Question 1. Dscribe the change you observed when you added 1 mL of 0.pdf

Question 1. Dscribe the change you observed when you added 1 mL of 0.1 M KSCN to the 2 mL
portion of the diluted solution. Copy the equation from the procedure and explain your
observations in terms of LeChatelier’s Principle. Choose the best answer.
The additional thiocyantate ion shifted the equilibrium toward the products, producing
morehexathiocyanatoferrate(III) lightening the color.
Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq).
The additional thiocyantate ion shifted the equilibrium toward the reactants, producing
lesshexathiocyanatoferrate(III) and deepening the color.
morehexathiocyanatoferrate(III) and deepening the color.
Question 2. Show your calculations to determine the final volume of the 0.001 M FeCl3 solution.
Choose the best answer.
M1V1 = M2V2.
(0.001 M)V1=(0.1 M)(0.05 L)
V1=0.050 L = 50 mL
M1V1 = M2V2.
(0.001 M)V1=(0.1 M)(0.005 L)
V1=0.500 L = 500 mL
M1V1 = M2V2.
(0.1 M)(0.005 L)=(0.001 M)V2
V2=0.500 L = 500 mL
M1V1 = M2V2.
(0.1 M)(0.0005 L)=(0.001 M)V2
V2=0.050 L = 50 mL
Question 3. Describe the change you observed when you added 1 mL of 0.1 M FeCl3 to the
diluted mixture of 0.001 M FeCl3(aq) and 0.1 M KSCN(aq). Refer to the equation in step 1 and
explain your observations in terms of LeChatelier’s Principle. Choose the best answer.
Additional iron(III) ion shifted the equilibrium toward the products to form the red-colored
hexathiocyanatoferrate(III) complex and the intensity of color increased.color.

Additional iron(III) ion shifted the equilibrium toward the products to form the red-colored
hexathiocyanatoferrate(III) chloride precipitate.
Fe3+(aq) + 6SCN-(aq) Fe(SCN)6Cl3(s).
Additional iron(III) ion caused the equilibrium to shift to the reactants to compensate for the
additional added iron(III), which increased the intensity of the red color.
Additional iron(III) ion increased the concentration of the red-colored iron(III) ion.
Question 4. Predict and then describe what happened when you added HCl(aq) to the copper
nitrate solution. Write down the equation for the reaction. Choose the best answer.
The added hydrogen ion shifted the equilibrium toward the products so that more CuCl42-(aq)
was createdand the solution changed from blue to green.
Cu(H2O)42+(aq) + 4Cl-(aq) CuCl42-(aq) + 4H2O(l).
The added chloride ion shifted the equilibrium toward the products so that more CuCl42-(aq)
was created and the solution changed from blue to green.
The added chloride ion caused the precipitation of CuCl42-(s), which shifted the equilibrium
toward the products and the solution changed from blue to green.
Cu(H2O)42+(aq) + 4Cl-(aq) CuCl42-(s) + 4H2O(l).
The added hydrogen ion caused the precipitation of CuCl42-(s), which shifted the equilibrium
toward the products and the solution changed from blue to green.
Cu(H2O)42+(aq) + 4Cl-(aq) CuCl42-(s) + 4H2O(l).
Question 5. Describe the change, and explain what occurred when you added the water (in terms
of LeChatelier’s Principle). Choose the best answer.
The added water increased the volume and diluted the concentration of all the dissolved ions,
which caused the reaction to shift toward the reactants.
Cu(H2O)42+(aq) + 4Cl-(aq) CuCl42-(aq) + H2O(l).
The added water increased the volume and diluted the concentration of all the dissolved ions,
which caused the reaction to shift toward the products.
Adding water increased the water concentration, which caused the reaction to shift toward the
products.
Adding water increased the water concentration, which caused the reaction to shift toward the
reactants.

