- forward and backwards o Strong bases = soluble metal hydroxides(in general if it has OH it’s a strong base o Weak base = example is ammonia

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Monday, September-20-10 - Balanced right side of slide 22 = 14 mno 4 - + 3c 3 o 3 h 8 14mno 2 + 2 co 2 + 7co 3 2- + 12H 2 o Acid-Base reactions - Properties common to all acids o Sour o Turn litmus paper red o Reacts with metals H 2 (g) Due to H 3 o (aq) hydronium cation o Bronsted definition (1923) Acid = H + donor Base = H + acceptor o A-H + :B A - + BH + (needs at least one lone pair and one H atom) The acid must have one H atom to give away
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While the base needs to have at least one pair because it needs to accept an H and needs to give pairs in return. o Strong acids complete ionization in water o Weak acids partial ionization in H 2 0 o If it’s a weak acid there is chemical equilibrium where the reaction goes
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Unformatted text preview: forward and backwards o Strong bases = soluble metal hydroxides (in general if it has OH it’s a strong base) o Weak base = example is ammonia which is used frequently in the lab, only example that seems we should worry about – go through chemical equilibrium -Other basic compounds : Alkali oxides, and Alkali hydrides o Aqueous acid-base reaction (neutralization) HBR + naOH naBr + H 2 o • After using the net equation and putting everythin into its ions and removing all the spectator ions you obtain the net ionic equation of o H + + OH- H 2 o o Redox reactions in steel making...
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This note was uploaded on 10/22/2010 for the course PHYSICS 1D03 taught by Professor N. mckay during the Spring '08 term at McMaster University.

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- forward and backwards o Strong bases = soluble metal hydroxides(in general if it has OH it’s a strong base o Weak base = example is ammonia

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