CH 18(CH 10 Kaplan) Acids and Bases Flashcards by K Matthews | Brainscape

Q

What is the definition or an Arrhenius Acid/Base?

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Q

What is the definition or an Arrhenius Acid/Base?

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Q

What is the definition of a Lewis Acid/Base?

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Lewis Acid = Electron Acceptor, has a vacant orbital to accept a lone pair

Lewis Base= Electron Donor

Most comprehensive definition

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Q

Lower the pKa the (stronger/weaker the acid)?

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Lower the pKa the stronger the acid

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Higher the pKa the (stronger/weaker the acid)?

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Higher the pKA = weaker acid

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Q

Higher Ka = stronger or weaker acid?

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Higher Ka = stronger acid

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Lower Ka = stronger or weaker acid?

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Lower Ka = weaker acid

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Q

What is the definition of a Bronsted-Lowry Acid?

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What is the definition of a Bronsted-Lowry Base?

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What is the definition of a Lewis Acid?

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What is a Lewis Base?

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What is the definition of a Lewis Acid-Base reaction?

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Donation and acceptance of a lone pair to form a covalent bond

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Which species are considered amphoteric? (3 answers)

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1) Partially dissociated conjugated base of polyvalent acid
2)Hydroxides of certain metals (Al, Zn, Pb, and Cr)
3)Oxidizing and reducing agents

Q

True or false: Every Arrhenius acid is a Bronsted-Lowry acid and every Bronsted-Lowry Acid is a Lewis Acid?

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True

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Which acid/base definition is considered amphiprotic?

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Bronsted-Lowry: can donate or accept a proton making it amphiprotic

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/(Electronegative elements positioned near an acidic proton ________ (increase/decrease) acid strength by__________________

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Electronegative elements positioned near an acidic proton INCREASE acid strength by pulling electron density away from the bond holding the proton

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What are the approximate pH values for these reactions?

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Periodic Table trends: Acidity _________ across a period and down a group

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