why did the addition of water to the equilibrium involving cocl4 -2 cause the color change,...
why did the addition of water to the equilibrium involving cocl4 -2 cause the color change, I.e. shifted the equilibrium toward reactants? you will have to write a reaction quotients for before and after the dilution
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![- When cobalt(II) chloride is dissolved in water, it forms ; complex ion ces mentioned; (ColHol] 2t Reaction taking place; [C](http://img.homeworklib.com/questions/d1a23bb0-7540-11ea-9055-db4a1a844f3a.png?x-oss-process=image/resize,w_560)
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why did the addition of water to the equilibrium
involving cocl4 -2 cause the color change,...
The equilibrium of Co and CF with CoCl- 5 Initial Color: blue Color after addition of...
The equilibrium of Co and CF with CoCl- 5 Initial Color: blue Color after addition of HCI: Piuk bue/Paxle Color after addition of HCI: Color after heating: Pak Color after cooling: Questions Chatelier's Principle to explain the different colors found in the following equilibria. Write balance chemical equations for all chemical reactions. Write net ionic equations for the reaction between Fe(NO3)2(aq) and KSCN(aq) a Explain the color change when Fe(NO3)2 is added to the reaction at equilibrium. b Write net...
Le Chateler's principle In the chart below: • Indicate the color of each solution as darker...
Le
Chateler's principle
In the chart below: • Indicate the color of each solution as darker or lighter than the control after the addition of the specified substance. • Indicate the direction the equilibrium shifted as "toward products" or "toward reactants" based on the color change. • Based on the direction of the shift, indicate the substance(s) that increased which will either be the two reactants present on the reactant side of the equilibrium equation or the complex present on...
Reaction Rates and Chemical Equilibrim 09 In test tube 2, did the equilibrium shift in the direct...
Reaction Rates and Chemical Equilibrim 09 In test tube 2, did the equilibrium shift in the direction of products or reactants? Explain. 010 In test tube 3, what is the evidence that the shift in equilibrium was in the direc- tion of products? 011 In test tube 4, what is the evidence that the shift in equilibrium was in the direc- tion of reactants? C.2 Effect of Temperature Test tube Color Temperature Color is deeper or [FeSCN (increased or lighter...
C. Complex Ion Equilibria 5.Explain the color change that occurred when water was added in Step...
C. Complex Ion Equilibria 5.Explain the color change that occurred when water was added in Step 2 of the procedure. 6.Explain the color change that occurred when the diluted solution was heated. i.How did increasing the temperature affect the value of Kc? ii.What is the sign of ΔH in Reaction 7? Co(H2O)6^2+ (aq) + 4Cl- (aq) <——> CoCl4^2+ (aq) + 6H2O
Determine if the system shifted toward reactants or products for each of the changes. Explain how...
Determine if the system shifted toward reactants or products for each of the changes. Explain how each change affected the equilibrium in terms of Le Châtelier’s principle. For the forward reaction, is the system endothermic or exothermic? Fe+3(aq) + SCN–(aq) ⇋ Fe(SCN)+2(aq) a. The addition of KSCN b. The addition of Fe(NO3)3 c. The addition of NaF (s) d. hot water bath e. ice water bath [CoCl4]–2(alcohol) + 6 H2O(ℓ) ⇋ [Co(H2O)6]+2(aq) + 4 Cl–(aq) a. addition of HCl b....
Adding acetate ion produces a change in the color of the indicator. Watch Video-le where a...
Adding acetate ion produces a change in the color of the indicator. Watch Video-le where a drop of methyl orange is added to each of two 3-mL samples of 0.1 M CH3COOH (acetic acid). The 1 M Na CH3COO (sodium acetate) is added a few drops at a time (with mixing) to one of the samples. The effect on the dissociation of acetic acid that is produced by adding sodium acetate is called the common ion effect. Specify the color...
For each experiment described below 1) provide the relevant equilibrium reaction or reactions, 2) use LeChatelier's...
