Guided Virtual Lab Activity: The Complex Nickel Salt Procedure Data & Observations D Accurately weigh approximately 0.05 g of salt A or B and quantitatively transfer it into an Erlenmeyer flask. Salt A was analyzed. It was a pale blue powder, 0.0513 g Salt A 2) Add 10.00 mL of standardized 0.2 M HCI (aq) and 2-3 drops of Bromocresol green indicator to the flask. The solution should be yellow at this point. HCI is clear, colorless. [HCI]-0.2108 M Used volumetric pipet to transfer the HCI The salt dissolved in the HCI, and the resulting solution was an extremely pale green-hlue color. Solution turns yellow when indicator is added. 3) Slowly titrate the solution with standardized 0.1 M NaOH (ag) until you observe the first permanent color change. (You are forming a new complex cation in the titration, which requires a little time - slower titrations tend to give better results on this experiment.) NaOH is clear and colorless. [NaOH] =0.1008 M Trial Endpoint Initial Volume NAOH 2.61 ml 20.78 ml 0.33 ml Final Volume NAOH Observations Pale green 20.78 ml. 39.16 ml. Pale green-blu 18.56 mL Pale green 4) Repeat steps 1-3 until you have 3 good trials. Mass of salt A used in trial 2 = 0.0489 g Mass of salt A used in trial 3 - 0.0508 Titration data is in data table above. Assume someone performed this experiment on the salt you synthesized. Use this data to calculate the percent by mass of en in the synthesized salt.