GC2-7 Studying the effects of changes in conditions on an equilibrium system Lab Report (2)
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G. C 2 - 7 LABORATORY REPORT
Name: Abigail Stark
Lab Partner’s Name: Joshua E.
Z Number:
Lab TA’s Name and Section Number:
Answer the following with details using Le Chatelier’s principle to explain and support
your observations. Include the direction of the reaction shift in all answers.
SYSTEM #1: HC
2
H
3
O
2
(aq)
⮀ H
+
(aq)
+ C
2
H
3
O
2
- (aq)
Answer the following with details using Le Chatelier’s principle to explain and support your
observations. Include the direction of the reaction shift in all answers.
SOLUTIONS
pH
OBSERVATION
0.1M HC
2
H
3
O
2
2
NO CHANGE IN COLOR
0.1M HC
2
H
3
O
2
+ NaC
2
H
3
O
2
5
NO CHANGE IN COLOR
Questions 1.
Did the equilibrium shift and in which direction? When Sodium Acetate was added to Acetic Acid, there was a change in the pH of the solution,
which increased from 2 to 5. This change in pH indicates a shift in the concentration of H+ ions
and a shift in the equilibrium of the solution.
The increase in pH from a highly acidic 2 to a more neutral 5 suggests a decrease in the
concentration of H+ ions. This decrease causes the equilibrium of the solution to shift to the left,
favoring the formation of more reactants.
2.
How did the pH of the solution change after adding NaC
2
H
3
O
2
to it? (Hint: Identify
which ion is being added to the solution and how it affects the concentration of other ions
present in solution)
When Sodium Acetate (NaC2H3O2) was added to the solution, it started to dissociate into Na+
and C2H3O2- ions. As a result, the equilibrium of the solution shifted to the left to decrease the
concentration of the C2H3O2- ion, which subsequently decreased the concentration of H+ ions.
This decrease in H+ ions led to an increase in the pH level of the solution from 2 to 5. The shift
in equilibrium and the subsequent decrease in the concentration of H+ ions contributed to the
solution becoming more neutral, resulting in the observed increase in pH.
SYSTEM #2: 2CrO
4
2-
(aq)
+ 2H
+
(aq)
⮀ Cr
2
O
7
2-
(aq)
+ H
2
O (l)
Answer the following with details using Le Chatelier’s principle to explain and support your
observations. Include the direction of the reaction shift in all answers.
SOLUTIONS
OBSERVATIONS
Na
2
CrO
4
solution
YELLOW
Na
2
CrO
4
solution + HCl
DARK YELLOW/ ORANGE
Na
2
CrO
4
solution + NaOH
GOT LIGHTER AND TURNED TO ORIGINAL COLOR YELLOW
3.
Explain how the equilibrium shifted when you added HCl to the solution? When Hydrochloric Acid (HCl) was added to the Sodium Chromate (Na2CrO4) solution, the
mixture changed to a dark yellow/orange color. This color change occurred because the
equilibrium of the solution shifted to the right upon the addition of HCl, leading to the formation
of the dichromate ion.
4.
Which chromium ion is orange and which is yellow? How did you know?
When the Hydrochloric Acid (HCl) was added to the solution, it introduced the dichromate ion
(Cr2O7^2-), which changed the color of the solution to orange. HCl is an acid, so it shifted the
equilibrium of the solution to the right, favoring the formation of the orange dichromate ion.
The reaction can be represented as:
2 CrO4^2- + 2 HCl → Cr2O7^2- + 2 Cl^- + 2 H2O
Conversely, when Sodium Hydroxide (NaOH) was added to the solution, it introduced the
chromate ion (CrO4^2-), which changed the color of the solution back to yellow. NaOH is a
base, so it shifted the equilibrium of the solution to the left, favoring the formation of the yellow
chromate ion.
The reaction can be represented as:
Cr2O7^2- + 2 NaOH → 2 CrO4^2- + 2 Na^+ + H2O
5.
How did the equilibrium shift when you added NaOH to the solution? (Hint: Think about
what NaOH will react with and how that result will affect the other components present
in the solution.)
