Exam 3 NoteCard

Exam 3 NoteCard - -Hydroxides-Sulfides...

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Solubility : M a X b (s) ↔ aM b+ (aq) + b X a- (aq) K sp = [M b+ ] a [X a- ] b units (mol/L) ex. AgCl → Ag + + Cl - K f = formation constant ex. Ag + + (NH 3 ) 2 → Ag(NH 3 ) 2 + K = K sp * K f ex. AgAc ↔ Ag + + Ac - = K sp H + + Ac - ↔ HAc = 1 / K a AgAc + H + ↔ Ag + + HAc =K =K sp /K a Q = K sp Q > K sp Q < K sp ex. Q = [Ag + ] [Cl - ] - Insol. Salts whose anion is a conj. base of a weak acid will dissolve in a strong acid. - Salts whose anion is a conj. base of a weak acid will dissolved in H 2 O to greater extent than K sp Indicators: Noticeable color change = Base/Acid = 1/10 pH = pK a + log [Ind - ] / [HInd] pH = pK a – 1 Percent Ionized: ( [H + ] / [HA] ) * 100 Solubility Rules: Soluble Nitrates 1A metals Ammonium Chlorides (ex. Ag, Hg, Pb) Sulfates (ex. Pb, Ba, Sr) Insoluble ex(1A & ammonium)
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Unformatted text preview: -Hydroxides-Sulfides (S-2)-Carbonates-Phosphates Acid Strength: Strong HCl, HBr, HI, HNO 3 , HClO 4 , H 2 SO 4 Weak HF, HCN, H 2 S, HAc, RCOOH Base Strength: Strong 1A Metal OH, Ba(OH) 2 Weak NH 4 OH Acid, Base, Buffer &amp; Titration Equations: K w = [H 3 O + ] [OH-] = 1.0 E-14 pH = - log [H 3 O + ] pOH = - log [OH-] 14 = pH + pOH K w = K a * K b HA(aq) + H 2 O (l) H 3 O + (aq) + A-(aq) K a = [H 3 O + ] [A-] / [HA] K b = [OH-] [BH] / [B] pK a = - log K a Buffer w/ weak acid &amp; conj. base: [H 3 O + ] = [acid] / [conj base] * K a pH = pK a + log ( [conj. base] / [acid] ) Before equiv point of weak acid w/ strong base: [H 3 O + ] = K a ( [weak acid remaining] / [conj base produced] ) Half way point: pH = pK a...
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This note was uploaded on 04/29/2008 for the course CHEM 104 taught by Professor Tomasik during the Spring '08 term at Wisconsin.

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