For each experiment described below 1) provide the relevant equilibrium reaction or reactions, 2) use LeChatelier's Principle to explain why the reaction has shifted left (L) or right (R), and 3) answer any other questions. a) To a solution containing 1M Pb(NO3)2, 1 M HCl is slowly added until a white precipitate forms. The mixture is then heated and the precipitate disappears. Is the dissociation of the precipitate endothermic or exothermic? Does the equilibrium constant (Ksp) change when the solution...
B. Solubility Equilibrium; Finding a Value for Ksp 2. Explain why PbCl 2 did not precipitate...
B. Solubility Equilibrium; Finding a Value for Ksp 2. Explain why PbCl 2 did not precipitate immediately on addition of HCl. What conditions must be met by [Pb2 + ] and [Cl- ] if PbCl 2 is to form? 3. Explain your observations in Steps 3 (The amount of precipitate begins to decrease as it dissolves in the hot water.) and 4 (The precipitate reappears, forming after the test tube was put in ice water.) of the procedure. In which...
» What color did you observe after adding the 3M H2SO, solution? 4) What color did...
» What color did you observe after adding the 3M H2SO, solution? 4) What color did you observe after adding the IM NaOH solution? Assume that the dynamic equilibrium represented in the equation in I is present in the original solution you placed in the test tube. Based on LeChatelier's Principle, as stated above on page one, you will interpret the observations made in 2, above: (Note that H SO, produces H+ in solution.) a) When sulfuric acid was added,...
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) +...
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) + MV (aq) + H* (aq) yellow greenish-blue violet Step 1. Place about 4 mL of distilled water in a regular test tube. Add two drops of methyl violet indicator. Record the color of the solution. Violet Next, add drop by drop, add 6M HCI. This forces equilibrium to be shifted to the left or right-circle the right answer). Adding HCl changes color from to...
The equilibrium of Co and CF with CoCl- 5 Initial Color: blue Color after addition of HCI: Piuk bue/Paxle Color after addition of HCI: Color after heating: Pak Color after cooling: Questions Chatelier's Principle to explain the different colors found in the following equilibria. Write balance chemical equations for all chemical reactions. Write net ionic equations for the reaction between Fe(NO3)2(aq) and KSCN(aq) a Explain the color change when Fe(NO3)2 is added to the reaction at equilibrium. b Write net...
Le
Chateler's principle
In the chart below: • Indicate the color of each solution as darker or lighter than the control after the addition of the specified substance. • Indicate the direction the equilibrium shifted as "toward products" or "toward reactants" based on the color change. • Based on the direction of the shift, indicate the substance(s) that increased which will either be the two reactants present on the reactant side of the equilibrium equation or the complex present on...
Reaction Rates and Chemical Equilibrim 09 In test tube 2, did the equilibrium shift in the direction of products or reactants? Explain. 010 In test tube 3, what is the evidence that the shift in equilibrium was in the direc- tion of products? 011 In test tube 4, what is the evidence that the shift in equilibrium was in the direc- tion of reactants? C.2 Effect of Temperature Test tube Color Temperature Color is deeper or [FeSCN (increased or lighter...
Adding acetate ion produces a change in the color of the indicator. Watch Video-le where a drop of methyl orange is added to each of two 3-mL samples of 0.1 M CH3COOH (acetic acid). The 1 M Na CH3COO (sodium acetate) is added a few drops at a time (with mixing) to one of the samples. The effect on the dissociation of acetic acid that is produced by adding sodium acetate is called the common ion effect. Specify the color...
» What color did you observe after adding the 3M H2SO, solution? 4) What color did you observe after adding the IM NaOH solution? Assume that the dynamic equilibrium represented in the equation in I is present in the original solution you placed in the test tube. Based on LeChatelier's Principle, as stated above on page one, you will interpret the observations made in 2, above: (Note that H SO, produces H+ in solution.) a) When sulfuric acid was added,...
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) + MV (aq) + H* (aq) yellow greenish-blue violet Step 1. Place about 4 mL of distilled water in a regular test tube. Add two drops of methyl violet indicator. Record the color of the solution. Violet Next, add drop by drop, add 6M HCI. This forces equilibrium to be shifted to the left or right-circle the right answer). Adding HCl changes color from to...
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