In the two cited molecules Br is more electronegative than I Therefore the O H

In the two cited molecules br is more electronegative

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In the two cited molecules, Br is more electronegative than I. Therefore, the O-H bond in HBrO 3 is weaker than the O-H bond in HIO 3 , so HBrO 3 is the stronger acid. b. HNO 2 , HNO 3 HNO 3 > HNO 2 . Four electronegative groups in HNO 3 , vs three in HNO 2 , result in a more polar O- H bond, and therefore a weaker O-H bond. K a HNO 3 large HNO 2 7.2 x 10 -4 c. HOCl, HOI HOCl > HOI . Cl is more electronegative than I. This results in a more polar O-H bond, and therefore a weaker O-H bond. d. H 3 PO 4 , H 3 PO 3 H 3 PO 4 > H 3 PO 3 . H 3 PO 4 has 5 electronegative groups separating the O-H as compared to the 4 electronegative groups in H 3 PO 3. This makes the O-H bond in H 3 PO 4 more polar and therefore weaker. Chem 162-2015 Chapter 17 Tro Acid-Base Equilibria 19
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STRENGTHS OF CARBOXYLIC ACIDS CH 3 CH 2 COOH Propanoic acid K a = 1.3 x 10 -5 I-CH 2 CH 2 COOH Cl-CH 2 CH 2 COOH CH 3 CHClCOOH CH 3 CCl 2 COOH 3-Iodopropanoic acid 3-Chloropropanoic acid 2-Chloropropanoic acid 2,2-Dichloropropanoic acid K a = 8.3 x 10 -5 K a = 1.0 x 10 -4 K a = 1.4 x 10 -3 K a = 8.7 x 10 -3 Chem 162-2015 Chapter 17 Tro Acid-Base Equilibria 20
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STRENGTHS OF AMINES AS BASES Recall that a Bronsted-Lowry base is anything that tends to react with a proton.
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