'Nh 4 nh 3' diaporamas de présentation

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ACIDS & BASES Acids: - acids are sour tasting - Arrhenius acid: Any substance that when

ACIDS & BASES Acids: - acids are sour tasting - Arrhenius acid: Any substance that when dissolved in water, increases the concentration of hydronium ion (H 3 O + ) - Bronsted-Lowry acid: A proton donor - Lewis Acid: An Electron acceptor Bases:

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??? ?????? acid-base disturbance

???????? ------- ?????. ??? ?????? acid-base disturbance. ???? ??????????????????? ????????????? ???????????. ????????????. ?. ?? ?????????????????. ?????? H ? ? ???. ?? HCl H 2 SO 4 H 2 CO 3 NH ? 4. CO 2. CO 2. H 2 CO 3. ????. CO 2. CO 2. H 2 O. ?????. ????????.

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??? ?????? acid-base disturbance

??? ?????? acid-base disturbance. ???? ??????????????????? ????????????? ???????????. ????????????. ???????????????????. ?????? H ? ? ???. ?. ?? HCl H 2 SO 4 H 2 CO 3 NH ? 4. CO 2. CO 2. H 2 CO 3. ????. CO 2. CO 2. H 2 O. ?????. ????????. H 2 SO 4 H 3 PO 4

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??? ?????? acid-base disturbance

??? ?????? acid-base disturbance. ???? ??????????????????? ????????????? ???????????. ????????????. ???????????????????. ?????? H ? ? ???. ?. ?? HCl H 2 SO 4 H 2 CO 3 NH ? 4. CO 2. CO 2. H 2 CO 3. ????. CO 2. CO 2. H 2 O. ?????. ????????. H 2 SO 4 H 3 PO 4

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??? ?????? acid-base disturbance

??? ?????? acid-base disturbance. ???? ??????????????????? ????????????? ???????????. ????????????. ???????????????????. ?????? H ? ? ???. ?. ?? HCl H 2 SO 4 H 2 CO 3 NH ? 4. CO 2. CO 2. H 2 CO 3. ????. CO 2. CO 2. H 2 O. ?????. ????????. H 2 SO 4 H 3 PO 4

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Acids and Bases

Acids and Bases. Properties of Acids. They are corrosive pH range is 0 to 7, lower the pH, more acidic the acid Taste sour Turns litmus paper red Often reacts with metals to produce H 2 gas Often produces H+ in water. Example; HCl ? H + + Cl -. Symbol used for acids.

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Acids and Bases

Acids and Bases. Properties of Acids. They are corrosive pH range is 0 to 7, lower the pH, more acidic the acid Taste sour Turns litmus paper red Often reacts with metals to produce H 2 gas Often produces H+ in water. Example; HCl ? H + + Cl -. Symbol used for acids.

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EQUILBRIUM OF Acids and Bases

EQUILBRIUM OF Acids and Bases. Chapter 17. Water. AUTOIONIZATION. H 2 O can function as both an ACID and a BASE. Equilibrium constant for water = K w K w = [H 3 O + ] [OH - ] = 1.00 x 10 -14 at 25 o C. Water. K w = [H 3 O + ] [OH - ] = 1.00 x 10 -14 at 25 o C

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EQUILBRIUM OF Acids and Bases

EQUILBRIUM OF Acids and Bases. Chapter 17. Water. AUTOIONIZATION. H 2 O can function as both an ACID and a BASE. Equilibrium constant for water = K w K w = [H 3 O + ] [OH - ] = 1.00 x 10 -14 at 25 o C. Water. K w = [H 3 O + ] [OH - ] = 1.00 x 10 -14 at 25 o C

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pH = p K a2 pH = p K a1

Acids and Bases in aqueous solution. p K a2 = 2.33. p K a1 = 9.45. pH = p K a2 pH = p K a1. The properties of water:. Water is held together by H-bonding, which gives it its surprisingly high B.Pt. and M.Pt. for such a small molecule. Note that

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General properties

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Acid-Base Pairs

Acid-Base Pairs. H 2 O + NH 3 ? OH - + NH 4 + acid base base acid H 2 O/OH - are an acid-base pair hydroxide ion is the conjugate base of water NH 4 + /NH 3 are an acid-base pair ammonium ion is the conjugate acid of ammonia.

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TITRATION OF A WEAK ACID WITH A STRONG BASE

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