When Sodium Hydroxide (NaOH) was added to the Sodium Chromate (Na2CrO4) solution,
the mixture went back to its yellow color. This color change occurred because the equilibrium of
the solution shifted to the left after the addition of NaOH, favoring the formation of the chromate
ion and maintaining the yellow color of the solution. Since NaOH is a base, it shifted the
equilibrium to the left, promoting the presence of the yellow chromate ion in the solution.
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SYSTEM #3:
BiCl
3(aq)
+ H
2
O
(l)
⮀ 2H
+
(aq)
+ BiOCl
(s)
+ 2Cl
-
(aq)
Answer the following with details using Le Chatelier’s principle to explain and support your
observations. Include the direction of the reaction shift in all answers.
SOLUTIONS OBSERVATIONS
BiCl
3
mixed with water
PURE WHITE Mixture plus HCl
TURNED CLEAR
Mixture diluted with water
TURNED WHITE
6.
Explain how the equilibrium shifted when you dissolved the BiCl
3
in excess water.
When Bismuth Chloride (BiCl3) was diluted in water, the solution transformed into a pure
white-colored mixture. This change occurred because the excess water attempted to dissolve
more Bismuth Chloride than originally added, leading to a shift in equilibrium to the right. This
shift in equilibrium was evidenced by the formation of a white precipitate.
As more water was added, the equilibrium shifted towards the formation of a complex with
water molecules, resulting in the white precipitate. This shift in equilibrium and formation of the
precipitate changed the appearance of the solution to a pure white color.
7.
Explain how the equilibrium shifted after the addition of HCl.
When Hydrochloric Acid (HCl) was added to the Bismuth Chloride and water solution, the
mixture became clear. This change occurred because the HCl was added to the product side of
the equilibrium, which counteracted the precipitate formed in the previous step when Bismuth
Chloride was added. This counteraction caused the color change and restored the solution to a
clear state. By adding HCl, the equilibrium shifted to the left, favoring the formation of Bismuth
Chloride (BiCl3) and water (H2O), which are both clear substances. This shift counteracted the
formation of the precipitate, leading to the solution becoming clear again.
8.
Explain how the equilibrium shifted after dilution.
When the mixture was diluted with water again, the solution turned back to a pure white-
colored mixture. This color change was due to an equilibrium shift to the reactant side. Adding
water to the reactant side of the solution was counteracted by the presence of Bismuth Chloride,
leading to the formation of more white precipitate on the product side. This shift in equilibrium
reduced the concentration of reactants and increased the concentration of the white precipitate,
resulting in the solution appearing white again.
SYSTEM #4: [Co(H
2
O)
6
]
2+
(aq)
+ 4Cl
-
(aq) ⮀ [CoCl
4
]
2-
(aq)
+ 6H
2
O
(l)
Answer the following with details using Le Chatelier’s principle to explain and support your
observations. Include the direction of the reaction shift in all answers.
SOLUTIONS
OBSERVATIONS
Dissolved CoCl
2
.6H
2
O
PINK
Solution plus HCl
BLUE
Heated solution
TURNED FROM VIOLET TO BLUE
Cooled solution
TURNED FROM VIOLET TO PINK
9.
According to the equilibrium equation, which ion(s) do you have after the solid was
diluted? Explain how you know the identity of the ion(s) present.
After diluting the CoCl2·6H2O solid, a transformation occurred, yielding [Co(H2O)6]2+ ions.
These ions were identified by observing the solution's color. Upon adding the CoCl2·6H2O
powder to water, the solution transitioned to a shade of pink, confirming the presence of
[Co(H2O)6]2+ ions.
10.
Explain what happened when the HCl was added to the solution.
After adding HCl to the solution, a color change occurred, transforming the mixture into a blue
color. This change is a result of the increased concentration of Cl- ions in the solution. The
addition of HCl introduces more Cl- ions into the solution. According to Le Chatelier's Principle,
the system responds to this increase by shifting the equilibrium to the right, favoring the
formation of more [Co(H2O)6]2+ ions and Cl- ions. This shift leads to the observed color change
to blue, which indicates a higher concentration of [Co(H2O)6]2+ ions in the solution.
11.
Explain what happened when the solution was heated. Was the reaction exothermic or
endothermic?
When the solution was heated in the hot water bath, it underwent an endothermic reaction,
turning into a blue color. This change occurred because the heat energy from the water bath was
absorbed by the solution.
