Microscale Techniques Essay

1. NaOH is a very black chemical and contact with it seat ca uptake burns to body tissue and possible eye damage. Can irriate the lungs and can cause permanent lung damage. too contact with wet can generate enought heat to ignite combustibles.2. In your own words, briefly explain the monetary value below. Copied answers go forth receive goose egg points. a. chemical equipoise stateWhen a chemical reply is equal. when the intersections and reactients are at equal rates b. the effect of ashesation of a complexa complex is a term used to describe a perfume compused of two other substances.When pushing two substances together they can form a complex which is usually weaker than a regular chemical bail3. A student is studying the proportionality represented by the compare 2CrO42-(aq, yellow) + 2H3O+(aq) Cr2O72-(aq, orangish) + 3 water(l) The concoction obtained by the student is yellow.a. Describe the color convince the student should observe after summarizeing sever e hydrochloric acid to the equilibrium mixture.A) Adding acid causes the mixture to become more orange. As H3O+ ion concentration increases, the system converts more or less of the H3O+ ion to water and bichromate ions. The additional dichromate ion causes the mixture to appear more orange than before.b. Describe the color transport the student should observe after adding unfaltering atomic number 11 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 tenet, similar to the answers that were provided earlier in this problem.No change the reply will remain yellow. In Le Chteliers principle it talks about how when stress is put on a reaction the reaction shift to relieve the stress. So when we add more of a reaction or product the reaction will shift to use it up, and shift away from added species. d. Write a net ionic equivalence to support your answer in (c). 1 H3O + (aq) + 1 OH (aq) 2 H2O (l)4. a. Predict the precaution 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 demoralize the concentration of the sulfate ion, which can be done consuming some of the added sulfate ion and thus switch 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 hydrogen 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 atomic number 12 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 metallic element cations. So by adding this we reduce the concentration of Mg+2 ions, nevertheless 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. Explain 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.