Question 6. Describe the change, copy the equation, and explain what occurred when you added
the sulfuric acid to the potassium chromate solution. Choose the best answer.
The additional hydronium ions caused a shift toward the reactant side, decreasing the
concentration of the dichromate ion and turning the solution to an orange color.
2CrO42-(aq) + 2H3O+(aq) Cr2O72-(aq) + 3H2O(l).
The additional hydronium ions caused a shift toward the product side, increasing the
The additional hydronium ions caused a shift toward the product side, decreasing the
The additional hydronium ions caused a shift toward the reactant side, increasing the
Question 7. Describe the observed change when you added sodium hydroxide to the solution?
Neither Na+ nor OH- ions appear in the chromate-dichromate equilibrium. Why, then, did the
equilibrium shift? Choose the best answer.
The solution changed to orange. The added hydroxide ions caused the change.
The solution changed to yellow. The added sodium ions caused the change.
The solution changed to orange. The added sodium ions caused the change.
The solution changed to yellow. The added hydroxide ions caused the change.
There was no change since neither the Na+(aq) ion nor the OH-(aq) ion appears in the chromate-
dichromate equilibrium.
Question 8. Explain the color changes in terms of Le Chatelier’s principle. Choose the best
answer.
Additional hydroxide ion reacts with the hydronium ion (creating water). The additional water on
the product side caused the equilibrium to shift to the reactants.
The added hydroxide ions decreased the hydronium ion concentration, which shifted the reaction
toward the products.
The added hydroxide ions decreased the hydronium ion concentration, which shifted the reaction
toward the reactants.
There was no shift in the equilibrium since neither the Na+(aq) ion nor the OH-(aq) ion appears
in the chromate-dichromate equilibrium.
Additional hydroxide ion reacts with the hydronium ion (creating water). The additional water on
the product side caused the equilibrium to shift to the products.
Question 9. Describe what you observed when concentrated hyrochloric acid was added to

saturated sodium chloride? Write the equation for the equilibrium, and explain what you
observed in terms of LeChatelier’s Principle. Choose the best answer.
Excess chloride ion from the hydrochloric acid shifted the reaction toward reactants, and the
precipitate NaCl was formed (see equation).
NaCl(s) Na+(aq) + Cl-(aq)
Excess hydrogen ion from the hydrochloric acid increased the acidity of the solution and the
precipitate NaCl was formed (see equation).
Excess hydrogen ion from the hydrochloric acid increased the acidity of the solution and the
precipitate NaCl dissolved (see equation).
Excess hydrogen ion from the hydrochloric acid shifted the reaction toward reactants, and the
precipitate HCl was formed (see equation).
HCl(s) H+(aq) + Cl-(aq)
Excess chloride ion from the hydrochloric acid shifted the reaction toward reactants, and the
precipitate NaCl dissolved (see equation).
Excess hydrogen ion from the hydrochloric acid shifted the reaction toward reactants, and the
precipitate HCl dissolved (see equation).
HCl(s) H+(aq) + Cl-(aq)
Question 10. Describe the effect water had on the mixture. Explain the change properly in terms
of the LeChatelier principle. Choose the best answer.
Additonal water increased the volume and reduced the concentrations of sodium ion and chloride
ions, which shifted the reaction toward reactants.
Additional water caused the sodium chloride precipitate to fall to the bottom of the test tube.
Additonal water increased the volume and reduced the concentrations of sodium and chloride
ions, which shifted the reaction toward products.
Additional water caused an increase in the amount of NaCl(s) in solution, which shifted the
equilibrium to the right, dissolving the solid sodium chloride.
Question 11. The equilibrium equation shows that SbCl3 reacts with water to form insoluble
SbOCl. Why does the solution of antimony(III) chloride have no visible precipitate in it? Choose
the best answer.
There is very little H+(aq) present.
The SbCl3(aq) and HCl(aq) have not yet been added together, so no SbOCl(s) has been created.
A substantial amount of HCl(aq) already exists in the solution, so the equilibrium has shifted
completely to the reactants and all of the SbOCl(s) has dissolved.

