AP Chemistry- Chapter 4 Worksheet
1.
What is the difference between a strong acid and a weak acid?
2.
Acetic acid, HC2H3O2 is a weak electrolyte. What solute particles are present in the
solution?
3.
Identify the precipitate formed in a reaction between solutions of Barium nitrate and
sodium sulfate.
4.
Which of the following solutions is the most basic (has largest concentration of OH-1in
solution); 0.15 M KOH, 0.10 M Ba(OH)2 or 0.10 M Al(OH)3
4.
Calculate the molarity of K+1 ions in a solution made when 250. mL of 0.10 M K2SO4 is
added to 250. mL of 0.10 M KNO3
5.
Complete the following reactions and then write balanced net ionic reactions
A)
Barium Nitrate (aq) + Sodium carbonate (aq)
B)
Ammonium chloride (aq) + silver nitrate (aq)
C)
Chromium III sulfate (aq) + ammonium carbonate (aq)
D)
Fluorine (g) + Sodium iodide (aq)
E)
potassium (s) + calcium chloride (aq)
6.
Calculate the molarity of a solution created when 2.05 grams of KI is added to 450 mL of
water.
7.
Calculate the mass of NaNO3 needed to make a 250 mL 0.25 M solution of NaNO3
8.
How much water should be added to 0.25 grams of K2O in order to form a 0.12 M
solution?
9.
A solution of 125 mL 0.15M H3PO4 is neutralized with 175 mL of NaOH.
10.
A)
Write the complete balanced equation for the reaction
B)
How many moles of acid are there in this reaction?
C)
How many moles of base are needed to neutralize the acid?
D)
Find the molarity of the base used to neutralize this acid.
Describe how you would make a 200. mL 0.10 M HCl solution from 12.0 M HCl. Support
your answers with calculations.
11.
A reaction between 125 mL 0.10 M Na3PO4 and 175 mL 0.15 M Ba(NO3)2 occurs.
A)
Write the balanced equation of the reaction
B)
Write the balanced net ionic equation
C)
Identify the limiting, support your answer with calculations
D)
Find mass of precipitate form
E)
Find molarity of all remaining ions in the solution.