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57 Cards in this Set

  • Front
  • Back
properties of acids (4)
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
taking a strong acid and a strong base and combining them together to get something neutral (salt and water)
properties of bases (3)
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
which are the strongest bases
Group 1 + OH
as you move across the table --->, it gets less of a base
which are the strongest acids
table K-top are stronger
assume top 3 are 100% acidic
how to name binary acids
hydro+ anion + ic
ex. HCl
hydrochloric acid
ex. HBr
hydrobromic acid
ex. HI
hydroionic acid
how to name ternary acids
the negative log of the hydrogen ion concentration
pH of 1
1 x 10^-1 M
why do are some electrolytes weak
have fewer ions in solution and less dissocation
why does water have a pH of 7?
equal number of protons and hydroxyls
lewis acid
substance that can accept a pair of electrons to form a covalent bond
titration formula
conjugate acid-base pair
consists of two substances related by the loss or gain of a single hydrogen ion
conjugate acid/conjugate base
ocnjugate acid= new acid that accepted the H
conjugate base=new base that lost the H
where are hydrolyzing salts usually derived from
a strong acid and a weak base or a strong base and a weak acid
hydrolysis of salts
process of breaking salts by water
water + salt
strong acid + weak base--> ?
water + acidic salt
weak acid + strong base--> ?
water + basic salt
strong acid + strong base--> ?
water + neutral salt
weak acid + weak base--> ?
water + neutral salt
what makes an acid weak/strong?
# of hyudrogens that CAN dissociate and how many actually dissociate
ionization constant
what is the strength of an acid the function of?
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
how do you find the parent acids and bases
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
what is the pH of blood
what happens when you hold your breath
pH drops
evimivalence point
the endpoint of a neautralization reaction
titration reaction
determines the molarity or concentration of an unknown substance
neutral point
standard solution
the solution you know the pH of
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
how do you determine whats an alcohol
OH on the end of a carbon
arrhenius acid
substance whose water solutions contain hydrogen ions as the only positive ions
substance whose water solutions contain hydroxyl ions as the only negative ions
Bronsted Lowry idea
H+ does not exist on its own
bronsted lowry acid
anything that is a proton donor
bronsted lowry base
CONJUGATE acid-base pairs
the one that loses the H and the one that gains the H on each side are pairs
monoprotic/diprotic/triprotic acids
mono=1 H
di=2 H
tri=3 H
SAT 2 titration formula
Ma x Va x # H+ = Mb x Vb x #OH-
amphiprotic or amphteric
can be either acids or bases
5 ways to produce a salt
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
what is H3O
hydronium- it is an acid formed from a proton and water
in an aqueous solution, the process in which a molecular compounds reacts with water and forms ions
when ionic compounds dissolve in water
what is the different between a strong electrolyte and a weak electrolyte
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
taste of acid
taste of base
what is an electrolyte
all ionic compunds that conduct an electric current
why do acids act as electrolytes when combined with water
water breaks acids into ions
what is the difference between a weak arrhenius base and a strong arrhenius base
the extent of dissociation of hydroxyls
existing ions separate from each other
brondsted lowry losses and gains
stronger acids lose H+, weaker bases gain H+
what is the definition of neautralization in the arrhenius system of acids and bases
equalizing of hydrogen and hydroxyl ions