Acids and Bases Flashcards
acids examples
- hydrochloric acid.
- sulfuric acid.
- nitric acid.
- carbonic acid.
bases examples
- lithium hydroxide
- sodium hydroxide
- potassium hydroxide
- magnesium hydroxide
properties of acids
- react with bases to form water & a salt (neutralizations)
- change color of acid base indicators to litmus red
- reacts with some metals to product H2 gas
dilute acids
have a sour taste
aqueous solutions of are
electrolytes (strong or weak)
properties of bases
- react with acids to form water & a salt (neutralization)
- change color of acid-base indicators to litmus blue
aqueous solutions of bases
taste bitter & feel slippery
acid formula
- acids are a compound that products hydrogen ions (H+) when dissolved in water
- no oxygen present
so formulas of acids usually are in “HX”
- x can be monatomic or polyatomic
- focuses on naming the anion
naming acids
- if anion ends in ide-, acid becomes with hydro-.
suffix of anion changes to -ic and ends with acid - if anion ends in -ite, suffix of anion changes to -ous
ends with acid - if anion ends in -ate, suffix of anion is -ic
ends with acid
name of HBr
hydrobromic acid
name of H2S
hydrosulfuric acid
name of HNO2
nitrous acid
name of H2SO3
sulfurous acid
name of H3PO3
phosphorous acid
name of HNO3
nitric acid
name of H2CO3
carbonic acid
name of H3PO4
phosphoric acid
base formula
- base produces hydroxide ions when dissolved in OH
= if the base is an ionic compound (cation+anion), it is named like any ionic compound
dissociation of water
- “pure” h2o is not really pure
- h2o can disassociate just like ionic compounds in water into H+ and OH-
because water can do this, it plays a large role in acid base reactions
rate of water disassociation
only 1-2 water molecules out of 10 million are disassociated
hydrogen ions in water
- attracted to partial negative charge on oxygen
- form the ion hydronium H3O+
H3O+
H+
(they’re the same)
2 water molecules colliding
H2O+H2O –> H3O+ + OH-
H2O –> H+ +
OH-
self ionization of water
self ionization of water
within liquid water there is ac chemical reaction of water disassociating into H3O+ and OH-
ion-product constant for water (Kw)
Kw = [H+] x [OH-] = 1.0 x 10^14
Kw
KW ALWAYS EQUALS 1.0 x 10^14
the equilibrium constant when water goes through self-ionization
[H3O+][OH-] or Kw = [H+][OH-]
acidic solution example
HCl(g) → H+(aq) + Cl-(aq)
always:
[H+] is greater than 1.0*10^-7
basic solutions example
NaOH(s) → Na+(aq) + OH-(aq)
always:
[H+] is less than 1.0 x 10-7 M
[OH-] is greater than 1.0 x 10-7 M
pH
tells us about [H+] in a solution
ranges from 0-14
pH<7
acidic solution
pH=7
natural solution
pH>7
basic solution
pH formual
-log[H+]
[H+] formula
10^-ph
pOH
-log [OH-]
tells us about [OH-]
pH + pOH = 14
arrhenius acid
substance that yields H+ when dissolved in water
HCl(g) → H+(aq) + Cl-(aq)
OH-
-10^-pOH
tripotic acids
3 ionizable hydrogens (H3PO4)
arrhenius base
substance that yields OH- when dissolved in water
KOH(s) → K+(aq) + OH-(aq)
monoprotic acids
1 ionizable hydrogen (HNO3)
diprotic acids
2 ionizable hydrogens (H2CO3)
hydrogen ionizing
not all hydrogens ionize
CH3COOH(aq) → CH3COO-(aq)+ H+(aq)
brønsted-lowry
acids: H+ donor
base: H+ acceptor
amphoteric
- (water) can act as an acid and a base
conjugate pairs
2 substances that differ by 1 H+
each pair has one acid and one base
acids have the additional H+
lewis base
substance that can donate a pair of electron to form a covalent bond
6 strong acids
- HClO4
- HCl
- HBr
- HI
- HNO37
- H2SO4
lewis acid
substance that can accept a pair of electrons to form a covalent bond
identify parts
NH3 + H2O —> NH4+ + OH-
NH3 base
H2O acid
NH4+ conjugate acid
OH- base
NH3 NH4+ conjugate pair
H2O OH- conjugate pair
lewis acids need
dot structures to see electron pairs
strong acids
completely disassociate in water
HCl(g) → H+(aq) + Cl-(aq)
weak acids
only partially ionize
CH3COOH(aq) → CH3COO-(aq)+ H+(aq)
6 strong bases
- LiOH
- NaOH
- KOH
- CA(OH)2
- SR(OH)2
- BA(OH)2
salt
an ionic compound formed from an acid (anion) & a base (cation)
all neutralization rxns
double replacement rxns
acid base titrations
a method used to determine the concentration of a solution
makes use of neutralization reactions
- an indicator is added to signal when the neutralization has occurred
standard solution
the solution of known concentration
acid base titrations indicators
- the point when it changes colors is the end point
- end point / equivalence point is when neutralization has been reached
normality
(N) a unit of concentration used mainly in acid-base titration
- considers # of H+ or OH- ions in solition
titration formula
N1V1 = N2V2
titration for acids
- monoprotic: N=M
- diprotic: N=2M
- triprotic: N=3M
titration for bases
- for 1 OH- ion N=M
- for 2 OH- ion N=2M
- for 3 OH- ion N=3M
normality
20.0 g NaOH in 1.0 L of solution
20g * (1mol/40g) = 0.5 mol
0.5mol=1L=0.5M
1 OH so, 0.5N
hydrolysis
a reaction of a substance with water
salt hydrolysis
salts that react with water to form H+ or OH-
weak acids, strong bases
weak acids neutralized by strong bases produce basic salt solutions
K3PO4
strong acids, weak bases
strong acids neutralized by weak bases produce acidic salt solutions
NH4NO3
strong acids, strong bases
strong acids neutralized by strong bases produce neutral salt solutions
NaCL
buffers
- solutions that actively resist changes in pH
- remain constant when small amounts of acid or base are added
- a solution of a weak acid and one of its salts, or a solution of a weak base and one of its salts
- made of conjugate acid-base pairs
buffer, pH
buffer cannot control pH when too much acid or base is added
