Notes Auto Ionization of Water

Ion product of water ion product constant kw equation

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Unformatted text preview: n Product of Water: -ion product constant: Kw -Equation: Kw= 1.0*10^(-14) -So, [H3O+][OH-]=[H+][OH-]= 1.0*10^ -14 -when [H+]=[OH-], solution is neutral ! The pH Scale: -pH=negative logarithm in base 10 of [H+] Ex/ pH=-log(1.0*10^-7)=7 -only numbers to right of decimal are significant in a logarithm -as [H+] increases, the pH decreases (negative) -look at equations in notebook ! Measuring pH: -pH meter -electrochemistry -voltage varies with pH -acid-base indicators: color change ! -a change in [H+] by a factor of 10 causes the pH to change by 1 ! Strong Acids: -you will recall that the seven strong acids are HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4 -These are, by definition, strong electrolytes and exist totally as ions in aqueous solution -for the monoprotic strong acids: [H3O+]=[acids] because it dissociates completely • -difference of 2 or greater of number of oxygens-number of hydrogens=expect it to be strong ! Strong Bases: -strong bases are the soluble hydroxides which are the alkali metal and heavier alkaline earth metal hydroxides (Ca2+, Sr2+, and Ba2+) -oxides of group one and group two metals -if you put an oxide in water, it becomes a strong hydroxide -dissociate 100% ! Dissociat...
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This document was uploaded on 03/26/2014 for the course CHEMISTRY AP Chemist at Lindbergh Sr. High.

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