In an endothermic reaction, the reactants absorb heat energy from the surroundings to form
products. This absorption of heat causes the equilibrium of the reaction to shift towards the right,
favoring the formation of more products. In this case, as the solution absorbed heat energy from
the water bath, the equilibrium shifted towards the formation of more [Co(H2O)6]2+ ions,
resulting in the observed blue color.
12.
Explain what happened when the solution was cooled. Was the reaction exothermic or
endothermic?
When the solution was cooled in the ice bath, it changed to a pink color. This color change was
the result of an exothermic reaction, where the heat energy inside the solution was removed.
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In an exothermic reaction, energy is released from the system to the surroundings. In this case,
as the solution released heat energy to the ice bath, the equilibrium of the reaction shifted
towards the left. This shift favored the formation of more reactants, reducing the concentration of
[Co(H2O)6]2+ ions. As a result, the color of the solution changed from violet to pink due to the
decrease in the concentration of [Co(H2O)6]2+ ions, which are responsible for the violet color.
SYSTEM #5:
Fe
3+
+ SCN
-
⮀ [Fe(SCN)]
2+
Answer the following with details using Le Chatelier’s principle to explain and support your
observations. Include the direction of the reaction shift in all answers.
SOLUTIONS OBSERVATIONS
Fe(NO
3
)
3
+ KSCN mixture
DEEP RED
Diluted solution
LIGHTER RED
Heated solution
DARK YELLOW/ORANGE COLOR
Cooled solution
DEEPER RED
Solution + Fe(NO
3
)
3
LIGHTER RED
Solution + KSCN
DEEP RED
Solution + AgNO
3
CLOUDY WHITE
Solution + NaOH
ORANGE
13.
When the beral pipet was placed in the hot water bath, was the reaction endothermic or
exothermic? Explain.
When the beral pipet containing the solution was placed in the hot water bath, an endothermic
reaction occurred. In endothermic reactions, energy is absorbed, which was shown when the
diluted Fe(NO3)3 + KSCN mixture changed from a deep red to a light red color.
The absorption of heat energy caused the equilibrium of the solution to shift to the right. This
shift favored the formation of more product molecules, leading to the color change. The initial
deep red color indicated a higher concentration of product molecules, while the lighter red color
indicated a lower concentration as the equilibrium shifted toward the right.
14.
Explain what is happening when you add more Fe(NO
3
)
3
and KSCN.
When additional Iron Nitrate was added to the diluted solution, there was only a slight change
in the mixture's color, resulting in a slightly lighter red color. However, the change was not
significant. In contrast, when more KSCN was added to the diluted solution, the intensity of the
red color increased, deepening the shade of red.
This change in color intensity was caused by a shift in the equilibrium of the reaction. Upon
adding KSCN to the solution, the equilibrium shifted to the right, favoring the formation of more
product molecules. This increase in product concentration led to the observed deepening of the
red color in the mixture.
15.
Explain what happened after you added AgNO
3
. Hint: Determine the potential products
being formed from adding AgNO
3
to the solution.
After the addition of Silver Nitrate (AgNO3) to the mixture, a significant color change
occurred. Initially, the solution was a deep red color. However, after the AgNO3 was added, the
solution first turned orange and then became a cloudy white/clear mixture.
This color change was caused by the formation of a precipitate, AgSCN, or Silver Thiocyanate.
When AgNO3 was added, the Thiocyanate ion from the Potassium Thiocyanate (KSCN) was
removed by precipitation. This caused the equilibrium of the solution to shift to the left, leading
to a decrease in the concentration of the reactant.
The potential products formed from the addition of AgNO3 to the solution would be
Ag(SCN) and KNO3, making the chemical equation for the reaction KSCN + AgNO3 →
Ag(SCN) + KNO3.
16.
Explain what happened after you added NaOH. Hint: Determine the potential products
being formed from adding NaOH to the solution.
After the addition of Sodium Hydroxide (NaOH) to the mixture, the solution changed to an
orange color. This change occurred because Sodium Hydroxide reacted with Iron Nitrate
(Fe(NO3)3) to form Iron(III) Hydroxide (Fe(OH)3).