The solid SbOCl is present in such a small concentration that it is not visible.
Question 12. Describe what happened when you added water to the solution. Copy the equation,
and explain your observation. Choose the best answer.
The addition of water increases the volume and dilutes all dissolved ions. The reaction shifts to
the side with the greatest moles of solute and solid SbOCl is formed.
SbCl3(aq) + H2O(l) SbOCl(s) + 2 HCl(aq).
the side with the greatest moles of solute and solid SbOCl is consumed.
the side with the fewest moles of solute and solid SbOCl is formed.
the side with the fewest moles of solute and solid SbOCl is consumed.
Question 13. Describe what effect the concentrated hydrochloric acid had? Why? Choose the
best answer.
Adding HCl shifts the equilibrium toward the reactants, which causes solid SbOCl to dissolve.
Adding HCl shifts the equilibrium toward the products, which causes solid SbOCl to form.
Adding HCl increases the concentration of water (a reactant), which causes solid SbOCl to
dissolve.
Adding HCl increases the concentration of water (a reactant), which causes solid SbOCl to form.
Question 14. Write the net-ionic equation for the reaction you observed between barium chloride
and potassium chromate. Indicate the states of all reactants and products. Choose the best
answer.
Ba2+(aq) + CrO42-(aq) BaCrO4(s).
Ba2+(aq) + CrO4-(aq) Ba(CrO4)2(s).
BaCl2(aq) + K2CrO4(aq) BaCrO4(s) + K2Cl2(aq).
BaCl2(aq) + K2CrO4(aq) BaCrO4(s) + 2KCl(aq).
Question 15. Describe what happened when HCl(aq) was added? Record both changes that you
observed. To explain these observations, first tell what effect the addition of HCl(aq) had on the
chromate-dichromate equilibrium (see Step 6). Then explain how that equilibrium shift in turn
affected the barium chromate equilibrium (see Step 14). Write both equations again here as part
of your explanation. Choose the best answer.
2CrO42- + 2H3O+ Cr2O72- + 3H2O(l).

Adding HCl shifted the second reaction to the right decreasing the chromate concentration. This
in turn, caused the first equation to shift to the right and the solid barium chromate to form.
2CrO42- + 2H3O+ Cr2O72- + 3H2O(l).
Adding HCl shifted the second reaction to the left increasing the chromate concentration. This in
turn, caused the first equation to shift to the right and the solid barium chromate to form.
2CrO42- + 2H3O+ Cr2O72- + 3H2O(l).
in turn, caused the first equation to shift to the left and the solid barium chromate to dissolve.
2CrO42- + 2H3O+ Cr2O72- + 3H2O(l).
Adding HCl shifted the second reaction to the left increasing the chromate concentration. This in
turn, caused the first equation to shift to the left and the solid barium chromate to dissolve.
Application of Principles. Question 1. The silver ion, Ag+, forms the colorless diamminesilver(I)
complex ion, Ag(NH3)2+, that is soluble, when it is in an ammonia solution. If ammonia is
added to a solution that contains a AgCl precipitate, the solid dissolves completely. Write a net-
ionic equation for the equilibrium involved. Choose the best answer.
AgCl(s) + NH3(aq) Ag(NH3)2+(aq) + Cl-(aq).
Ag+(aq) + 2NH3(aq) Ag(NH3)2+(aq).
AgCl(s) + 2NH3(aq) Ag(NH3)2+(aq).
AgCl(s) + 2NH3(aq) Ag(NH3)2+(aq) + Cl-(aq).
Application of Principles. Question 2. When concentrated H2SO4 (18M) is added to a saturated
solution of sodium sulfate, a white precipitate is formed. Write a net-ionic equation for the
equilibrium in saturated sodium sulfate, and explain the change in terms of Le Chatelier’s
principle. Choose the best answer.
2Na+(aq) + SO42-(aq) + 2H+(aq) + SO42+(aq) Na2SO4(s).
Excess SO42-(aq) (beyond saturation) from the sulfuric acid causes the reaction to shift to the
right and solid sodium sulfate to form.
2Na+(aq) + SO42-(aq) +H2SO4(aq) Na2SO4(s).
left and solid sodium sulfate to dissolve.
2Na+(aq) + SO42-(aq) Na2SO4(s).
Excess SO42- (beyond saturation) from the sulfuric acid causes the reaction to shift to the right
and solid sodium sulfate to form.
Na+(aq) + SO4-(aq) NaSO4(s).

