Calculations and Conclusions Write your chemical equations and answers to the qu
ID: 636179 • Letter: C
Question
Calculations and Conclusions Write your chemical equations and answers to the questions in the spaces provided L Studying the lonization of HC,H,0, In Water Equlilibrium 1. Based on the initial solution color, is the HO concentration in the original equilibrium mixture relatively high or relatively low? Briefly explain. 2. What experimental evidence do you have that the equilibrium is affected by the addition of solid NaC,H,O2? What must have happened to the HO concentration to produce this evidence? 3. NaCaHO, is not a component of the HCohO, equilibrium. Explain why the equilibrium is by the addition of solid NaC,HyOp 4. When the equilibrium mixture was heated, did the H,O" concentration increase or decrease? Briefly explain. 5. Based on your answer to Calculation 4, is the forward reaction exothermic or endothermic? Rewrite the equilibrium reaction to include the heat term. ICo(H20 Equilibrium II. Studying the [Cocl (Eq. 2 CoCL12-(aq, blue) + 6 H20() = Co(H2O)?(aq, pink) + 4cr (aq) 6. Use Le Châtelier's principle to account for the color change you observed when you added 12M HC to the equilibrium mixture. z2T
Explanation / Answer
Q.1: Since the color of the solution was initially red, the H3O+ concentration of the original equilibrium mixture was relatively high.
Q.2: The red color of the solution gradually fades to orange upon the addition of solid NaC2H3O2. The H3O+ concentration decreases to produce this evidence.
Q.3: NaC2H3O2 when dissolved in solution produces C2H3O2-(aq) wihch is a product of the HC2H3O2 equilibrium. Hence the equilibrium is affected according to Le-Chatelier's principle and more reactant is formed.
Q.4: When equilibrium was heated, it turms yellow indicating increase in pH. Hence the H3O+ concentration decreases.
Q.5: Since increase in temperature favors backward reaction, the reaction is exothermic.
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