Page 1 of 1
1. Weigh 2.0-2.5 g of NiCl2-6H20 accurately into a clean 100 mL beaker. 2. Dissolve in about 25 mL of 0.5 M H2SO4 and tr
Posted: Wed May 18, 2022 12:33 pm
by answerhappygod
- 1 Weigh 2 0 2 5 G Of Nicl2 6h20 Accurately Into A Clean 100 Ml Beaker 2 Dissolve In About 25 Ml Of 0 5 M H2so4 And Tr 1 (42.12 KiB) Viewed 49 times
- 1 Weigh 2 0 2 5 G Of Nicl2 6h20 Accurately Into A Clean 100 Ml Beaker 2 Dissolve In About 25 Ml Of 0 5 M H2so4 And Tr 2 (8.63 KiB) Viewed 49 times
1. Weigh 2.0-2.5 g of NiCl2-6H20 accurately into a clean 100 mL beaker. 2. Dissolve in about 25 mL of 0.5 M H2SO4 and transfer the solution quantitatively, rinsing with distilled water, into a 100 mL volumetric flask. Dilute to volume with distilled water and mix thoroughly. This is the stock solution. 3. Prepare dilutions of 20.00 mL, 10.00 mL, and 5.00 mL of stock solution into 25 mL volumetric flasks. Use distilled water to dilute to volume and mix the solutions thoroughly. You now have four standard solutions, including the stock solution, for which to obtain the absorbance readings which you will then use to construct your Beer's Law plot. CALCULATE THE CONCENTRATION FOR EACH OF YOUR FOUR STANDARD SOLUTIONS IN mg of Ni2+/mL OF SOLUTION.
Determine the concentration in mg Ni2+/mL for the 20.00 mL dilution if the mass of nickel chloride hexahydrate=2.2619 g.