C401Ch16LN1 - Chapter 16: Applications of Aqueous...

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Chapter 16: Applications of Aqueous Equilibrium Neutralization Acid-Base Reactions In Ch 4.5 you learned that if you mix an acid and a base together, they will react together to produce water and a salt. This is called a neutralization reaction, as the acid and base neutralize each other (but the pH is not necessarily 7!). Neutralization rxns have very high K values, and so almost all go essentially to completion (except the weak acid/weak base case). There are 4 cases of neutralization rxns: Strong Acid-Strong Base LiOH + HBr ± LiBr + H 2 O The above is the classic neutralization rxn, water and a salt of a weak base is formed so the sln is neutral, and the pH at completion is 7. If you write the net ionic equation, you can see why the rxn goes to completion: What’s the K value for the above net ionic equation? Strong Acid-Weak Base 1) HI + NH 3 ± NH 4 I Hey, where’s the water? If you write the net ionic equation, you can see where it comes from: 2) 3) You should hopefully be able to predict whether the resulting solution is neutral, acidic, or basic: which is it and why? What’s the K value for equation 3) above? You may get it from the 2 following reactions: 4) OH - + H 3 O + ± 2 H 2 O 1/ K w = 1x10 14 + 5) H 2 O + NH 3 ± NH 4 + + OH - K b = 1.8x10 -5 = 3) K = ____________
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Weak Acid-Strong Base 6) HF + NaOH ± NaF + H 2 O Again, you should be able to figure out whether the resulting sln is neutral, acidic, or basic. Which is it and why?
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This note was uploaded on 06/25/2008 for the course CHEM 400-401 taught by Professor Dr.samples during the Fall '06 term at American River.

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C401Ch16LN1 - Chapter 16: Applications of Aqueous...

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