I could make the corresponding buffer system on the lab bench by adding two salt

Question

I could make the corresponding buffer system on the lab bench by adding two salts to water. The two salts I should choose are: a. Na_3PO_4 and Na_2HPO-4 b. Na_3PO_4 and NaH_2PO_4 c. NaH_2PO_4 and Na_2HPO_4 d. NaH_2PO_4 If the phosphate buffer is adjusted to a pH of 7.4, the addition of lactic acid into blood from exercise would cause the equilibria to shift and thereby the pH back towards the 7.4 to achieve homeostasis. a. Right, lower b. Right, raise c. Left, lower d. Left, raise This dissociation reaction is slightly exothermic. An increase in the body's temperature would cause the equilibrium to shift and thereby the pH. a. Left, lower b. Left, raise c. Right, lower d. Right, raise For questions 8-9 consider the gas phase equilibria of the production of ammonia from hydrogen and nitrogen; 3H_2(g) + N_2(g) 2NH_3(g) If the system were at equilibrium in a container and then the volume of the container was reduced, the system would produce more to the pressure. a. Hydrogen, increase b. Hydrogen, decrease c. ammonia, increase d. Ammonia, decrease Imagine a container of the three gases at equilibrium. The moles of hydrogen in this container are 0.25. Now imagine that I add 0.50 moles of hydrogen and perturb the equilibrium. After the system shifts right to restore the equilibrium, there will be: a. 0.25 moles of hydrogen or less in the container. b. Between 0.25 and 0.75 moles of hydrogen in the container. c. 0.75 moles of hydrogen in the container. d. More than 0.75 moles of hydrogen in the container

Explanation / Answer

5)

mixture should have salt and the corresponding acid

Answer: d

6)

when we add lactic acid pH will decrease, so buffer will shift to left and will raise the pH

Answer: d

7)

increase temperature will favour endothermic reaction

So equilibrium will shift to left which will lower the pH

Answer: a

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