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Chemistry: Structure and Properties (Tro)
Chapter 8 Introductions to Solutions and Aqueous Reactions
A solute is _________________________________________________________________.
A solvent is __________________________________________________________________.
Molarity is _______________________________________________________________________
A strong electrolyte is _________________________________________________________
A weak electrolyte is ___________________________________________________________
A non-electrolyte is _______________________________________________________________
An acid is _________________________________________________________________
A weak acid is _________________________________________________________________
A strong acid is _________________________________________________________________
A base is _________________________________________________________
A weak base is ______________________________________________________________
A strong base is ______________________________________________________________
A precipitation reaction is _____________________________________________________
How can you predict if a precipitation reaction will take place?
Explain how a molecular equation, complete ionic equation and a net ionic equation differ.
How can you predict that a gas is produced in a chemical reaction?
How can you tell that a reaction is a redox reaction?
Write the formulas for these compounds:
Sodium chloride ___________ magnesium hydroxide ____________
Potassium nitrate _________________ calcium carbonate ________________
Lithium sulfate ________________ sodium sulfide ______________
ammonium nitrate ________________ potassium phosphate _____________
sodium sulfate _________________ silver nitrate _________________
- Calculate the molarity of a solution made by dissolving 15.5 g NaCl in water to yield 6 50.0 mL of
solution. (0.408 M)
- Determine the molarity of a solution made by dissolving:
a) 5.50 g of Mn(NO 3
2 in water to yield 1 50.0 mL of solution. (0.205 M)
b) 5.50 g of Mn(NO 3
2
โข 4 H
2 O in water to yield 1 50.0 mL of solution. (0.146 M)
- 15 0 mL of a 1.0 0 M HCl solution is diluted to 1.00 L with water. What is the concentration of the
new solution? (0.1 50 M)
- How many moles of HCl are in 2 5.0 mL of a 0. 25 M HCl solution? (0. 00625 moles)
- How many moles of glucose, C 6
H
12
O
6 , are in 3 5.0 mL of a 0.2 0 M glucose solution?
(0.0070 moles)
- 15 0 mL of a 2.5 M NaCl solution is mixed with 6 5 mL of a 1.8 M NaCl solution. What is the
concentration of the new NaCl solution? (2.3 M)
- How many milliliters of a 0. 250 M KNO 3
solution are needed to provide 0. 375 moles of KNO 3
( 1500 mL)
- What volume of a 0. 250 M Na 2
SO
4 solution is required to make 150.0 mL of 0.100 M Na 2
SO
4
solution? (60.0 mL)
- Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 12 M HNO 3
solution to 150.0 mL. (2.0 M)
- How many grams of KOH are in 250.0 mL of 0. 200 M KOH solution? (2.81 g)
- How many grams of NaCl are required to make 300 mL of a 2. 00 M NaCl solution? (35.1 g)
- A) What is the concentration of FeCl 3
in a solution prepared by dissolving 3 5 .0 g of FeCl 3
in
enough water to make 300 mL of solution? (0.718 M)
B) What is the concentration of the Fe
3+
ions? What is the concentration of the Cl
ions?
- What is the concentration (M) of a NaCl solution prepared by dissolving 5. 50 g of NaCl in
sufficient water to give 15 0 mL of solution? (0.627 M)
- What is the concentration of HCl in the final solution when 25 .0 mL of a 9. 0 0 M HCl solution is
diluted with water to a total volume of 0. 200 L? (1.13 M)
- A chemist wants to prepare 2.00 L of a 0.300 M CaCl 2 solution. How much CaCl 2
โข 2 H
2 O is
needed? (88.2 g)
- A solution is prepared by dissolving 2.50 g of CuSO 4
โข 5H
2 O in water to make 50 mL solution.
What is the molarity (molar concentration) of this solution? (0.20 M)
- The titration to the equivalence point of 80.0 mL of an unknown concentration H 3
PO
solution
requires 126 mL of 0.218 M KOH solution. What is the concentration of the H 3
PO
solution (in
M)? (0.114 M)
- a) A beaker contains 0.50 mol of potassium bromide in 600 mL of water. Calculate the molar
concentration of KBr in this solution. (0.833 M)
b) An additional 600 mL of water is added. The number of moles of potassium bromide in the
beaker is ____. What is the concentration of KBr in the final solution? (0.417 M)
- An aqueous solution of manganese (II) nitrate is combined with an aqueous solution of
ammonium sulfide. What precipitate will form? Write the equation of this reaction. (MnS)
- 6.74 g of the monoprotic acid HA (MM = 204.2 g/mol) is dissolved into water. The sample is
titrated with a 0.703 M solution of calcium hydroxide to the equivalence point.
