Question

Fe3+(aq, yello) + SCN-(colerless) ≈[FeSCN]2+(aq,red) A sttudent studying this equilibrium begins with an equilibrium mixture that...

Fe3+(aq, yello) + SCN-(colerless) ≈[FeSCN]2+(aq,red) A sttudent studying this equilibrium begins with an equilibrium mixture that is light pink. 1. what change will the student observe when a solution containing Fe3+ion is added to this mixture? 2.Briefly explain how your answer to (1.) is consistent with Le Chateliers principle.

Homework Answers

Answer #1

Fe3+(aq. yellow) + SCN- (aq, colorless) <-----> [FeSCN]2+ (aq,red)

When a solution containing Fe3+ ion is added to the mixture it will react with SCN- to form [FeSCN]2+, which is red in color.

According to Le Chatelier, the position of equilibrium will move in such a way as to counteract the change. That means that the position of equilibrium will move so that the concentration of Fe3+ ion decreases again - by reacting it with SCN- and turning it into [FeSCN]2+. The position of equilibrium moves to the right.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. When the system Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) is at equilibrium, which one of the...
1. When the system Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) is at equilibrium, which one of the following statements best describes the equilibrium state? a.neither the forward nor the reverse reaction has stopped b. the value of the equilibrium constant is 1 c. the concentrations of Fe3+, SCN-, and FeSCN2+ are always equal at equilibrium d. both the forward and the reverse reaction has stopped 2. Which of the following will change the value of an equilibrium constant? I) varying the...
Suppose that the reaction of Fe3+ and SCN– produces Fe(SCN)2+. 5.00 mL of 2.0 mM Fe3+...
Suppose that the reaction of Fe3+ and SCN– produces Fe(SCN)2+. 5.00 mL of 2.0 mM Fe3+ (aq) is mixed with 5.00 mL of 2.0 mM SCN– (aq). The student finds the equilibrium concentration of Fe(SCN)2+ to be 0.3 mM. 1. Write a balanced chemical equation for this reaction in solution. 2. Write an equilibrium constant expression for the reaction. 3. What is the initial number of moles of each species present? 4. What is the equilibrium number of moles of...
1. A student extended the study of the cobalt ion equilibrium in Part V. When silver...
1. A student extended the study of the cobalt ion equilibrium in Part V. When silver nitrate was added to a test tube containing a blue equilibrium mixture of [CoCl4]2-, a white precipitate formed and the solution turned pink. The student correctly concluded that the white precipitate was silver chloride (AgCl). Explain this result using Le Chatelier’s Principle, and include appropriate chemical reactions to support your explanation.
Chemical Equilibrium: Le Chatelier’s Principle. 1. Add 0.5 mL of 0.1 M FeCl3(aq) to 0.5 mL...
Chemical Equilibrium: Le Chatelier’s Principle. 1. Add 0.5 mL of 0.1 M FeCl3(aq) to 0.5 mL of 0.1 M KSCN(aq), and then add 15 mL of distilled water. To a 2-mL portion of this mixture, add 1 mL of 0.1 M KSCN(aq). Observe any difference in the color from the original solution and explain your observations. Because you are combining equal volumes of equal concentrations, and because they combine in a 1 to 6 mole ratio, Fe3+(aq) should be in...
A student prepared the following two mixtures and recorded their absorbances in a cuvette with a...
A student prepared the following two mixtures and recorded their absorbances in a cuvette with a 1.00 cm path length: Mix # .20 M Fe3 .020 M Fe3 3.25*10^-4M SCN Absorbance 1 10.0 mL -- 10.0 mL .708 2 -- 10.0 mL 10.0 mL .423 1. Write the balanced equilibrium reaction of Fe3 (aq) with SCN (aq) to form [FeSCN]2 (aq). 2. Write the equilibrium formation constant equation for the reaction (Kf expression). Determination of moral absoptivity 3. Assuming that...
Write the net ionic equation for the CrO42 ion/CrO7^2 ion equilibrium. 1) what if any experimental...
Write the net ionic equation for the CrO42 ion/CrO7^2 ion equilibrium. 1) what if any experimental evidence do you have that the equilibrium is affected by the addition of H2SO4 solution. 2)are your observation and explanation in (1) consistent with Le Chatelier's principle.
Tetrachlorocobalt (II) ion reacts with water to form hexaaquacobalt (II) ion according to the following net...
Tetrachlorocobalt (II) ion reacts with water to form hexaaquacobalt (II) ion according to the following net ionic equation: [CoCl4]2-(aq, blue) + 6 H2O(l) <=> [Co(H2O)6]2+(aq, pink) + 4 Cl-(aq) (A) A student doing this experiment placed a test tube containing a blue equilibrium mixture in an ice-water bath. The solution turned pink. When the student removed the test tube from the ice-water bath and placed it in the hot water bath, the solution turned blue. Is the forward reaction exothermic...
± Common-Ion Effect on Solubility for Lead Thiocyanate Lead thiocyanate, Pb(SCN)2, has a Ksp value of...
± Common-Ion Effect on Solubility for Lead Thiocyanate Lead thiocyanate, Pb(SCN)2, has a Ksp value of 2.00×10−5. Part A Calculate the molar solubility of lead thiocyanate in pure water. The molar solubility is the maximum amount of lead thiocyanate the solution can hold. Express your answer with the appropriate units. SubmitHintsMy AnswersGive UpReview Part Common-Ion Effect Consider the dissolution of AB(s) : AB(s)⇌A+(aq)+B−(aq) Le Châtelier's principle tells us that an increase in either [A+] or [B−] will shift this equilibrium...
Re-write the chemical reaction for the equilibrium established between the chromate and dichromate ion. Label the...
Re-write the chemical reaction for the equilibrium established between the chromate and dichromate ion. Label the colors expected for the chromate and dichromate ions. You may refer to the experimental procedure. 2CrO42- (aq) + 2H3O+ (aq) Û Cr2O72- (aq) + 3H2O (l) (chromate-yellow)                   (dichromate-yellow) A completed data table #1. Change to the Reaction Drops Added Visual Observations Shift in the reaction (to products, reactants, or no change) K2CrO4 solution only The color after the change to the reaction is yellow....
I recently performed a lab on Chemical Equilibrium. Here is some background on the experiment: -We...
I recently performed a lab on Chemical Equilibrium. Here is some background on the experiment: -We made a stock solution by combining Fe(NO3)3 and NH4SCN. This made a blood red solution. Then, we added different reagents to see the change of color and the shift of equilibrium. I'm being asked the following question: Based on the color of solutions reported, determine the direction of the reaction's: Fe^3+(aq)+SCN^- --> [FeSCN]^2+(aq) equilibrium shift upon each addition of each reagent investigated and write...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT