1. The use of microscale techniques does not change the hazardous nature of the reagents we use. Briefly describe the hazards associated with even small amounts of each of the following:
a. concentrated hydrochloric acid, HCl
HCL may be corrosive. It can cause burns to dosy tissue and can be deadly if inhaled or swallowed. b. sodium hydroxide, NaOH, solution
NaOH is a very corrosive chemical and contact with it can 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 will receive zero…show more content…
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 Châtelier's principle, similar to the answers that were provided earlier in this problem.
No change the solution will remain yellow. In Le Châtelier's 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 equation to support your answer in (c).
1 H3O + (aq) + 1 OH - (aq) → 2 H2O (l)
4. a. Predict the direction 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 shifting 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