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</html>";s:4:"text";s:24930:"This reaction removes Cl- ions from the equilibrium reaction and forms the precipitate, AgCl (s), which could be seen in the wells of row D. Since. Exercise caution around solution and vapors. Predict the effect of adding HCl to the reaction. 2. If spillage does occur, it should be washed with plenty of water and a teacher should be informed. Here K' is the true equilibrium constant which would be for a system in water with a zero concentration of cobalt chloride. Equilibrium and Le Chatelier’s Principle^ PURPOSE To observe systems at equilibrium, and to determine what happens when stresses are applied to such systems. There are three different stresses that pertains to an equilibrium system. How to solve: How does the cobalt chloride equilibrium respond? 10. The addition of water caused the equilibrium to shift to the left. If an inert gas is dded at constant volume, the concentrations and partial pressures of reactants and products do not change. In some of the wells on the well plate, there were black substances on the sides of the plastic and on the bottom. 5. 4. This would form AgCl, which appeared to be in the form of a solid. how many grams of each species will be present at the end when 0.500g of copper is added to 2.500g of AgNO3? The reaction mixture became pink and cloudy and a white precipate settled out leaving a clear, pink solution. Which one, HCl or NaOH, should you add? Changes in temperature also causes a change in the value of Kc or Kp. 7. 1. a) The equilibrium was shifted to the right with the addition of HCl. One way is to add or remove a product or a reactant in a chemical reaction at equilibrium. Calculate the maximum yield of cobalt (II) choloride-6-water and show that cobalt (II) carbonate was in excess. As the poster said above, adding AgNO3 (soluble in water) into the system will cause the equilibrium to shift left. In one test tube, the student added silver nitrate (AgNO3) to a blue equilibrium mixture prepared from CoCl2. GOALS 1 To observe the e ect on equilibrium of adding or removing products and reactants. If an aqueous solution contains both cobalt(II) and chloride ions, the blue ion CoCl 4 2 … The addition of water to the solutions resulted in a light pink color, indifferent from the original purple produced by the HCl and CoCl2 mixture. Some examples of changes in temperature are when the test tube is placed in the almost boiling water and when the test tube is placed in the ice cold water. They form weak bonds to water molecules. Add 25 mL of [Co(H 2 O) 6] +2 to an empty Erlenmeyer flask. In row D, add five drops of AgNO3 solution to each well and stir with the toothpick. Assignment: Use the equilibrium concentrations after each step to determine the K for the above equation. Add a solution of HCl to test tube 1 and with a clean dry stirring rod stir the mixture 4. Let the solution cool for 10 minutes. There would be a greater number of pink wells on the well plate. There would be no change in equilibrium. It is important to remember that when looking at concentration, if a product or reactant contains a solid or liquid, that reactant or product should be omitted. Is the reaction as written endo or exothermic? 10) Shift of equilibrium to the right: add silver nitrate solution dropwise to the blue solution until a precipitate forms. Background: Cobalt(II) does not exist in aqueous solution as a free ion, but forms a complex ion where 6 water molecules, acting That addition of heat would shift the reaction to the right. 9. Given that Keq = 6 x 10^9 for the reaction, it tells the inspectors that the concentration of the products is very high and the concentration of the reactants is low. Safety precautions that must be observed with hydrochloric acid (HCl) is that gloves must be worn when working with hydrochloric acid. We can see as the acetone content increases that the cobalt cations are more likely to react with the chloride anions to form $\ce{CoCl4}$ dianions than they are in the aqueous system. B. The stresses that will be studied in this experiment are changes in the temperature of the system and changes in concentrations of reactants or products. Therefore, equilibrium will shift to the right to remove the stress, increasing the concentration of the products. Why? 3. Safety equipment (googles, latex gloves, and safety aprons) are equipped. Place 5 mL of cobalt solution in a test tube. Follow edited May 2 '17 at 13:50. ggmate. The addition of heats shifts the reaction to the left. Since AgCl (s) is a product, I would expect to have more solid silver chloride rather than silver and chloride ions. Initially, the beaker contains a red-pink solution of cobalt (II) chloride, present as [Co (H 2 O) 6] 2+ ions and chloride ions. In row C, add five drops of distilled water to each well and stir with the toothpick. Now