This reaction resulted in a decrease in the concentration of Fe3+ ions, causing the
equilibrium to shift to the left. The potential products formed from the addition of NaOH
to the solution would be Fe(OH)3 and Sodium Nitrate (NaNO3), making the chemical
equation for the reaction 3NaOH + Fe(NO3)3 → Fe(OH)3 + 3NaNO3.
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- The equilibrium below is a key step in the ocean acidification process. CO2 (g) + H2O (l) ⇌ H+ (aq) + HCO3− (aq) ΔH < 0 What is the effect of increasing the temperature of this equilibrium? Group of answer choices The pH will increase The [H+] will increase CO2 pressure will decrease No change will be observedarrow_forwardDetermine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. KIO 4- 3. 2+ | 3+ 4+ + 1 3 4 6. 7 8 9 Do (s) (1) (g) (aq) NR OH Reset • x H,O Delete 2 2. 3. 2.arrow_forwardFind the equilibrium concentration of H3O+ starting with 0.072 M solution of acetic acid. Ka = 1.8 x 10-5. Acetic acid is HC2H3O2 (aq).HC2H3O2 (aq) + H2O (l) ⇌ H3O (aq) + C2H3O2- (aq) a) 1.3 x 10-6 b) 1.1 x 10-3 c) 1.5 x 10-2 d) 3.6 x 10-5arrow_forward
- No plagiarism Please! Use the equation of sodium chloride dissolving in water to complete NaCl(s) ⇄ Na+(aq) + Cl–(aq) A student is testing two clear liquids. One liquid is water that has been modified to have a basic pH. The other liquid is a sports drink that contains added electrolytes, including Na+(aq). How can the student use the equilibrium reaction of sodium chloride to determine which liquid is which? In three to five sentences, explain your answer. 17. Which property of spider silk is not shared by Kevlar? A. tensile strength B. shock resistance C. flexibility D. found in naturearrow_forwardit's a chemistry hw needed asaparrow_forwardGiven the equilibrium reactions below and their equilibrium constants. H3O+ (aq) + A (aq) ⇒ HA(aq) + H₂O (1) Kc1 = 2.5 x 104 A™ + H₂O(1) OH- (aq) (aq) + HA(aq) 2.5 x 10-10 What is the value of Kc for the reaction 2 H₂O) H3O+ + OH (aq) (aq) 1.0 x 10¹4 6.3 x 10-6 1.0 x 10-14 none of the answers are correct Kc2 =arrow_forward
- $ 4 The value of K, for hypochlorous acid, HCIO, is 3.50x10-8. Write the equation for the reaction that goes with this equilibrium constant. (Use H3O+ instead of H*.) 000 000 F4 R F Submit Answer % + 5 T G FS Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining A Cengage Learning Cengage Technical Support 6 MacBook Air Y F6 H 87 & + F7 U * 8 F8 9 K >> F9 O 0 F10 P F11 Previous + Next> Save and Ex F12 11arrow_forwardKc for formic acid dissociation in water is 1.8x10-4. What are the equilibrium concentrations of H30+ HCOO- and HCOOH if the initial concentration of HCOOH is .15 mol? HCOOH (aq) +H20 (L) >< H30 (aq) + HCOO (aq)arrow_forwardFe3+(aq) + SCN-(aq) to Fe(SCN)2+(aq). Identify the reactant or product that increases or decreases when HCl is added.arrow_forward
- The concentration of H2S in a saturated aqueous solution at room temperature is approximately 0.1 M. Calculate [H3 O+], [HS−], and [S2−] in the solution:H2 S(aq) + H2 O(l) ⇌ H3 O+(aq) + HS−(aq) Ka1 = 8.9 × 10−8HS−(aq) + H2 O(l) ⇌ H3 O+(aq) + S2−(aq) Ka2 = 1.0 × 10−19arrow_forwardUse the following neutralization reaction to answer the questions: 2HCl(aq) + Ca(OH)2(aq) → CaCl2(aq) + 2H2O(l) Determine the number of moles of HCl needed to perfectly neutralize 0.037 moles of Ca(OH)2. Starting with 0.037 moles of Ca(OH)2, what would be the concentration of CaCl2(aq) if the total volume of the solution is 500.0mL?arrow_forwardNot all of, just number 4arrow_forward
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