Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride

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1 Acids and Bases

2 Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated acids have large molarities Ex: conc. HCl = 12M; H 2 SO 4 = 18M In the lab, we usually use dilute solutions Ex: 1.0M HCl, or 0.1M H 2 SO 4

3 Electrolytes Substances that, when dissolved in water, produce aqueous solutions that will conduct electricity Strong electrolytes release many ions Many ionic compounds Weak electrolytes release few ions

4 Autoionization of water Water molecules can react with each other H 2 O + H 2 O H 3 O + + OH - At 25ºC, [H 3 O + ] = [OH - ] [H 2 O] is a constant K w = [H 3 O + ] [OH - ] = 1x10-14

5 Let s use [H+] instead of [H 3 O + ] Pure water is neutral [H + ] = [OH - ] = 1x10-7 M If [H + ] > [OH - ], the solution is acidic If [H + ] < [OH - ], the solution is basic

6 ph scale Used to indicate how acidic ( [H + ] ) or basic ( [OH - ] ) a solution is tells how strongly acidic a solution is - NOT how strong an acid is! the lower the ph, the more H + s, the more acidic the solution

7 ph scale 0-2 strongly acidic 2-4 moderately acidic weakly acidic (7 = neutral) weakly basic moderately basic strongly basic

8 What is an acid? Brønsted/Lowry acid: a proton donor proton donor?... a proton is also an H + ion in water, H 2 O + donated H + H 3 O + H 3 O + = hydronium ion

9 Properties of acids React with most metals to produce H 2(g) react with carbonates to produce CO 2 taste sour damage living tissues ph 0-7 neutralize bases

10 Common acids Acid formulas usually start with H HCl hydrochloric acid H 2 SO 4 sulfuric acid HNO 3 nitric acid HClO 4 perchloric acid H 3 PO 4 phosphoric acid HC 2 H 3 O 2 acetic acid Also written CH 3 COOH (strong) (strong) (strong) (strong)

11 ph calculation ph = -log [H + ] [H + ] = 10 -ph

12 ph scale The ph is the measurement of how many H + s are in the water NOT a measure of if the H + s came from a strong or weak acid!!!

13 Acid Strength Compare the difference in these two statements: 1) The more H + ions in the water, the more acidic the solution 2) The more H + ions a compound produces, the stronger the acid

14 Acid Strength Strong acids release all of their H + ions [strong acid] = [H + ] Strong acids are strong electrolytes Weak acids hold on to most of their H + ions [weak acid]>>>[h + ] Weak acids are weak electrolytes Weak acids reach equilibrium with neutralization products

15 Don t get confused! A solution of a strong acid can actually be less acidic than a solution of a weak acid! IF: the strong acid solution is very dilute and the weak acid is concentrated! ex: HCl is a strong acid, but if in a solution [HCl] = 1x10-6 M, the ph = 6 and it is a weakly acidic solution of a strong acid.

16 What is an base? Brønsted/Lowry base: a proton acceptor proton acceptor?... any substance that will take an H + ion in water, H 2 O + base OH - + Hbase +

17 Properties of bases Commonly called antacids React with fats and oils to produce soap feel slippery taste bitter damage living tissues ph 7-14 neutralize acids

18 Common bases There are three common varieties of bases: 1) Hydroxide compounds (OH - ) ex: NaOH, Ba(OH) 2 2) Carbonates (CO 3 2- ) and bicarbonates (HCO 3- ) ex: Na 2 CO 3, NaHCO 3, CaCO 3 3) Ammonia (NH 3 ) and amines

19 poh calculation poh = -log [OH - ] [OH - ] = 10 -poh

20 ph & poh relationship In pure water at 25 C: [H+] = 1x10-7 M [OH-] = 1x10-7 M Therefore, [H + ] x [OH - ] = 1x10-14 And ph + poh = 14

21 the Big 5 ph = -log [H + ] [H + ] = 10 -ph poh = -log [OH - ] [OH - ] = 10 -poh ph + poh = 14