do so in very small incremental steps until the equilibrium has shifted. Equations. According to our table of solubilities (you can easily find this online), Ag+ ions will react with Cl- ions to form SOLID AgCl (Silver chloride) precipitate. Now add liquid H2O to test tube 2 and stir with a stirring rod and record the change of color and equilibrium 7. The ion Co 2+ (aq) is pink. Another example is the, addition of AgNO3, which caused the equilibrium to shift to the left. Place 5 mL of cobalt solution in a test tube. Continue to add the deionized water in 1 mL increments until the white \(\ce{PbCl2}\) solid just dissolves (or disappears). Stress causes the equilibrium system to shift left, right, or not at all. Now add 12 M HCl in 1mL increments until the equilibrium color has changed. Adding AgNO3 to a saturated solution of AgCl increases the concentration of the Ag+ ion thereby increasing the collisions between Ag+ ion and NO 3-ion that results in the formation of more solid AgCl. There is a way to speed up the process of reaching equilibrium. Plastic toothpick is rinsed. The sizes of each drop could vary since there was no exact measurement. A violet-coloured solution should be formed. The shift could be more or less depending on how many greater or fewer drops of which solution was used. This was a minor error but it may have affected the reaction in some ways. Adding an inert gas to an equilibrium system depends on if it is added to constant pressure or volume. C. If NaOH is added, I predict that equilibrium system will shift towards the left because the OH- ions from NaOH will neutralize the H+ ions in the reactants; therefore, the decrease in the H+ concentration will result in a shift to the left. Add a volume of 95% ethyl alcohol (also called ethanol and abbreviated EtOH) approximately When AgNO3 was added to the solutions, it would successfully react with the Cl-. 4. Objective: To gain an understanding of LeChatlier’s principle through the observation of the effect of induced perturbations on the equilibrium distribution of various cobalt(II) complexes. 4. Because AgCl(s) is the product, it is expected that silver chloride will have more in amount. 4.) They are changes in concentration, changes in temperature, and changes in pressure or volume for a gaseous condition. Cobalt Complex Ions continued 3 21 linn cientiic Inc ll ihts esere rium for a reversible chemical reaction is expressed intuitively in LeChâtelier’s Principle: “If the conditions of a system, initially at equilibrium, are changed, the equilibrium will shift in such a direction as to tend to restore the original conditions.” This could also change the intensity of the equilibrium shift. When HCl dissociates, it dissociates into H+ and Cl- ions. The reaction shown in the Introductions was endothermic. Demonstration showing the changing equilibrium of cobalt complexes in solution. Record observations. If H2O is added, I predict that equilibrium system will not be affected because water is a liquid, and pure liquids and solids does not change the concentration, so it does not affect equilibrium. The Le Chatelier's principle states that when an equilibrium system is subjected to a stress, the system responds by attaining a new equilibrium condition that minimizes the imposed stress. 10. Chem 12 silver nitrate + CoCl4 2- The equilibrium that is set up is this, [Co(H 2 O) 6] 2+ (aq) + 4Cl – (aq) ⇌ [CoCl 4] 2-(aq) + 6H 2 O (l). A student doing the experiment extended the study of the 2- ion/2+ ion equilibrium. In one test tube, the student added silver nitrate (AgNO3) to a blue equliibrium mixture prepared from CoCl2.The reaction misture became pink and cloudy, and a white precipitate steeled out leaving a clear , pink solution. 8. The purpose of this lab is to see how different stresses can have an affect on a system at equilibrium. Make the pink cobalt chloride solution up to 100 cm 3 with 60 cm 3 concentrated hydrochloric acid from a measuring cylinder. Addition of water c. Addition of AgNO3 d. Chemistry. and the aqueous solution that is added dropwise is 0.1 M silver nitrate. To the solution in test tube #4, add 0.1 M \(\ce{AgNO3}\) (aq) drop-wise until all the color disappears. Equilibrium and Le Chatelier’s Principle^ PURPOSE To observe systems at equilibrium, and to determine what happens when stresses are applied to such systems. If more drops of CoCl2 were used, then more of the wells would appear pink. AgNO3(aq) <==> Ag+ + NO3-Ag++ Cl – <==> AgCl(s) AgNO3(aq) + Cl – <==> AgCl(s) + NO3-3.) It is the common mode of peroxide self-decomposition: 2 H 2O 2 → 2 H 2O + O 2 (g) Slowly and carefully, add 30 mL (0.48 mol) 16 M HNO 3. A second sample is used as a reference. Decreasing heat would work vice versa. Because it was a solid, the concentration of Cl- is decreased, causing the equilibrium system to shift to the left. One source of error is that when heating