a) Calculate the number of moles of HA ; b) Write and balance the chemical reaction ;
c) Calculate the volume of Ca(OH) 2 used. (23.5 mL)
- Write the reaction for dissolving each compound in water. Calculate the molar concentration of
chloride ions in each solution:
Solution Process of dissolution in water [Cl-], M
0.10 M NaCl
0.10 M MgCl 2
0.10 M AlCl 3
0.05 M CaCl 2
- A stock solution of contains 12.1 M of. If 25.0 mL of the stock solution is diluted to
a final volume of 0.500 L. What is the molar concentration of HNO 3 in the diluted solution?
(0.605 M)
- How many milliliters of 0.260 M Na 2
S are needed to react stoichiometrically with 25.00 mL of
0.315 M AgNO 3
Na 2
S (aq) + 2 AgNO 3
(aq) โ 2 NaNO 3
(aq) + Ag 2
S (s) (15.1 mL)
- How many grams of H 2
gas can be produced by the reaction of 63.0 g of Al(s) with an excess of
hydrochloric acid in the reaction shown below?
2 Al (s) + 6 HCl (aq) โ 2 AlCl 3
(aq) + 3 H 2
(g) (7.0 g)
- Based on the solubility rules, which compounds should be soluble in water?
- Based on the solubility rules, which compounds are insoluble in water?
- Write a balanced ionic equation that describes the process of dissolving the following
compounds in water: Na 2
CO
3 , NaOH, K 2
SO
4
, CH
3
COOK, NH
4
NO
3 , HCl, NH 4 Cl , NaHCO 3
NaCl (s) Na
+
(aq) + Cl
-
(aq)
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
(NH
4
3
PO
4
Ca 3
(PO
4
2
AlPO 4
Ag 3
PO
4
Na 3
PO
4
CaCO 3
(NH
4
2
CO
3
Na 2
CO
3
MgCO 3
KNO
3
- A volume of 250.0 mL of 0.05 M HCl is added to 100.0 mL of a 0. 0 75 M Mg(OH) 2 solution.
Will the resulting solution be basic, neutral or acidic? Answer the question by finding the reagent
in excess. (basic)
- Write the net ionic equation for a neutralization reaction.
- The following redox reaction is used to calculate the concentration of a hydrogen peroxide
solution:
2 KMnO 4
+ 5 H
2
O
2
+ 3 H
2
SO
4
โ 5 O
2
+ K
2
SO
4
+ 8 H
2
O
A sample of 2 0 .0 mL of a hydrogen peroxide solution of unknown concentration was titrated to the
equivalence point with 20.8 mL of a 1.0 M KMnO 4
. Using the stoichiometry of the reaction above
calculate the molar concentration of the hydrogen peroxide solution. (2.6 M)
- A) Write the reaction between H 2
SO
4 and KOH.
B) What is the concentration of a sulfuric acid solution if 50.0 mL of H 2
SO
4 were titrated to the
equivalence point using 22.1 mL of a 0.50 M KOH. (0.11 M)
- A) Write the reaction between H 2
SO
4 and KOH.
b) The titration to the equivalence point of 25.0 mL of an unknown concentration H 2
SO
solution requires 80.6 mL of 0.125 M LiOH solution. What is the concentration of the H 2
SO
solution (in M)? (0.202 M)
47. For each reaction:
- Write the oxidation state on every atom.
- Write the two half-reactions and label the oxidation reaction and the reduction reaction
- Balance the reaction using the half-reaction method
a) NaClO 3 (s) โ NaCl(s) + O 2 (g)
b) Al 2
O
3
c) Cu(NO 3
2
2
d) NaI + Cl 2 โ NaCl + I 2
e) Zn + HCl โ H 2
f) Cu + HNO 3 โ Cu(NO 3
2
+ NO + H
2
O
g) CH 4
+ O
2
โ CO
2
+ H
2
O
