Molarity and Percent Solution Lab Essay

ObjectiveThe objective of this lab was to determine the meter and percent closure of a solving with an unknown concentration.Background mebibyte is the number of moles of a solute per liter of a solution. Percent solution is the part of a solute in a specific lot or saturation of a solvent. A solute is a solid that gets dissolved in a solvent or a liquid that is a smaller follow than the solvent. A solvent is a liquid that dissolves the solute and it always is a bigger amount. Solvation is when solute particles are surrounded by solvent molecules. A lab technique that was used during the lab was to boil the solution in order to freestanding the solute from the solvent.Materials List 10mL graduated cylinder solvent with unknown concentration sulphurous plate Pipette Hot grip Scale 100mL beakerProcedure1. detect the solution with the unknown concentration from Mrs. Magdaleno. 2. Measure the volume of the solution by pouring it in the 10mL graduated cylinder. Use the pipette to take stunned solution in the graduated cylinder until the volume was at 6mL. phonograph recording it in the info table. 3. Measure the empty 100mL beaker victimization the scale. Record it in the data table. 4. Pour the solution in the 100mL beaker.5. Find the mass of the beaker and solution using the scale. Make sure to subtract original beaker mass from the mass of the beaker and solution. 6. Boil the solution to separate the solute from the solvent by using the vitriolic plate set to nine. 7. Once all the water has dethawd use the red-hot grips to remove the beaker from the hot plate and let cool. Find the mass of the beaker and solute using the scale. Make sure to subtract beaker mass from the beaker and solute mass. 8. Use the data from the data table to solve for molarity and percent solution.Observations The water started to boil and evaporate when it was on the hot plate. It smelt like the common salt was burning. Some salt spil conduct protrude on the lab statio n when the water completely evaporated.selective information TableVolume of solution (L) 6mL=0.006L band of beaker (g) 68.95g Mass of solution and beaker(g) 75.06g Mass of solution(g) 6.12g Mass of solute and beaker(g) 69.41g Mass of solute(g) 0.46g ResultsA MolarityB Percent SolutionConclusionThe molarity that was calculated for the unknown solution was 1.31M. The percent solution that was calculated for the unknown solution was 7.52%. A procedural that would have led to a lower concentration value was when some salt spilled out onto the lab station after all of the water had evaporated from the beaker. A nonher erroneous belief that would result in a higher concentration would be if the beaker was not dry when the mass was measured with the scale. Something that could be done differently to aim to a more accurate concentration would be to take the beaker moody the hot plate sooner and not let the salt induct and burn or come out of the beaker.