If the reaction is first order, its graphical representation is seen as ln[A] (natural log of concentration) vs. time, and the slope of its like is also the negative rate constant. Finally, for a second order reaction the graph is shown as 1/[A] (inverse of concentration) vs. time, and the slope of its given line is the positive rate constant. By understanding the rate law and finding the value of the correct rate constant with respect to the order of the reaction, one can determine the half-life of the crystal violet. This is because the crystal violet undergoes a decay reaction with the sodium hydroxide. According to Beer's Law, the absorbance of crystal violet is proportional to its concentration.
Ag+ Add drops of HNO3(aq) and test with blue litmus until acidic. The litmus paper turs red. The white precipitate reappears HNO3(aq [Ag(NH3)2]+ (aq) + Cl-(aq) AgCl(s)+2 NH3(aq) 2NH3(aq) +2H3O+(aq) 2NH4+(aq)+2H2O(l) 7. Cu2+ Add NH3 (aq) to the supernatant. Formation of a deep-blue solution NH3(aq) Bi3+(aq)+3NH3(aq)+3H2O(l) Bi(OH)3(s)+3 NH4+(aq) Cu2+(aq)+ 4NH3(aq) [Cu(NH3)4]2+(aq)
Add 2 drops (approximately 0.1 mL) of Blue #1 dye and stir. This will give you a starting concentration of approximately 2.6x10-5 M. c. Calculate and record the concentration of this “starting” solution in
To observe the change in properties of various synthesized copper compounds in order to identify the reactions and products being formed. Secondly, to become familiar with methods of separating compounds through decanting, heating with Bunsen burner and suction filtration system. In doing so, be able to recover copper metal and interpret the resulting percentage yield by applying the law of conservation of matter. Upon combining 20.0mL of NaOH to 10.0mL of Cu(NO3)2 and stirring the solution, there was a darkening of the initial blue color. Adding distilled water to the solution lowers the initial intensity of the blue color, bringing back to a lighter blue.
What color do you observe? NH3 (ammonia, a base) and 1 drop of BTB (bromothymol blue). What color do you observe? Record the colors you expect when BTB reacts with an acid and with a base. HCI and blue dye.
Of the two remaining, one turns slightly yellow, while the other remains blue. What can you assume about the acid/base content of these particular flavors of Vitamin Water? * You could come to the conclusion that the first three will have a balance while the other two do not. The one that turned yellow, would be an acid. The one that stayed blue is a base.
Therefore the alkalinity of water samples is being calculated. In the second approach, the two volume readings for the respective amounts of sulfuric acid used are being determined an indicator based method. Congo red and bromocresol green are being used as the indicators. Procedure (Outline provided as pre-lab): A. The pH meter was calibrated using standard pH solutions provided.
2) Predict which of the following in each set of compounds will have the highest water solubility. Which will have the lowest? Explain your answers. 3) Show how you could separate the components of the following mixtures. a) + O OH 1) dissolve in organic solvent like Et2O or CH2Cl2 2) add water solution of NaOH + O H2O layer O Et2O layer O O 1) add Et2O 2) add HCl OH O H2O layer Et2O layer 1) dry over MgSO4 2) remove Et2O NaCl O OH 1) dry over MgSO4 2) remove Et2O OH O b) O O + N 1) dissolve in organic solvent like Et2O or CH2Cl2 2) add water solution of HCl O O H2O layer + N H Et2O layer O N H O 1) dry over MgSO4 2) remove Et2O O O H2O layer Et2O layer 1) add Et2O 2) add NaOH N NaCl N 1) dry over MgSO4 2) remove Et2O N c) O O + N 1) dissolve in organic solvent like Et2O or CH2Cl2 2) add water solution of HCl O O H2O layer + N H Et2O layer O N H O 1) dry over MgSO4 2) remove Et2O O O H2O layer Et2O layer 1) add Et2O 2) add NaOH N NaCl N 1) dry over MgSO4 2) remove Et2O N d)
Solutions 1,2,3,5 and 7 could not possibly be in unknown I because when Blom thymol is added to unknown I it turn blue but when blom thymol was added to solutions 1,2,3 and 5 turn yellow and solution 7 turn green. 5. For what practical application can Brom thymol blue be used for in the chemistry lab? Brom thymol blue is used in solutions to identify the pH profile of the unknown substance. Solutions with a pH less than 7 are said to be acidic and solutions with a pH greater than 7 are basic.
One progress on TLC called high performance TLC (HPTLC; Sherma and Jain, 2000).HPTLC makes use of gel qualities that are finer, so that thinner plates and smaller. This allows faster separation times and better separation efficiency. HPTLC has improved reduced resolution and detection limits, so that the to walk two dimensions. To phospholipids visible on the TLC plates are used detection reagents. spots corresponding phospholipids may be carbonized by the addition of phosphomolybdic acid, sulfuric acid or copper sulfate in phosphoric acid, and then heating of the sample.