the beaker, the water has boiled in many of occasions. If HCl is added, I predict that equilibrium system will shift towards the right because there will be an increase in the concentration of H+ in the reactants. CoCO3 +2HCl = CoCl2 . ... Part 4 - Cobalt(II) Chloride Solution. The addition of HCl caused the equilibrium to shift to the right because when HCl dissociates, it dissociates into H+ and Cl- ions. It is extremely corrosive, so spilling it on skin and on clothing should be avoided. The biggest source of error may have been the fact that the water that was used in this lab was not distilled water. Equilibrium shifts to the left to remove the stress. Cu(s) + 2 AgNO3(aq) --> 2 Ag(s) + Cu(NO3)2 (aq) Because Cl- ions are a reactant, increasing the amount of Cl- ions will cause a stress on the system. There are several ways to stress an equilibrium. The student identified the precipitate as silver chloride, AgCl. 5 drops of AgNO3 were added to row D and were stirred with a toothpick. Note the formation of a pink color. Freezing Point Depression with Antifreeze Lab. Dilute solutions of Fe(NCS)2+ have their equilibrium positions shifted with the addition of Fe(NO3)3, KSCN, NaOH, and AgNO3. Following the mention of the cobalt(II) complex ion system in this post from a couple of days ago, here’s a 30 second video clip of Le Châtelier’s principle in action in the same (with The Smiths).. Decreasing the volume would do the opposite. 3. If more drops of HCl were used, then more of the wells would appear blue. This blue solution shifts back to pink as the AgNO3 is added. Because it was a solid, the concentration of Cl- is decreased, causing the equilibrium system to shift to the left. 5 mL of the cobalt solution were placed in a test tube, and HCl was added until the color of the solution was halfway between pink and blue. Record observations. To another sample of the equilibrium mixture add, with stirring, several drops of 6 M NaOH until you observe the formation of solid reddish precipitate. Did the solution change color as you predicted? When hydrochloric acid is added, the added chloride ions shift the equilibrium position in favour of blue [CoCl 4] 2-ions and water. Add about 1 mL of deionized water to the large test tube containing the \(\ce{PbCl2}\) solid. BACKGROUND INFORMATION The element cobalt can form compounds in two different oxidation states, +2 and +3.The +2 state is more common. This indicates a left shift in the reaction. pure liquids and solids does not change the concentration, it does not affect equilibrium. AgNO3is added to produce Co(H2O)62+again. If heat is a product, this shows that the reaction is exothermic. These shifts indicates that the reaction is indeed endothermic. Equilibrium Cr 2O7 2-to CrO 4 2-Similar to the above demonstration, color changes are observed upon either addition of NaOH to K 2Cr 2O7 (orange to yellow) or the addition of HCl to K2CrO 4 (yellow to orange). When talking about heat, it is important to know that the heat is affecting the whole reaction, not just one side. 6. When AgNO3 was added to the solutions, it would successfully react with the Cl-. Other compounds of cobalt(II), which include both anhydrous Co 2+ and complex ions, are commonly blue.. Therefore, equilibrium will shift to the right to remove the stress, increasing the concentration of the products. A. I. Cobalt system (/25) Chemical Equation: CoCl 4-2 {blue} + 6 H 2 O Co(H 2 O) 6 +2 {red} + 4 Cl-+ heat System at equilibrium: Purple System at equilibrium: Exothermic Stress Applied Observation Chemical Explanation Heat applied to the system System turns darker blue … asked May 2 '17 at 4:47. Record observations. This is because solid and liquid does not affect a concentration. Instead, tap water was used. If you add AgNO3, which will remove Cl− ions from the solution, the equilibrium will shift to the left and the color will be pink again. The record the results. HCl is added to a third sample at room temperature. The increase in the concentration of reactants or the decrease in the concentration of products would lead to the equilibrium shifting towards the right. Be sure to include appropriate dilution factors (as they will not cancel). The attachment of A chemical system at equilibrium can be temporarily shifted out of equilibrium by adding or removing one or more of the reactants or products. Take test tube number 1 again, to the mixture add AgNO3 and stir with a clean stirring rod and record the results. 6. Because Cl- ions are a reactant, increasing the amount of Cl- ions will cause a stress on the system. It is important to know that catalysts do not change the equilibrium point. 3. In this case, the reaction would shift to the side with more moles. Add five drops of AgNO3 solution to each well in row D and stir thoroughly with the toothpick. Observations: When the solution is heated to boiling, it turns from pink to blue. Adding AgNO3 to the solution will ppt AgCl, removing Cl^- from the left side of the equation and shifting the equilibrium to the left. 1. equilibrium. Keq = [products] / [reactants]. 