CHEM 1B Lecture Notes - Lecture 7: Methyl Orange, Phenolphthalein, Sodium Hydroxide

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pucesquirrel907

12 Apr 2020

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UCSB

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Chemistry and Biochemistry

Course

CHEM 1B

Professor

Kunkel

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CHEM 1B Full Course Notes

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Experiment 7: le ch telier"s principle and chemical equilibrium. The purpose of this experiment was to observe reaction reversibility and equilibrium by changing the concentration of certain reactants and products to force a shift in equilibrium. First, a methyl orange indicator was used to observe the changes in equilibrium by monitoring shifts in color. When 6 m hydrochloric acid (hcl) was added, the color of the solution changed from yellow to red, indicating that the equilibrium shifted left. This occurred due to the increase in h+ ions with the addition of aqueous hcl. Contrastingly, when 6 m sodium hydroxide (naoh) was added to the same test tube, the solution changed from red back to yellow, indicating a rightward shift in equilibrium. This change occurred due to the decrease of h+ ions, caused by the oh- ions from. Next, the same process was repeated for a 0. 1% phenolphthalein indicator with the same chemical formula as shown above.

Related Questions

Hi, can someone help me answer these questions? I promise to rate you!!

1. In Le Chatlier's principle, can you describe the reaction between Fe+3 and SCN- with Fe(SCN)+2. The reaction turned reddish brown when Fe+3 and SCN- were mixed together. Where does the equilibrium shift?

2. In Le Chatlier's principle, can you describe the reaction when 0.1 M Ni(NO3)2 and 6 M of NH3 are mixed together. The color changed from light blue to dark blue. After that we added 6 M HCl, the color changed again to a lighter color. Where does the equilibrium shift?

3. In Le Chatlier's prinicple, can you describe the precipitation that occured when NaOH and Ca(NO3)2 were mixed together? Also, after being centrifuged, the solution and the precipitation solid (white) separated. We threw out the liquid and added HCl and NaOH. Where does the equilibrium shift?

4. In Le Chatlier's prinicple, can you describe the reaction that occured when 5 drops of 0.1 M Co(NO3) is added mixed with 5 drops of concentrated HCl. The color changed into pink. When we added water, the color changed into light pink. Then when we boiled it, it turned blue. After cooling, it turned pink again. Where does the equilibrium shift?

5. We took two test tubes, marking one ACID and one is BASE. We added 3 mL of H2O in each. We added 6 drops of 6 M HCl to the acid tubes and a drop of NaOH to the base tube. Then we added 4 drops of the indicator on each (methyl orange- indicator). The acid tube turned into color pink after the indicator and NaOH again was added. The base tube turned yellow after the indicator and HCl solution is added. In Le, Chatlier's principle, can you describe this whole reaction? Where does the equilibrium shifts?

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Use Le Chatelier's principle to explain the different colors found in the following equilibiria. Show all chemical reactions.Ni 2+, NH3 and Ni(NH3)6 2+Methyl orangeFor our Ni2+ experiment the color started light green/blue, then when added NH3 turned purple/blue, then after adding HCl turned back to light green/blueFor our Methyl orange experiment the solution turned red after adding HCl, turned orange after adding NaOH and turned back to red when added HCl

#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.

CHEM 1B Lecture Notes - Lecture 7: Methyl Orange, Phenolphthalein, Sodium Hydroxide

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