exam 2

exam 2 - Exam 2 Bases: strong acids and strong bases are...

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Exam 2 Bases: strong acids and strong bases are strong electrolytes strong acids are: HCL, HBr, Hl,HClO 3 HClO 4 H 2 SO 4 and HNO strong bases: group 1A metal hydroxides, CA(OH)2, Ba(OH)2, and Sr(OH)2 weak acids and weak bases are weak electrolytes potentially dissociate or ionize in H2O weak acids include: HF, H2SO3, HClO and HNO2 weak bases include: NH3, Fe(OH), and Cr(OH)2 Neutralization reactions and salts neutralization occurs when there is a reaction between an acid and a base Skip section 4.4 Section 4.5 Concentration of solutions concentration--quality of solute contained in a quantity og solution molarity--term used to define concentrations units = moles/liter by knowing molarity of a quantity of liters of solution, one can determine the number of moles of solute Molarity: 3 quantities (molarity, moles solute, liters of solution) If we know 2, we can get the 3 rd Molarity = moles of solute / liters of solvent Dilution--changing the concentration of the solution by addition of solvent the moles of solute is the same in the concentration and dilute forms of the solution M.concentrated X V.concentrated = M. Dilute X V. dilute M1V1 = M2V2 or M. known(V. known) = M. unknown (V. unknown) you are given a solution of 14.8 M NH3, How many milliliters od this solution do you require to give 100ml of 1.00 M NH3 when diluted section 4.6 Solution stoichiometry and chemical analysis titration: a neutralization reaction between an acid and a base a solution of know concentration is used to determine the concentration of an unknown solution the point at which stoichiometrically equivilent quantities of reactants are brough together is called equivilanve point/ end point the indicator: signals the endpoint by changing colors
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This note was uploaded on 04/25/2008 for the course V 011 taught by Professor Staff during the Fall '06 term at NYU.

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exam 2 - Exam 2 Bases: strong acids and strong bases are...

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