et2O layer O O 1) add Et2O 2) add HCl OH O H2O layer Et2O layer 1) dry over MgSO4 2) remove Et2O NaCl O OH 1) dry over MgSO4 2) remove Et2O OH O b) O O + N 1) dissolve in organic solvent like Et2O or CH2Cl2 2) add water solution of HCl O O H2O layer + N H Et2O layer O N H O 1) dry over MgSO4 2) remove Et2O O O H2O layer Et2O layer 1) add Et2O 2) add NaOH N NaCl N 1) dry over MgSO4 2) remove Et2O N c) O O + N 1) dissolve in organic solvent like Et2O or CH2Cl2 2) add water solution of HCl O O H2O layer + N H Et2O layer O N H O 1) dry over MgSO4 2) remove Et2O O O H2O layer Et2O layer 1) add Et2O 2) add NaOH N NaCl N 1) dry over MgSO4 2) remove Et2O N d)
Identify the processes (e.g., coagulation) that were used in this lab and describe how they were performed. You start out with the contaminated water that has not been filtered out or has not had any chemicals added to it, this is many done so air can meet the water and this gives the chemicals and gases to release. I then added Alum to the dirty water since when mixing Alum with the dirty water it allows all the big particles to “stick” to the Alum and then pushes all of these particles to the bottom of the water. The dirty water is then put through a filter of sand, charcoal, and gravel in order for any of the smaller particles to stick to them and makes the water clean and free of any other particle. After I did all this I then had to add a few drops of bleach so I could disinfect the water from any other dirt
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.