1. Calculate the concentrations of H3O+ and the pH of each acidic solution. Since HCl is a monoprotic acid
(an acid that donates only one proton or hydrogen atom permolecule to an aqueous solution), the H 3O
1. Calculate the concentrations of H3O+ and the pH of each acidic solution. Since HCl is a monoprotic acid, the H3O+ concentration is equivalent to the HCl molarity. To find the new pH values, you need to find the new concentrations. Remember M1V1 = M2V2
1. What was the level of background radiation you observed?
2. What are some of the sources of background radiation?
1. Record the radiation emitted from each of the materials. Subtract the background count to
obtain the radiatio
Titration of Strong and Weak Acids
1. Create a graph of pH vs. volume of added NaOH (mL) to the HCl solution of unknown concentration, to
produce a titration curve. Combine both
mL NaOH(x axis)
2. Find the equivalence point on the
1. Record and calculate the following masses:
mass of empty beaker (g)
mass of beaker plus Na2CO3 (g)
mass of Na2CO3 (g)
mass of beaker plus NaCl (after boiling off the water) (g)
mass of NaCl (d - a
1. Calculate the concentrations of H3O+ and the pH of each acidic solution. Since HCl is a monoprotic
acid (an acid that donates only one proton or hydrogen atom permolecule to an aqueous solution), the H3O+
concentration is equ
Oxidation States of Manganese
1. For each test tube - #3, #4 and #5 - record the following results of the reactions:
a Color of the solution
b Color of the precipitate, if any
pale pink in aqueous so
Chapter 19 #1
The atomic number sum and the mass number sum must remain the same on both sides of a
nuclear equation Use the atomic number to identify the element or par
Problems - Chapter 15 (with solutions)
1) What is the significance of the equilibrium constant? What does a large equilibrium
constant tell us about a reaction? A small one?
The equilibrium constant tells you the relationship between product and reactant
Answer to 586729
Stoichiometry of an Acid-Base Reaction Lab (Between HCl & Na2CO3 to produce
NaCl, CO2 & H2O)
After doing the lab these are the givens:
Total mass of empty beaker= 85.000g
After 2g Sodium Carbonate (Na2CO3) added total mass = 87.000g
First you need to find a balanced reaction:
2 MnO4- + 5 H2O2 + 6 H+ 8 H2O + 2 Mn+2 + 5 O2
Now that you have the reaction, you
1. For the NEW bottle of hydrogen peroxide, record and calculate the following:
a Volume of potassium permanganate used in each titration (mL)
b The volume of potassium permanganate req
1. For your most exact titration, record the following:
Volume of NaOH solution in the burette at the start (mL):
Volume of NaOH solution in the burette at the end (mL):
Volume of NaOH solution delivered to the flask
1. For each beaker, record the mass of the beaker plus the water and vinegar. Add the mass of the Alka Seltzer tablet
(3.0g) to the result. This is the initial mass.
2. Record the mass of the beaker with its solution after
Chapter 18 #1
(a)The problem is given in ionic form, so the halfreactions are
Chapter 24 #1
The molecule has a general formula C n H 2n , which means the isomers can have different
.alkenes and cycloalkane structures. Draw the longest chain carbon skel
Chapter 15 #1
Write the formula of the conjugate base for the following acids:
(a) HNO2 The conjugate base looks similar- missing a H+ = NO2(b) H2SO4 The conjugate base looks similar- missing a H+ = HSO4(c) H2S
Chapter 15 #2
Chapter 14 #1
Write equilibrium constant expressions for Kc and for KP for the following processes.
Assume that the partial pressures of the gases can be measured
2CO2(g) 2CO( g ) + O2(g )
Use the following model
Chapter 14 #2
Chapter 16 #1
Which of the following additions will result in a decrease in the pH of the solution?
Decreasing pH means an increase in H+, reactions that add H+ will lower the pH.
Adding ammonium nitrate to an ammonia solution
NH4+ NH3 + H+
Chapter 17 #1
Predict whether the entropy change is positive or negative for each of the following reactions.
2 KClO4( s ) 2 KClO3( s ) + O2(g )
H2O(g) H2O( l )
Entropy, S , is the measure of disorder or randomness of a system. Entropy increases with
Chapter 17 Worksheet: Thermodynamics
Q1. Which of the following processes are spontaneous and which are non spontaneous?
a) spreading of the fragrance of perfume/ air freshener in a room
b) cleaning your room
c) 2H2O (l) 2H2 (g
NVCC AL Campus CHM 112 Worksheet
Chapter 14: Chemical Equilibrium
Write the equilibrium expression for following reactions. Hint: what happens to liquids and solids in these expressions?
1) SO2 (g) + NO2 (g)
SO3(g) + NO (g)
2) 5 Fe2+ (aq) +
Chapter 15 Worksheet: Acids and Bases
The appropriate Ka or Kb values can be found in your textbook.
What are the conjugate bases of the following acids?
Chapter 12 Worksheet: Properties of Solutions
Which aqueous solution is likely to have a higher boiling point, 0.50 m NaCl or 0.50 m Na2CO3? Why?
Methanol (CH3OH) is soluble in water in all proportions. Explain why.
H bonds with
NVCC AL Campus CHM 112 Worksheet
Chapter 16 Aqueous Equilibria and Buffers
Look up the appropriate values of Ka, Kb or Ksp in your book.
Using the ICE table Calculate the pH of a solution that contains 0.075 M Nitrous acid and 0.085 M sodium n