22 Hydroxide bases Soluble hydroxides release OH - directly into the water NaOH(s) Na + (aq)+oh - (aq) Strong bases = 100% of the OH-s released into water Alkali metals + Ba(OH) 2

23 Arrhenius Neutralization Works for the reaction of a strong acid with a strong base (OH - compounds) Remember acid (or base strength) has to do with how much of the acid (or base) ionizes in water, not directly how many H+ or OH- are present 100% ionization = strong

24 Arrhenius Neutralization Hydroxide base general form Strong Acid + Strong Base Salt + H 2 O what s actually happening? H + + OH - H 2 O Salt = the anion from the acid + the cation from the base ph = 7 at the end point (no excess reagents) Both products are neutral

25 Arrhenius Neutralization Examples with a hydroxide base NaOH + HCl NaCl + H 2 O H 2 SO 4 + Ba(OH) 2 BaSO H 2 O

26 What is an acid? Brønsted/Lowry acid: a proton donor proton donor?... a proton is also an H + ion in water, H 2 O + donated H + H 3 O + H 3 O + = hydronium ion

27 What is an base? Brønsted/Lowry base: a proton acceptor proton acceptor?... any substance that will take an H + ion in water, H 2 O + base OH - + Hbase

28 Brønsted /Lowry neutralization Acid 1 + Base 1 Acid 2 + Base 2 For weak acids and weak bases what s actually happening? Note the double arrow

29 Acid 1 + Base 1 Acid 2 + Base 2 Acid 1 H + + Base 2 Acid 1 donates H + and becomes Base 2, its conjugate base H + + Base 1 Acid 2 Base 1 accepts the H+ from Acid 1 and becomes Acid 2, its conjugate acid

30 Brønsted /Lowry neutralization Examples HF + H 2 O F - + H 3 O + HF donates an H + is an acid H 2 O takes the H + from the HF it is the base

31 Brønsted /Lowry neutralization HF + H 2 O F - + H 3 O + Look at the reverse reaction which donates an H+? it is an acid H 3 O + which takes the H+ from the H 3 O +? it is the base F -

32 Brønsted /Lowry neutralization HF + H 2 O F - + H 3 O + HF a weak acid becomes F -, a base H 2 O, acting as a base, becomes H 3 O +, an acid The acid becomes its conjugate base The base becomes its conjugate acid

33 Brønsted /Lowry neutralization Examples NH 3 + H 2 O NH 4+ + OH - H 2 O donates an H+ is an acid NH 3 takes the H+ from the H 2 O it is the base

34 Brönsted /Lowry neutralization NH 3 + H 2 O NH 4+ + OH - Look at the reverse reaction which donates an H+? it is an acid NH 4 + which takes the H+ from the NH 4+? it is the base OH -

35 Brönsted /Lowry neutralization NH 3 + H 2 O NH 4+ + OH - H 2 O a weak acid becomes OH -, a base NH 3, acting as a base, becomes NH 4+, an acid The acid becomes its conjugate base The base becomes its conjugate acid

36 Brønsted /Lowry neutralization a weak acid their conjugate + a weak base acid and base

37 Weak acids lose an H + and become their conjugate bases Weak bases gain an H + and become their conjugate acids

38 What is the conjugate base of HCl? HNO 3? Cl - NO 3 - HNO 2? NO 2 - NH 4+? NH 3 CH 3 COOH? CH 3 COO - H 2 CO 3? HCO 3 - HCO 3-? CO 3 2- H 3 O +? H 2 O

39 What is the conjugate acid of PO 3-4? HPO 2-4 HPO 2-4? H 2 PO - 4 H 2 PO 4-? H 3 PO 4 NH 2-? NH 3 NH 3? NH + 4 CH 3 COO -? CH 3 COOH HCO 3-? H 2 CO 3 H 2 O? H 3 O +

40 Did you notice that H 2 O was listed as an acid, and as a base but a pure H 2 O solution has ph = 7? H 2 O can act as an acid (lose an H + ) or a base (accept an H + ) depending on what it is combined with AMPHOTERIC: act as an acid when with a base; act as a base when with an acid

41 Acids and Bases

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