5. Addition of HCl b. D. The Equilibrium in a Saturated NaCl Solution Page 152 and Page 159. Likewise, if the drops of CoCl2 were small and the drops of HCl were large, then the solutions in the wells would appear to be more blue than normal. Some examples of changes in concentrations of reactants or products are the addition of HCl and the addition of distilled water, respectively. A shift to the left causes a decrease in temperature and a shift to the right causes a increase in temperature. Predict the effect of adding HCl to the reaction. CoCl2 at room temperature: purple (between blue and pink). With the addition of NaCl, there would be an increase in Cl- ions due to NaCl separating into ions, adding to the amount of Cl- ions. This would form AgCl, which appeared to be in the form of a solid. After discarding the toothpick, the colors of the solutions were recorded. Equilibrium shifts toe the side with more moles. 9. +50 kJ/mol + Co(H2O)6^2+ + 4Cl- <--> CoCl4^2- + 6H2O. The equilibrium that is set up is this, [Co(H 2 O) 6] 2+ (aq) + 4Cl – (aq) ⇌ [CoCl 4] 2-(aq) + 6H 2 O (l). 1. 8. THE COBALT CHLORIDE EQUILIBRIUM. The concentrations of both reactants and products then undergo additional changes to return the system to equilibrium. … he addition of HCl, which caused the equilibrium to shift to the right. When trying to determine what side the equilibrium shifts to,increasing temperature or decreasing temperature can be thought of as adding or subtracting "heat". According to Le Chatelier’s principle, it is a shift in equilibrium from right to … The complex is formed according to the reaction: The addition of HCl to a mixture/solution of HCl and CoCl2 creates a dark blue color inside of the wells, indicating the reaction to shift towards the right. 3. AgNO3(aq) <==> Ag+ + NO3-Ag++ Cl – <==> AgCl(s) AgNO3(aq) + Cl – <==> AgCl(s) + NO3-3.) Observations was recorded. AgNO3 removes Cl- ions from the equilibrium reaction and forms the precipitate, AgCl (s), which could be seen in the wells of row D. Since. When hydrochloric acid is added, the added chloride ions shift the equilibrium position in favour of blue [CoCl 4] 2-ions and water. Because the equilibrium constant is affected. The name given to compounds such as solid cobalt(II) chloride, CoCl2 * 6H2O, which have water as a part of their crystal structure is a hydrate. 1.) The formal statement is called Le Chatelier’s principle: If an equilibrium is stressed, then the reaction shifts to reduce the stress. AgNO3(aq) Ag+ + NO: Ag++ Cl -> AgCl(s) AgNO3(aq) + Cl > AgCl(s) + NO3- Note by the above equation how Age scavenges free chloride ions by tying them up in a precipitate, and thus removes them from the solution. The decrease in the concentration of reactants or the increase in the concentration of products will cause a shift to the left. 8. Make note of the color of the solution left behind. Discussion: While the nature of the species in solution during the cobalt Hazards 6M HCl is very corrosive! Always make sure to add acid to less concentrated solutions, rather than adding less concentrated solutions to My guess is that adding water does affect equilibrium for a reaction with different number of moles on each side. The addition of AgNO3 gave out a precipitate, causing the concentration of the reactants to decrease, shifting the reaction to the left. This would increase the concentration in Cl-, causing the forward rate of reaction to increase in order to obtain equilibrium. We can see as the acetone content increases that the cobalt cations are more likely to react with the chloride anions to form $\ce{CoCl4}$ dianions than they are in the aqueous system. Dissolve a small amount of solid CoCl 2 • 6 H 2 O in a beaker containing ethanol. If heat is a reactant, it shows that the reaction is endothermic. 10. 2. chem please help. Following the mention of the cobalt(II) complex ion system in this post from a couple of days ago, here’s a 30 second video clip of Le Châtelier’s principle in action in the same (with The Smiths).. In what direction was the equilibrium shifted by: a. This lab really helped my understanding of Le Chatelier's Principle. Left or Right The reaction would shift left when a reverse reaction is favored. This would have changed the intensity of the equilibrium shift, either left or right depending on what particles the water contained. Improve this question. Also, the number of drops were not exact. Is this right? This could have also changed the intensity of the equilibrium shift. Silver Chloride should be expected to be more present . In the procedures, it measures the amounts of solutions in each well in "drops." To another sample of the equilibrium mixture, add 10 drops of 0.1 M AgNO3. … GOALS 1 To observe the e ect on equilibrium of adding or removing products and reactants. Adding a more hydrochloric acid will produce a blue solution containing mainly [CoCl 4] 2–, while adding water will restore the pink colour. Chemical equilibrium in cobalt complexes Some ionic compounds exist as hydrates. 