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57 Cards in this Set
- Front
- Back
properties of acids (4)
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1. aqueous solutions of acids conduct an electric current
2. acids react with certain metals to generate hydrogen gas 3. acids cause acid base indicators to change color 4. acids react with bases to form a salt and water=neutralization |
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neutrailization
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taking a strong acid and a strong base and combining them together to get something neutral (salt and water)
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properties of bases (3)
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1. aqueos solutions of them conduct an electric current
2. cause pH indicators to change color 3. react with acids to form salt water in a neautraliztion reaction |
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which are the strongest bases
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Group 1 + OH
as you move across the table --->, it gets less of a base |
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which are the strongest acids
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table K-top are stronger
HCl HNO3 HSo4 assume top 3 are 100% acidic |
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how to name binary acids
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hydro+ anion + ic
ex. HCl hydrochloric acid ex. HBr hydrobromic acid ex. HI hydroionic acid |
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how to name ternary acids
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ate-->ic
ite-->ous H2SO4- |
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pH
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the negative log of the hydrogen ion concentration
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pH of 1
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1 x 10^-1 M
or .1M |
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why do are some electrolytes weak
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have fewer ions in solution and less dissocation
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why does water have a pH of 7?
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equal number of protons and hydroxyls
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lewis acid
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substance that can accept a pair of electrons to form a covalent bond
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titration formula
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MaVa=MvVb
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conjugate acid-base pair
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consists of two substances related by the loss or gain of a single hydrogen ion
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conjugate acid/conjugate base
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ocnjugate acid= new acid that accepted the H
conjugate base=new base that lost the H |
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where are hydrolyzing salts usually derived from
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a strong acid and a weak base or a strong base and a weak acid
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hydrolysis of salts
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process of breaking salts by water
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acid+base-->?
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water + salt
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strong acid + weak base--> ?
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water + acidic salt
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weak acid + strong base--> ?
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water + basic salt
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strong acid + strong base--> ?
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water + neutral salt
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weak acid + weak base--> ?
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water + neutral salt
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what makes an acid weak/strong?
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# of hyudrogens that CAN dissociate and how many actually dissociate
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Ka
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ionization constant
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what is the strength of an acid the function of?
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dissociation
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which is a weaker acid
Ka= 1.5 x 10^-4 Ka= 1.3 x 10^-5 |
Ka= 1.3 x 10^-5 is weaker bc it has less particles
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how do you find the parent acids and bases
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positive ions goes with negative OH, negative ion goes with positive H
ex. NaCl Na+ and OH- Cl- and H+ parent acid= HCl parent base=NaOH |
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what is the pH of blood
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7.4
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what happens when you hold your breath
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pH drops
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evimivalence point
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the endpoint of a neautralization reaction
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titration reaction
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determines the molarity or concentration of an unknown substance
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endpoint
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neutral point
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standard solution
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the solution you know the pH of
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buffers
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something that resists change in pH
-made from a weak acid and one of its salts or a weak base and one of its salts |
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how do you determine whats an alcohol
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OH on the end of a carbon
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arrhenius acid
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substance whose water solutions contain hydrogen ions as the only positive ions
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base
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substance whose water solutions contain hydroxyl ions as the only negative ions
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Bronsted Lowry idea
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H+ does not exist on its own
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bronsted lowry acid
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anything that is a proton donor
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bronsted lowry base
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ANYTHING THAT IS A PROTON ACCEPTOR
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CONJUGATE acid-base pairs
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the one that loses the H and the one that gains the H on each side are pairs
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monoprotic/diprotic/triprotic acids
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mono=1 H
di=2 H tri=3 H |
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SAT 2 titration formula
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Ma x Va x # H+ = Mb x Vb x #OH-
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amphiprotic or amphteric
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can be either acids or bases
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5 ways to produce a salt
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1. neutralization ex. NaCl
2. double replacement- soluble solutions--> insoluble precipitate 3. acid + active metal-single replacement 4. synthesis (direct combination) 5. metallic oxide + nonmetallic oxide |
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what is H3O
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hydronium- it is an acid formed from a proton and water
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ionization
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in an aqueous solution, the process in which a molecular compounds reacts with water and forms ions
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dissociation
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when ionic compounds dissolve in water
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what is the different between a strong electrolyte and a weak electrolyte
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when a weak electroylte is in solution, only a fraction of the solute exists as ions. when a strong electrolyte is dissolved, almost all the solute exists as separate ions
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taste of acid
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sour
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taste of base
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bitter
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what is an electrolyte
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all ionic compunds that conduct an electric current
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why do acids act as electrolytes when combined with water
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water breaks acids into ions
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what is the difference between a weak arrhenius base and a strong arrhenius base
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the extent of dissociation of hydroxyls
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dissociation
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existing ions separate from each other
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brondsted lowry losses and gains
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stronger acids lose H+, weaker bases gain H+
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what is the definition of neautralization in the arrhenius system of acids and bases
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equalizing of hydrogen and hydroxyl ions
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