Lecture #9 - Chemistry 2A-c w2009 (Ch5-17)64 VII. Acid-Base...

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Chemistry 2A Chemistry 2A -c w2009 c w2009 (Ch5 (Ch5 -17)64 17)64 VII. Acid-Base Titrations Example: HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) 1.00 M 2.00 M 100.0 mL ? mL(50 mL) When we say that we neutralize an acid or a base, we mean that the number of moles of H 3 O + (or H + ) ions = the number of moles of OH - ions Example: H 2 SO 4 (aq) + 2KOH(aq) K 2 SO 4 (aq) + 2H 2 O 0.100M 0.100 M 100.0 mL ? mL (200.0 mL ) Example: 2HNO 3 (aq) + Ba(OH) 2 (aq) Ba(NO 3 ) 2 (aq) + 2H 2 O(l) 0.100 M 0.100 M 100.0 mL ? (50.0 mL)
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Chemistry 2A Chemistry 2A -c w2009 c w2009 (Ch5 (Ch5 -18)65 18)65 Definition of Acids and Bases Arrhenius Definition (Based on water as a solvent) Acid : a substance increases the concentration of H + or H 3 O + in solution Example: HCl + H 2 O H 3 O + (aq) + Cl - (aq) or HCl(aq) H + (aq) + Cl - (aq) Strong acids: 100% ionized such as HCl weak acid such as CH 3 COOH, about <12% ionized Monoprotic acids : HCl, HBr, CH 3 COOH (or HAc) can only provide one H + Diprotic acids: H 2 SO 4 , H 2 S , , etc., can provide two H + Acidic anhydride: (an acid loses one water; non-metal oxide) SO 2 + H 2 O H 2 SO 3
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Chemistry 2A Chemistry 2A -c w2009 c w2009 (Ch5 (Ch5 -19)66 19)66 Bases : a substance increases the concentration of OH
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Lecture #9 - Chemistry 2A-c w2009 (Ch5-17)64 VII. Acid-Base...

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