Microscale Techniques Essay

1. NaOH is a very corrosive chemical and contact with it goat cause burns to body tissue and possible eye damage. Can irriate the lungs and can cause permanent lung damage. also contact with water can generate enought heat to ignite combustibles.2. In your own words, briefly explain the terms below. Copied answers go forth receive zero points. a. symmetricalness stateWhen a chemical answer is equal. when the products and reactients are at equal rates b. the effect of organizeation of a decomposablea complex is a term used to describe a substance compused of two other substances.When pushing two substances together they can form a complex which is usually weaker than a regular chemical bond3. A student is studying the equilibrium represented by the equation 2CrO42-(aq, yellow) + 2H3O+(aq) Cr2O72-(aq, orange) + 3H2O(l) The miscellany obtained by the student is yellow.a. Describe the color counterchange the student should observe after adding concentrated hydrochloric acid to t he equilibrium mixture.A) Adding acid causes the mixture to become more than orange. As H3O+ ion concentration increases, the schema converts some of the H3O+ ion to water and dichromate ions. The additional dichromate ion causes the mixture to appear more orange than before.b. Describe the color change the student should observe after adding solid sodium chromate to the equilibrium mixture.(HINT when sodium chromate is dissolved in water, it dissociates into ions.) D) Adding solid sodium chromate causes the mixture to become more orange. As it dissolves, the chromate ion increases and CrO4 -2 ion is converted to dichromate ions. The dichromate ion concentration increases, so the mixture appears more orange.c. Describe the color change the student should observe after adding excess sodium hydroxide to the equilibrium mixture in (b).Briefly explain your answer in terms of Le Chteliers principle, similar to the answers that were provided earlier in this problem.No change the solutio n get out remain yellow. In Le Chteliers principle it talks about how when stress is put on a reaction the reaction transformation to relieve the stress. So when we add more of a reaction or product the reaction will put forward to use it up, and fracture away from added species. d. Write a net ionic equation to support your answer in (c). 1 H3O + (aq) + 1 OH (aq) 2 H2O (l)4. a. forecast the delegacy in which the equilibrium should shift when you add sodium sulfate solution to the mixture in well A1. Explain why.B) The equilibrium will shift to the left. The system wants to lower the concentration of the sulfate ion, which can be done consuming some of the added sulfate ion and thus devious the equilibrium to the reactant side. b. Predict the direction in which the equilibrium should shift when you add solid sodium hydrogen sulfate solution to the mixture in well A3. Explain why.C) The equilibrium will shift to the right. The system wants to lower the concentration of the h ydrogen sulfate ion, which can be done by consuming some of the added hydrogen sulfate ion and shifting the equilibrium to the product side.c. Predict the direction in which the equilibrium should shift when you add concentrated hydrochloric acid to the mixture in well C1. Explain why.A) The equilibrium will shift to the right. The added acid reacts with hydroxide ions to form water, thus reducing the hydroxide ion concentration. The system responds by converting solid magnesium hydroxide to aqueous magnesium hydroxide.d. Predict the direction in which the equilibrium should shift when you add Na4EDTA solution to the mixture in well C2.to the rightExplain why.EDTA purpuse to bind metal cations. So by adding this we reduce the concentration of Mg+2 ions, but we are also adding more OH- ions, and that means that the concentration of OH- ions is decreasing.e. Predict the direction in which the equilibrium should shift when your TA adds water to the hexaaquacobalt(II) ion mixture. Expla in why.D) The equilibrium should shift to the right. The system lowers the concentration of the water by consuming some of the added water to form the hexahydrate complex, thus shifting the equilibrium to the product side.