Na+(aq) + SO4-(aq) NaSO4(s).
2Na+(aq) + SO42-(aq) +H2SO4(aq) Na2SO4(s).
2Na+(aq) + SO42-(aq) Na2SO4(s).
2Na+(aq) + SO42-(aq) + 2H+(aq) + SO42+(aq) Na2SO4(s).
Application of Principles. Question 3. A solution contains the blood-red
hexathiocyanatoferrate(III) complex ion, Fe(SCN)63-, in equilibrium with the iron(III) ion,
Fe3+, and six thiocyanate ions, SCN-. If the solution is diluted with water, will the color deepen,
fade, or stay the same? Why? In addition to predicting whether the solution will deepen, fade, or
stay the same, give TWO reasons for that prediction. One of those reasons will involve Le
Chatelier’s Principle, and one will not. (At least that will be the case if you make the right
prediction!) Choose the best answer.
The color of the solution will fade. 1) The volume will increase, diluting the concentrations of all
ions, and the reaction will shift toward the side with hexathiocyanatoferrate(III) complex ions. 2)
The color will also fade because of dilution.
The color of the solution will deepen. 1) The volume will increase, diluting the concentrations of
all ions, and the reaction will shift toward the side with hexathiocyanatoferrate(III) complex ions.
2) The color will also fade because of dilution.
The color of the solution will deepen. 1) The volume will increase, diluting the concentrations of
all ions, and the reaction will shift toward the side with iron(III) and thiocyante ions. 2) The
color will also fade because of dilution.
The color of the solution will fade. 1) The volume will increase, diluting the concentrations of all
ions, and the reaction will shift toward the side with iron(III) and thiocyante ions. 2) The color
will also fade because of dilution.
The color will stay the same. 1) The reactions does not shift to either side. 2) The concentration
of the hexathiocyanatoferrate(II) complex ion does not change.
F*ck BYUI. Heres the answers to the chem 106 lab abouth le Chatelier's Principle. Hope you

find it helpful
lesshexathiocyanatoferrate(III) and deepening the color.
morehexathiocyanatoferrate(III) and deepening the color.
Solution
Le Chatelier's principle: Any change in one of the variable ( temperature, pressure,
volume,composition, inert gas) that determine the state of the system in equilibrium causes a
shift in the position of the equilibrium in a direction that tends to counteract the change in the
variables under consideration.
1.ans-The additional thiocyantate ion shifted the equilibrium toward the products,
producingmorehexathiocyanatoferrate(III) and deepening the color.
2. ans-M1V1 = M2V2.
(0.1 M)(0.0005 L)=(0.001 M)V2
V2=0.050 L = 50 mL
3. ans-Additional iron(III) ion shifted the equilibrium toward the products to form the red-
colored hexathiocyanatoferrate(III) complex and the intensity of color increased.color.
4. ans-The added chloride ion shifted the equilibrium toward the products so that more CuCl42-
(aq) was created and the solution changed from blue to green.
5. ans-The added water increased the volume and diluted the concentration of all the dissolved
ions, which caused the reaction to shift toward the reactants.

6. ans-The additional hydronium ions caused a shift toward the product side, increasing the
7. ans-The solution changed to yellow. The added hydroxide ions caused the change.
8.ans-The added hydroxide ions decreased the hydronium ion concentration, which shifted the
reaction toward the reactants.
9. ans-Excess chloride ion from the hydrochloric acid shifted the reaction toward reactants, and
the precipitate NaCl was formed (see equation).
10. ans-Additonal water increased the volume and reduced the concentrations of sodium and
chloride ions, which shifted the reaction toward products.
11. ans-A substantial amount of HCl(aq) already exists in the solution, so the equilibrium has
shifted completely to the reactants and all of the SbOCl(s) has dissolved.
12. ans-The addition of water increases the volume and dilutes all dissolved ions. The reaction
shifts to the side with the greatest moles of solute and solid SbOCl is formed.
13. ans-Adding HCl shifts the equilibrium toward the reactants, which causes solid SbOCl to
dissolve.
14. ans-Ba2+(aq) + CrO42-(aq) BaCrO4(s).
15. ans-Ba2+(aq) + CrO42-(aq) BaCrO4(s).
2CrO42- + 2H3O+ Cr2O72- + 3H2O(l).
in turn, caused the first equation to shift to the left and the solid barium chromate to dissolve.
16.1. ans-AgCl(s) + 2NH3(aq) Ag(NH3)2+(aq) + Cl-(aq).
16.2. ans-2Na+(aq) + SO42-(aq) Na2SO4(s).
Excess SO42- (beyond saturation) from the sulfuric acid causes the reaction to shift to the
rightand solid sodium sulfate to form.
16.3. ans-The color of the solution will fade. 1) The volume will increase, diluting the
concentrations of all ions, and the reaction will shift toward the side with iron(III) and thiocyante
ions. 2) The color will also fade because of dilution.

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