||Explain the meaning of the terms "strong" and "weak" when applied
to acids and bases.
||Give illustrations of a strong acid, a strong base, a weak acid and
a weak base.
||Phosphoric acid is the acitve ingredient in many commerical rust-removing
solutions. Calculate the volume of concentrated phosphoric aicd (14.6
M) that must be diluted to prepare 500 mL of a 1.25 M solution?
||How did Arrhenius define and acid and a base?
||Pure HClO4 is molecular. Write an equation for its
disoolution in water.
||What is the difference between a strong electrolyte and a weak electrolyte.
||If asubstance is a weak electrolyte, what does this mean in terms
of the tendency of the ions to react to form the molecular compound?
How does this compare with strong electrolytes?
||Nitrous acid, HNO2, is a weak acid. Write an equation
showing its reaction with water.
||Hydrazine is a toxic substance that can be formed when household
ammonia is mixed with a bleach such as CloroxTM. Its formula
is N2H4 and it is a weak base. Write a
chemical equation showing its reaction with water.
||HClO3 is a strong acid. Write an equation for its
reaction with water.
||Formic acid, HCHO2, is the substance that is responsible
for the painful bites of fire ants. It is a weak electrolyte and reacts
with water in the same manner as acetic acid. Write a chemical equation
that shows its ionization in water.
||Write the formula for the conjugate bases for each of these acids:
|a) HCl; b) CH4; c) HSO3-1;
d) H2SO4; e) NH3;
||Show how each of these acids react with water and forms a conjugate
|a) HCl; b) HNO3;
c) H2SO4; d) HClO4;
e) H2S; f) H3PO4
||Calculate the molarity of a solution that contains 10 grams of HCl
in 100 mL of solution.
||A solution contains 0.1 mole of HC2H3O2
dissolved in 0.5 L of solution. Calculate the molarity of the solution.
||500 mL of a solution contain 0.1 mole of HC2H3O2.
The solution is diluted with water to the 1 L mark. Calculate the molarity
of the resulting solution.
||A 250 mL solution of H2SO4 has a strength of
0.2 M. The solution is diluted with water to the 1 L mark. What is the molarity
of the solution so formed?
||If 0.3 mole of acetic acid is present in 150 mL of solution, calculate
the molarity of the acid solution.
||How many moles of acetic acid are required to make 125 ml of a 0.5
||To what volume must 125 mL of a 2 M solution of HCl be diluted
to make the solution 0.05M?
||What is the concentration of a solution formed by diluting 300 mL
of a solution containing 0.1 mole of HCl to 6 L?
||Give directions for preparing 2.0 L of 0.250 mol/L HCl using 11.7
||Give directions for preparing 5.00 L of 0.15 mol/L H2SO4
using 18.0 M H2SO4.
||What volume of 2.00 mol/L HNO3 is needed to yield 10.00
grams of HNO3?