1. An unknown solid was added to a formic acid solution, which increased the pH of the solution. Is the unknown substance NaNO3 or NaCHO2? Explain how you arrived at your decision. Formic acid is a weak acid with a molecular formula of HCHO2. In aqueous solution it is in equilibrium with its dissociated and undissociated forms:

HCHO2(aq) â H+(aq) + CHO2â(aq)

2. Consider the conceptual reaction of â¦. A â 2B

The forward reaction is endothermic. A is a blue substance, and B is a yellow substance. Together they make a green mixture. If this equilibrium mixture is heated up in a water bath, how will the color of the mixture change? Explain how you determined this.

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Lelia LubowitzLv2

13 Dec 2019

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#1-2 please

Adding a component common to a system at equilibrium will cause the equilibrium to shift opposite to the sid of the added stress. Removing a component from a system at equilibrium will cause the equilibrium to shift to the same side as th stress. For an Exothermic Reaction A + B â C + Heat A. Adding heat will cause the equilibrium to shift left B. Removing heat will cause the equilibrium to shift right. For an Endothermic Reaction Heat + A + B â C A. Adding heat will cause the equilibrium to shift right B. Removing heat will cause the equilibrium to shift left Given the following equilibrium system, what will be the affect of adding the following components? To detect the affect of the stress the following indicator was used Bromcresol reen Acid Color(yellow) Base Color(blue) PART A: Study of the Weak-Acid Equilibrium: green NH4+(aq) H2O() Â± + Blue B NHj(aq) CB Yellow H,0+(aq) CA - + A When adding ammonium chloride solution, the color of the equilibrium mixture changed from Green â Yellow 1. The color change indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? a. (L) left (R) right b. Explain your answer to question 1a. You should indicate which ion was added to or removed from the equilibrium mixture. When adding hydrochloric acid solution, the color of the equilibrium mixture changed from Green â Blue 2. The color change indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? a. (L) left (R) right Explain your answer to question 2a. You should indicate which ion was added to or removed from the equilibrium mixture b. When adding sodium hydroxide solution, the color of the equilibrium mixture changed from Green â Yellow 3. The color change indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? Explain your answer to question 3a. You should indicate which ion was added to or removed from the equilibrium mixture. a. (L) left (R) right b.

Tetrachlorocobalt (II) ion reacts with water to form hexaaquacobalt (II) ion according to the following net ionic equation:
[CoCl₄]²^-(aq, blue) + 6 H₂O(l) <=> [Co(H₂O)₆]²⁺(aq, pink) + 4 Cl^-(aq)

(A) A student doing this experiment placed a test tube containing a blue equilibrium mixture in an ice-water bath. The solution turned pink. When the student removed the test tube from the ice-water bath and placed it in the hot water bath, the solution turned blue. Is the forward reaction exothermic or endothermic? Give complete explanation.

(B) What change do you observe when you add concentrated hydrochloric acid, HCl, solution. HCl undergoes dissociation according the following equation: Give complete explanation.

HCl(aq) â H⁺(aq) + Cl^-(aq)

(C) What experimental evidence do you have that the equilibrium is affected by the addition of water. Give complete explanation.

Any help/explanations with this Le Chatelier's Principle lab would be extremely helpful. I attemtped to do question A, but I'm not exactly sure if my answer is interpreted correctly. I have included the actual lab procedure with the 5 questions. Thank you again.