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Acids & Bases

QuestionAnswer
Acid Taste sour
Acid Feel burn/itch
Acid Reaction reacts with active metals & produces H2 gas
Acid Electrolyte yes-conducts
Acid Corrosive yes-eats away
Base Taste bitter
Base Feel slippery
Base Reaction does not react
Base Electrolyte yes-conducts
Base Corrosive yes-eats away
Blue Litmus turns read in acid (B.R.A.) // stays blue in base
Red Litmus stays red in acid // turns blue in base (RB2)
Phenolphtalein clear/cloudy in acid // pink/magenta in base
Arrhenius In Acid produces H+ ions in a solution
Arrhenius In Base produces OH- ions in solution
Bronsted-Lowry In Acids H+ donor (proton donor)
Bronsted-Lowry In Bases H+ acceptor (proton acceptor)
Lewis In Acids e- pair acceptor (incomplete octet)
Lewis In Bases e- pair donor (central atom has unshared pair & non-metal ions)
Elements With Incomplete Octets group 13 & metal ions
Monoprotic vs Diprotic vs Triprotic mono: 1 ionizable hyrdogen // di: 2 ionizable hydrogen // tri: 3 ionizable hydrogens
Strong vs Weak Acids strong 100% ionize & weak partially ionize
Strong vs Weak Bases strong 100% dissociate & weak partially dissociate
General Neutralization Reaction acid + base = salt + water (salt is an ionic compund)
Amphoteric can act as an acid or a base
Conjugate Acid base H+ acceptor // what is formed after the base gains an H+
Conjugate Base acid H+ donor // what is formed after the acid loses an H+
Determining Reaction Direction RXN will move away from the stronger acid (strength chart)
Strong Acids Names hydrodic acid, perchloric acid, hydrobromic acid, hydrochloric acid, sulfuric acid, chloric acid, nitric acid
Strong Acid Formulas HI, HCLO4, HBr, HCl, H2SO4, HClO3, HNO3
Strongest Of The Weak Acids hydronium ion (H3O+)
Binary Acid an acid that contains only two different elements (prefix: hydro & suffix: ic)
Oxyacid an acid that is a compound of hydrogen, oxygen, & a third element (usually a non-metal)
The Stronger An Acid... the weaker the conjugate base
Proton-Transfer Reactions Favor... the production of the weaker acid and the weaker base
The 'pH' Equations Kw=[H+][OH-]=1.00x10^-14 // [H+]=10^-pH // [OH-]=10^-pOH // pH=-log[H+] // pOH=-log[OH-] // 14=pH+pOH
The "p" In "pH" Represents... mathematical "p-function"
A Titration Can Calculate... the concentration of an unknown acid
You Calculate The Amount Of Titration Delivered By... subtracting the initial volume from the final volume
Titrant the solution of the known concentration (standard solution)
Buret long tube used in titrations
Stopcock the stopper at the bottom of the buret to release the substance
A Titration Is Completed When... moles acids = moles base (eq. point)
The Equivalence Point Is Determined By... a pH meter & graph // an indicator
On A Graph, The Equivalence Point Is Found... in the middle of the straight line
Two Major Zones In A Titration Curve volume of base (base added to acid solution) & pH (pH electrode placed in acid solution)
Indicators Are Made From... color-changing compound based on the pH of the solution
Titration controlled neutralization reaction to determine unknown acid or base
A Strong Acid And A Strong Base Make... a neutral salt
A Strong Acid And A Weak Base Make... an acidic salt
A Weak Acid And A Strong Base Make... a basic salt
pH<7 acid
pH=7 neutral
pH>7 base
An Acid Is Strong If Its pH Is... less than two
A Base Is Strong If Its pH Is... greater than 12
Beaker Side Of A Titration Graph left
Buret Side Of A Titration Graph right
Buffer Region space on titration graph where the substance resists changes in pH
Created by: abievans
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