Unit 8 Flashcards by Ryan Deleon

Acids and bases modern inorganic definition

Bronsted-Lowry

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Acid

Any substance that can donate a H + ( proton)

HCl+H2O=H3O+ + Cl-
A. B. a. B

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Autoionization

Acid in water automatically forms ions

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Base

A substance that can accept a H + (proton)

NH3+HOH=NH4+ + OH-
B. a. A. B

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Hydronium ion

Acid

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Hydroxide ion

Base

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Characteristics of acids

Sour
Litmus red
Colorless in phenolphthalein 
Neutralize bases-forms h2o and salt
Corrosive-destroys metals liberates hydrogen gas ( oxidation)
Produces H3O+ in water
Formula starts with H
Dilution of acids exothermic

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Characteristics of bases

Bitter taste
Litmus blue
Pink in phenolphthalein
Neutralize acids-forms salt and h20
Caustic-skin irritant, destroys epidermis cells
Produces OH- in water 
Formula ends with -OH
Dilution of bases is exothermic
Hydrophilic-absorbs water from air

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Strong Acids-HCl

Hydrochloric acid

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Strong Acids-HBr

Hydrobromic acid

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Strong Acids-HI

Hydroiodic acid

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Strong Acids-HNO3

Nitric acid

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Strong Acids-HClO4

Perchloric acid

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Strong Acids-H2SO4

Sulfuric acid, 2protons=2 hydronium ions per molecule

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Strong Acids-HClO3

Chloric acid

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Strong acid definition

Ability of an acid to ionize 100% in water and produce 100% hydronium ions (H3O+)

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Strong bases definition

Ability of the base to dissociate 100% in water to produce 100% hydroxide ions (OH-)

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Strong bases to memorize

All group one metal hydroxides (LiOH, NaOH, KOH, RbOH, CsOH)

Only 3 group II hydroxides (Ca(OH)2, Ba(OH)2, Sr(OH)2

Reaction of acids-Ionization

HNO3+H20=H3O+ + NO3-
Nitric acid. Nitrate

Acid donates a proton to the water forming hydronium Ion and nitrate ion

Reaction of acids-Single replacement

Mg+2HBr=H2 + MgBr2

Metal replaces hydrogen in the acid forming hydrogen gas and salt. “Liberating”

Reactions of acids-neutralization

H2SO4 + 2NaOH=Na2SO4 + H2O
Sulfuric acid. Sodium hydroxide

Acid and base react to always form water (neutral) and salt

Neutralization reaction of HI + KOH

KI + H2O

In a neutralization reaction, moles of H3O+ always _____ moles of OH-

Equal

Dissociation of strong bases

LiOH + H2O

Break up

Li+ + OH- + H2O

Ionization of weak bases NH3 + H2O

Form new ions NH4+ + OH- Ammonium hydroxide

Amphiprotic substance

Can behave as a Bronsted acid (proton H+ loss) or a Bronsted base (gain protons H+). Water and ammonia are amphiprotic substances.

Conjugate acid-base pairs NH3 + H2O = NH4+ + OH-

Acid-base pair that are related through loss or gain of 1 proton H+. NH3 and NH4+ above are related and called a conjugate acid-base pair, as are H2O and OH-

General term "salts"

Any inorganic substance that does not fit the definition of an acid or a base is a salt. Or does not start with H and end with OH-

How to identify salts

Ionic salts dissociate in water and conduct electricity | Dilution of salts tends to be endothermic

Rules for naming binary acids (only 2 elements H + nonmetal)

Name begins with hydro (no O) 2nd part is nonmetal -change ending to ic and add acid Ex: HCl hydro-chloric-acid

Rules for naming oxyacids: H, nonmetal, and O

Polyatomic ions- - If ends in ate, change to ic - If ends in ite, change to ous - If it has one more O than ate ion add per with ic - if it has one less O than ite, use hypo H2SO4 sulfate= sulfuric acid HClO4 perchlorate= perchloric acid HClO hypochlorite= hypochlorus acid

Polyprotic acids

Have more than one ionizable hydrogen (proton) HCl Hydrochloric acid=1 monoprotic Sulfuric acid is diprotic. H2SO4 has 2 Phosphoric acid is triprotic H3PO4 has 3

Molarity

One mole of solute per liter of solution or mol/L

M1xV1=M2xV2

M1=most concentrated molarity V1=the volume of the most concentrated species M2= The dilute concentration V2=total volume. Includes V1 and water needed for dilution

To find the volume of water needed in a dilution, simply ______ V1 from V2

Subtract

V2=

V1 plus water added

Endpoint, equivalence, faint pink

In titration when neutralization is complete

MaxVa=MbxVb MAVA

Ma=molarity of the hydronium from the acid Va=volume of the acid used via the buret Mb=molarity of hydroxide from base Vb=volume of base used via the buret

H3O1+[OH1-]=1x10^-14M2

Kw or constant for water So OH=1x10^-14/H3O

pH scale 0-14, equation

0-7 acid 7 neutral 7-14 base (alkaline) pH=-log[H3O1+]

Kw or constant for water

H3O+ + OH-= 2 H2O and vice versa

H3O+(OH-)=

1x10^-14 M^2

7 strong acids

``` HCl Hydrochloric HBr hydrobromic HI hydroiodic HClO3 chloric HClO4 perchloric HNO3 nitric H2SO4 sulfuric ```