Download Chapter 4 Solution Stiochiometry

Problem 4.22 (b)
• Write ionic and net ionic equations for:
K3PO4 (aq) + Sr(NO3)2 (aq) 
Problem 4.34
• Balance the following equation and write the
corresponding ionic and net ionic equations
(a) CH3COOH (aq + KOH +
Problem 4.50 (a, b, c, d)
• Give oxidation numbers for all atoms in:
Mg3N2, CsO2, CaC2, CO32-
Problem 4.54
• Predict the outcome of the reactions
represent by the following equations by using
the activity series, balance the equations.
• (a) Cu(s) + HCl (aq) 
• (c ) Mg(s) + CuSO4 (aq) 
Problem 4.56
• Classify the following redox reactions.
• (a) P4 + 10Cl2  4PCl5
• (b) 2NO  N2 + O2
• ( c ) Cl2 + 2KI  2KCl + I2
SOLUTION STOICHIOMETRY
TITRATION
• SOLUTION
• CONCENTRATION OF SOLUTION
Conc = amount solute/amount solvent
DILUTION OF A SOLUTION
Solution Stoichiometry
• The concentration of a solution is the amount
of solute present in a given quantity of solvent
or solution.
M = molarity = moles solute/liters of
solution
• Calculate the moles of KI required to prepare
5.00 X 102 mL of a 2.80 M solution.
PROBLEM 4.59
• Calculate the mass of KI IN GRAMS REQUIRED
TO PREPARE 5.00 X 102 mL of a 2.80 M
solution.
Preparing a Solution of Known Concentration
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PROBLEM 4.62
• HOW MANY GRAMS OF KOH ARE PRESENT IN
35.0 mL OF A 5.50 M SOLUTION?
Problem 4.64 (a)
• Calculate the molarity of each of the following
solutions.
(a) 6.57 grams of ethanol (C2H5OH) in 1.50 x 102
ml of solution.
Dilution is the procedure for preparing a less concentrated
solution from a more concentrated solution.
Dilution
Add Solvent
Moles of solute
before dilution (i)
MiVi
=
=
Moles of solute
after dilution (f)
MfVf
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• How would you prepare 60.0 mL of 0.200 M
HNO3 from a stock solution of 4.00 M HNO3?
Mi Vi = Mf Vf
PROBLEM 4.70
• WATER IS ADDED TO 25.0 ML OF A 0.866 M
KNO3 SOLUTION UNTIL THE VOLUME OF THE
SOLUTION IS EXACTLY 500 ML. WHAT IS THE
CONCENTRATION OF THE FINAL SOLUTION?
Titrations
In a titration a solution of accurately known concentration is added gradually added to
another solution of unknown concentration until the chemical reaction between the two
solutions is complete.
Equivalence point – the point at which the reaction is complete
Indicator – substance that changes color at (or near) the
equivalence point
Slowly add base
to unknown acid
UNTIL
the indicator
changes color
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Titrations can be used in the analysis of
Acid-base reactions
H2SO4 + 2NaOH
2H2O + Na2SO4
Redox reactions
5Fe2+ + MnO4- + 8H+
Mn2+ + 5Fe3+ + 4H2O
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TITRATIONS: EQUIVALENCE POINT
• MOLES OF ACID = MOLES BASE
• (MOLES/LITER) ( LITERS) = (MOLES/LITER) (LITERS
PROBLEM 4.87
• CALCULATE THE VOLUME IN mL OF A 1.420 M
NaOH SOLUTION REQUIRED TO TITRATE THE
FOLLOWING SOLUTIONS?
• (a) 25.0 mL OF A 2.430 M HCl SOLUTION
• (b) 25.00 ML OF A 4.500 M H2SO4 SOLUTION
Problem 4.88 (a)
• What volume of a 0.500 M HCl solution is
needed to neutralize each of the following:
• (a) 10.0 mL of a 2.430 M HCl solution