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Study guide test 2

by: Erik Roseberry

Study guide test 2 CHEM 0970

Marketplace > Engineering and Tech > CHEM 0970 > Study guide test 2
Erik Roseberry
GPA 3.0
Chemistry 2
Dr. Maleckar

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Hey guys, this is study guide for test 2! Enjoy.
Chemistry 2
Dr. Maleckar
Study Guide
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This 3 page Study Guide was uploaded by Erik Roseberry on Saturday February 28, 2015. The Study Guide belongs to CHEM 0970 at a university taught by Dr. Maleckar in Fall. Since its upload, it has received 343 views.


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Date Created: 02/28/15
Erik Roseberry Dr Maleckar Chemistry 2 Notes Week 020615 Chapter 16 Chemical Equilibrium Part 1 Bronsted Acid substance that can donate a proton conjugate base bronsted acid after it has donated its proton Bronsted Base substance that can accept a proton The strength of an acid is determined by its tendency to ionize the stronger the bond of the molecule the harder it is to ionize the weaker the acid Oxoacids contain Oxygen Hydrogen and a nonmetal element the higher the electronegativity of the central atom the stronger the acid acid strength increases as more oxygens are attached to the central atom because polarity increases Water as a Bronsted AcidBase Water is both a bronsted acid and base because it can give and accept protons Water remains neutral because both happen simultaneously and are in equilibrium pH Scale pH scale is based on the log of the negative concentration of hydrogen protons ranges from 014 with 7 being neutral 2 is ten times more acidic than 3 pOH Scale sets 0 as basic and 14 as acidic Strong Acids and Bases Acids and Bases react until completion not equilibrium Strong Acids and Bases must react completely Strong Acids tend to be of low pH 02 Important Strong Acids Hydrochoric Acid HCI Hydrobromic Acid HBr Hydroiodic Acid H 4 Nitric Acid HN03 Choric Acid HC03 Perchoric Acid HCO4 SUfUFiC H2504 Ka is the equilibrium constant for acids Kb is the equilibrium constant for bases There are conjugate bases and conjugate acids that are determined by the loss or gaining of a proton 1 Sketch titration curves for the following acid base titrations a HCl versus NaOH b HCl versus CH3NH2 c CH3COOH versus NaOH In each case the base is added to the acid in an Erlenmeyer ask Your graphs should show the pH on the y axis and the volume of base added on the x axis 2 The pH of a bicarbonate carbonic acid buffer is 800 Calculate the ratio of the concentration of carbonic acid H CO to that of the bicarbonate ion HCO 3 A solution is made by mixing exactly 500 mL ofO 167 M NaOH with exactly 500 mL 0100 M HCOOH Calculate the equilibrium concentrations of H HCOOH HCOO OH and Na Amino acids are building blocks of proteins These compounds contain at least one amino group NHZ and one carboxyl group COOH Consider glycine NHZCHZCOOH Depending on the pH of the solution glycine can exist in one of three possible forms Fully protonated NH3 CH2 COOH Dipolar ion NH3 CH2 COO Fully ionized NH2 CH2 COO Predict the predominant form of glycine at pH 10 70 and 120 The pKa of the carboxyl group is 23 and that of the ammonium group NH3 is 96


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