ACIDSBASES ACIDS, BASES, & SALTS. Acids Properties of Acids 1.sour taste 2.electrolytes: - aqueous...
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Transcript of ACIDSBASES ACIDS, BASES, & SALTS. Acids Properties of Acids 1.sour taste 2.electrolytes: - aqueous...
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ACIDSACIDS, BASESBASES, & SALTS
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Properties of AcidsAcids1. sour taste2. electrolytes:
- aqueous solns conduct electric current
3. react with bases to form water and salt (neutralization reaction)
4. react with most metals to produce H2(g)5. acidds turn litmus paper redd
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ElectrolyteElectrolyte
• substance that dissolves in H2O to produce soln that conducts electric current
• acids, bases, & salts are electrolytes – form ions in H2O
HCl(s) H+1(aq) + Cl-1(aq)
NaOH(s) Na+1(aq) + OH-1(aq)
NaCl(s) Na+1(aq) + Cl-1(aq)
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Which metals react with acids?Which metals react with acids?
• See Table J
• All metals above H2 react with acids
• Cu, Ag, and AuCu, Ag, and Au do notnot react with acids
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2HCl + Mg MgCl2 + H2
• Mg above H2 so reaction proceeds
• single replacement reaction occurs
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Properties of BasesBases
1. bitter taste2. slippery or soapy feeling3. Electrolytes4. react with acids to produce
water and salt5.5. bbases turn litmus paper bblue
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Formula of Acid
• Format: HHX where X = nonmetal (F, Cl, Br, I)
or or X = negative polyatomic ion
• some acids have 2 or 3 HH’s–Ex: HHF, HH2S, HH3PO4
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Formula of Base
• Format: MOHOH where M is metal
•Ex: NaOHOH, Ca(OHOH)2
–exception: NH3 and NH4+1
• CH3OH is NOTNOT a base. WHY?
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Identify the Electrolytes• NaClNaCl
• CC22HH55OHOH
• HH22SOSO44
• NaOHNaOH
• CC66HH1212OO66
• CaICaI22
• HFHF
• Mg(OH)Mg(OH)22
• CC33HH77OHOH
• CClCCl44
• HNOHNO33
• CC55HH1212
• KK33POPO44
• CHCH33OCHOCH33
• LiOHLiOH
• HIHI
• (NH(NH44))22SOSO44
• CC1212HH2222OO1111
Yes - SYes - S
Yes - SYes - S
Yes - SYes - S
Yes - SYes - S
NONO
NONO
NONO
NONO
NONO
NONO
NONO
Yes - AYes - A
Yes - BYes - B
Yes - AYes - A
Yes - BYes - B
Yes - AYes - A
Yes - BYes - B
Yes - AYes - A
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Acid, Base, or Neutral?
• all H2O contains some H+1 and some OH-1 ions
– pure H2O: concentrations very low
• neutral solution: [H+1] = [OH-1]
• acidic solution: H+1 > OH-1
• basic solution: OH-1 > H+1
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Water & self-ionization
• H2O(l) + H2O(l) H3O+1(aq) + OH-1(aq)
HH33OO+1 +1 = hydronium ion
OHOH-1-1 = = hydroxide ion
• H2O(l) H+1(aq) + OH-1(aq)
H+1 and H3O+1 used interchangeably
HH+1+1 called proton or hydrogen ion
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Self-ionization of waterSelf-ionization of water
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Arrhenius Acid• substance that contains hydrogen &
ionizes to produce HH+1+1 ions in (aq) soln
HCl(g) HH+1+1(aq) + Cl-1(aq)
HNO3 HH+1+1(aq) + NO3-1(aq)
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Arrhenius Base
• substance that contains hydroxide group & ionizes to produce OHOH-1-1 ions in (aq) soln
NaOH(s) Na+1(aq) + OHOH-1-1(aq)
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Arrhenius Salt
• electrolyte where H+1 not only (+) ion and OH-1 not only (-) ion formed in aqueous solution
Ex: NaCl, CaBr2,KNO3, NH4I
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Salts in Water (ionic compounds)
• NaCl(s) Na+1(aq) + Cl-1(aq)
• CaBr2(s) Ca+2(aq) + 2Br-1(aq)
• KNO3(s) K+1(aq) + NO3-1(aq)
• NH4I(s) NH4+1(aq) + I-1(aq)
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Arrhenius Model has limitations
• Don’t always use H2O as solvent
– Arrhenius model only applies when H2O is solvent
• Doesn’t explain all cases:– NH3 (base) doesn’t contain OH-1 but it produces OH-1
NH3(g) NH4+1(aq) + OH-1(aq)
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Alternate Theory: Bronsted-Lowry
• Acid is a proton donorAcid is a proton donor• All Arrhenius acids = Bronsted-Lowry Acids
H+1
HX(g) + H2O(l) H3O+1 + X-1
HH+1+1 forms molecule-ion bond with water molecule HH33OO+1+1 (hydronium ion)hydronium ion)
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Bronsted-Lowry Acids
•HCl + H2O H3O+1 + Cl-1
•HNO3 + H2O H3O+1 + NO3-1
•H2SO4 + H2O H3O+1 + HSO4-1
•HSO4-1 + H2O H3O+1 + SO4
-2
H+1
H+1
H+1
H+1
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Bronsted-Lowry Base• Base is proton acceptorBase is proton acceptor
OH-1 is base
H+1 + OH-1 H2O
• not restricted to aqueous solution
NH3 + H2O NH4+1 + OH-1
NH3 is a base!
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Bronsted-Lowry Acids & BasesBronsted-Lowry Acids & Bases
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Amphoteric
• substance that acts as both acid & base
–H2O is amphoteric
HX(g) + H2O(l) H3O+1 + X-1 (base)
NH3 + HH22OO NH4+1 + OH-1
(acid)(acid)
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Water is amphoteric!Water is amphoteric!
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Naming Acids & Bases
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Naming Binary Acids
• Hydro + stem of nonmetal + ic
HF = ?
HCl = ?
H2S = ?
Hydrofluoric acid
Hydrochloric acid
Hydrosulfic acid
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Naming Ternary Acids
• Name derived from polyatomicpolyatomic anion (see Table E)
• Replace –iteite with –ousous , add acid
HNO2 is nitrous acid• Replace –ateate with –icic, add, add acid
HNO3 is nitric acid
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Ternary Acids
• polyatomics with S and P, make stem long again– H3PO4 = phosphoric acid, not phosphic acid
– H2SO4 = sulfuric acid, not sulfic acid
– H2SO3 = sulfurous acid, not sulfous acid
• SEE TABLE K
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Naming Bases
• Name the metal + hydroxide
NaOH = ?
Ca(OH)2 = ?
Mg(OH)2 = ?
Sodium hydroxide
Calcium hydroxide
Magnesium hydroxide