- Justin and Griff--0.07563
- Joe and Ben-- 0.07718
- Taylor and Nick-- 0.0727
- Henry and Evan-- 0.06379
- Matt Orians and Kyle-- 0.06697
- Charlie and Chris-- 0.0814
- Ryan and Jim-- 0.07667
- Donnie and Colby-- 0.07833
- Alex and Jacob-- 0.06356
- Will Long and Matt Johnson-- 0.07997
- Riley and Patrick Blose-- 0.07383
- Matt Farrel and Andrew Parmenter-- 0.06745
- Patrick "The Sweenenator" Sweeney and Peter-- 0.07885
Notes:
- The effect of temperature on the solubility of solids in liquids is more difficult to predict
- increasing the temperature increases the solubility of solids
- equivalent temperature increase can result in a large increase in solubility for some solvents and only a slight change for others
- in some cases, solubility of a solid decreases with an increase in temperature
- the formation of a solution is accompanied by an energy change.
- if you dissolve some KI in water you will find that the outside of the container feels cold to the touch
- if you dissolve some NaOH in water, the outside of the container feels hot
- the formation of a solid-liquid solution can apparently either absorb or release energy as heat
- before dissolving begins, solvent molecules are held together by intermolecular forces.
- in the solute, molecules are held together by intermolecular forces
- energy is required to separate solute molecules and solvent molecules from their neighbors
- a solute particle that is surrounded by solvent molecules is said to solvated
- the net amount of energy absorbed as eat by the solution when a specific amount of solute dissolves in a solvent is the enthalpy of solution
- the enthalpy of solution is negative (energy released) when the sum of attractions from Steps 1 and 2 is less than Step 3
- the enthalpy of solution is positive (energy absorbed) when the sum of attractions from steps 1 and 2 is less than Step 3
- the concentration of a solution is a measure of the amount of solute in a given amount of solvent or solution
- "dilute" just means that there is a relatively small amount of solute in a solvent
- note that these terms are unrelated to the degree to which a solution is saturated. a saturated solution of a substance that is not very soluble might be very dilute
- Molarity is the number of moles per solute in one liter of a solution
- to relate the molarity of a solution to the mass of solute present, you must know the molar mass of the solute. for example, a "one molar" solution of NaOH contains one mole of NaOH in every liter of solution
- the symbol for molarity is M, and the concentration of one molar solution of sodium hydroxide is written as 1 M NaOH
- one mole of NaOH has a mass of 40.0 g. If this quantity of NaOH is dissolved in enough water to make exactly 1.00 L of solution, the solution is a 1 M solution
molarity (M) = amount of solute (mol)/volume of solution (L)
- note that a 1 M solution is not made by adding 1 mol of solute to 1 L of solvent. in such a case, the final total volume of the solution might not be 1 L.
- the resulting solution is carefully diluted with more solvent to bring the total volume to 1 L
- see pages 420 and 421 for the answers and explanations of Sample Problems A, B, and C
- the lab is due tomorrow. dont forget to find the class avg and % error of the class average, as well as writing your conclusion
This site has some sample problems for molarity.
ReplyDeletehttp://www.chem.wisc.edu/deptfiles/genchem/sstutorial/Text11/molarity/molarityProb.htm
This site will help to explain molarity.
ReplyDeletehttp://dl.clackamas.edu/ch105-04/molarity.htm
This is a good site on molarity.
ReplyDeletehttp://www.fordhamprep.org/gcurran/sho/sho/lessons/lesson64.htm
Thanks Scheuner...
ReplyDeleteThis site talks about enthalpy of solution.
http://chemlab.truman.edu/CHEM120Labs/Calorimetry.htm
David and I's R value is .07475
ReplyDeletehttp://www.buzzle.com/articles/advanced-projects-in-chemistry-enthalpy-of-solution.html
ReplyDeleteThis site explains the enthalpy of solution.
Explaination of calculations with molarity:
ReplyDeletehttp://preparatorychemistry.com/Bishop_supersaturated.htm
http://www.graphpad.com/quickcalcs/Molarityform.cfm
ReplyDeleteHere is a molarity calculator.
http://cls.umc.edu/COURSES/LabMath/molarity.htm good site on molarity
ReplyDeletegood website on molarity.
ReplyDeletehttp://dl.clackamas.edu/ch105-04/molarity.htm
This comment has been removed by the author.
ReplyDeletehere's a nice site on molarity
ReplyDeletehttp://dl.clackamas.edu/ch105-04/molarity.htm
Here are some good Molality example problems:
ReplyDeletehttp://www.cartage.org.lb/en/themes/sciences/chemistry/generalchemistry/solutions/solubility/Solutionsindex/Molality/Molality.htm
remember that the lab is due today
ReplyDeletewebsite with molality practice problems
ReplyDeletehttp://chemistry.about.com/od/workedchemistryproblems/a/molality.htm