Acids and Bases
Word Bank
Sour taste
OH
low pH
Blue Litmus
Paper -> Red
-log[OH]
Proton
Acceptor
Red Litmus
Paper-> Blue
good
conductor
Hydrogen
Donator
Slippery
Bitter Taste
pH < 7
-log[H3O]
Hydrogen
Acceptor
pH > 7
Proton
Donator
H30
pH of 9
Acids
Sour Taste
pH < 7
Low pH
-log[H3O]
Hydrogen Donator
H30
Proton donor
Bases
Slippery
OH
pH > 7
Proton Acceptor
pH of 9
Hydrogen Acceptor
-log[OH]
Fill in the blank with the correct name.
Bronsted-Lowry Definition is: The acid is the proton donor and the base is the proton
acceptor. ( When water gains a proton it is called Hydronium and when it loses a proton
it is called Hydroxide )
Lewis Definition is: The acid accepts an electron pair to form a covalent bond. The
base donates an electron pair to form a covalent bond.
Arrhenius Definition is: The acid releases H+ ions in (aq) solutions (HCl -> H+ + Cl)
The base releases OH- ions in (aq) solutions ( NaOH -> Na+ + OH-). Also, acids and
bases neutralize each other.
Naming Binary and Tertiary Acids
Name the given acids or write the chemical formula. ( ate = ic & ite = ous)
1) ____H3PO4____ = Phosphoric Acid
2) HF = ___Hydrofluoric Acid____
3) Bromous Acid = ___HBrO2_____
4) HNO3 = ______Nitric acid______
5) _____H2CO3_____ = Carbonic Acid
6)HCl = _____Hydrochloric acid____
Acid-Base Reactions (in aqueous solutions)
1) HF + __H2O___ <------> H30 + F
2) HPO4 + H20 <------> H2PO4 + __OH__
3) __NH3___ + H20 <-----> NH4 + OH
4) OH + HCN <-----> __H2O__ + CN
Neutralization Reactions of Acids and Bases
1) HCl + NaOH <------> __NaCl__ + H20
2) HF + NAOH <----> __H2O__ + NaF
3) H2CO3 + __H2O__ <-------> HCO3 + H3O 4) H2O + __HCl__ <------> H30 + Cl
pH/pOH and Hydronium/ Hydroxide Ion Concentrations ( round please)
pH
pOH
[H3O]
[OH]
Acid or Base?
3
11
1 X 10^-3
1 X 10^-11
Acid
5
9
3.5 X10^-5
1 X 10^-9
Acid
6
8
1X 10^-6
1X 10^-8
Acid
Titrations ( Fill in the Blank)
The controlled ___addition___ and measurement of the amount of a solution of a
known concentration required to react __completely____ with a measured amount of a
solution of an _____unknown_____ concentration.
Titration Problems
1) If 3 mL of 0.185mol/L of NaOH is used to neutralize HCl, what is the molarity of the
acid solution.
(0.185 mol/L) * ( 3.0 mL) = X * 80.0
.555 = x * 80.0
6.94 * 10^-3 = x
2) A teacher titrates a 10.00 mL sample of HBr with unknown molarity. The titration
requires 10.05 mL of a 0.1726 M solution of NaOH. What is the molarity of the HBr
solution?
10.05(0.1726)= 10(M)
1.73463/10=10M/10
M=0.1735
3)A flask is labeled 3.00M H2CO3. You decide to titrate a 15.00 mL sample with 1.85M
NaOH. What volume of NaOh solution would you expect to use if the label is correct?
H2CO3 + 2NaOH ----> Na2(CO3) + 2H2O
3.00 M = x Moles / 0.015 L = 0.045 moles
0.045 moles X (2 moles NaOH / 1 H2CO3) = 0.09
1.85 = 0.09 / x = 0.048mL
x = 48.6 mL
4) An 8.00 ml sample of an H2SO4 is titrated with 40.5 ml of 0.150M KOH. What is
concentration of the acid?
H2SO4 + 2KOH ----> K2SO4 = 2H2O
0.150 M = x moles / 0.0405 L = 0.00607
0.00607 X (1 mol H2SO4 / 2 mol KOH) = 0.00303 mol
0.00303 / 0.008 = 0.379 M