4.) If inert gas is added at constant external pressure, then volume increases to accommodate the added gas, thereby decreasing overall pressure. Create your own unique website with customizable templates. 9. Therefore, equilibrium will shift to the right to remove the stress, increasing the concentration of the products. Since time was of the essence, our lab group decided to count out roughly the number of drops that were in the directions. In the reaction AgNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq) + heat, when 0.70 mole of AgNO3 and 0.70 mole of HCl react, the temperature of 50 g of water increases from 15°C to 30°C. Record and changes in color and formation of precipitates in the Data Table. and the aqueous solution that is added dropwise is 0.1 M silver nitrate. Is the reaction as written endo or exothermic? Keq = (CoCl4^-)/(CoH2O)6^+2 + (Cl^-)^4 DrBob222 Here K' is the true equilibrium constant which would be for a system in water with a zero concentration of cobalt chloride. Adding or removing a pure solid or liquid does not change the concentration, so it does not affect the equilibrium. In Parts A and B above, we considered equilibrium systems that were based on true chemical reactions. Demonstration 3: Equilibrium with Cobalt Complex Ions [Co(H 2 O) 6] 2+(aq) + 4 Cl−(aq) → *CoCl 4] 2− + 6 H 2 O H = + 50 kJ/mol pink blue 1. Now do so in very small incremental steps until the equilibrium has shifted. Keq = 6 x 10^9 for the reaction Ag+ (aq) + Cl- (aq) <--> AgCl (s). For example, if the drops of CoCl2 were large and the drops of HCl were small, then the solutions in the wells would appear to be more pink than normal. Demonstration showing the changing equilibrium of cobalt complexes in solution. The Le Chatelier's principle is when an equilibrium system is subjected to a stress, the system responds by attaining a new equilibrium condition that minimizes the imposed stress. When that solution is added into the ice bath, it turned to pink, indicating a shift to the left. Because the water was not pure and contained particles, water may have had an active role in the reaction. My lab partners forgot to wash the well plate; therefore, the black substances could have partook in the reaction, which would have altered the equilibrium shift. Co(H2O)6^2+ + 4Cl- + 50 kj/mol ←→ CoCl4^2- + 6H2O. Equilibrium System: Observations upon addition of \(\ce{HCl}\): In which direction did this stress cause the equilibrium system to shift? Equilibrium Response Observations Reaction Response Color Observation Purple Color Test Tube 1 - Control Choose Choose... Test Tube 2 - Add HCl(aq) Blue Color Choose Choose.. Question: (9pts) Part II: Cobalt Chloride Reaction (CoCl] (alc) + 6H2O(alc) = Deep Blue Co(H,0)]2+ (alc) + 4C1 (ale) Rose Pink Table View List View Table 2. 7. Part 2. 1. This precipitate is Fe(OH), (s). The addition of AgNO3 caused the equilibrium to shift to the left because AgNO3 (aq) + Cl- (aq) <--> AgCl (s) + NO3^-1 (aq). Add either HCl (6 M) or NaOH (6 M) to the solution dropwise to change the color of the solution. 9. Add just enough HCl to … There would be a greater number of blue wells on the well plate. We omitted this part of the experiment! The minerals in the tap water may have reacted in the reaction, affecting the severity of the equilibrium shift. Another source of error is the inconsistency in size of drops. 6H2O)++ ion in aquaous solution without adding any other chemical. clear yellow with red precipitate 9. The reaction would shift right when a forward reaction is favored. Increase in the volume of a container decreases pressure. Tap water was used, but it bubbled much more than normal and took quite a while for the bubbles to disappear. Share. 3 AgNO3 + CoCl3 ----> 3 AgCl + Co(NO3)3. i am not sure the what the charge on cobalt is, since it has multiple charges, but i assume that it has the … he mixture is stirred with a plastic toothpick. relatively little unreacted cobalt(II) remains. The water used in this experiment was far from distilled water. Stir the mixture and observe what happens. On your data sheet record the volume of water needed to dissolve the solid. This was determined after increasing the solution of CoCl2 and HCl at equilibrium. 2 To predict the direction in which the equilibrium shifts upon a change in concentration of one 2 To predict the direction in which the equilibrium shifts upon a change in concentration of one In row C, add five drops of distilled water to each well and stir with the toothpick. 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