2. A stock standard solution of copper (1000.0 ppm) is available. How would you prepare 50.00 mL each of a series of standards that have analyte ppm concentrations of 1.00, 2.00, 3.00, 4.00 and 5.00 ppm? Create a table and show all calculations. C₁V₁= C₂V₂

A 57.0 mL aliquot of a 0.500 M stock solution must be diluted to 0.100 M. Assuming the volumes are additive, how much water should be added? volume of water: 4 R V % 5 T 20 F5 B ^ 6 MacBook Air H & 7 N F7 * 00 8 M DII FB ( 9 K F9 O ) O F10 P F11 + mL F12 81

A student performed three H2SO4 titrations in Part 2 using their 0.1276 M NaOH solution which they previously standardized in Part 1. They reported the following measurements:   Determination #1 Determination #2 Determination #3 Final NaOH Burette Reading 20.72 mL 41.54 mL 21.59 mL Initial NaOH Burette Reading 0.12 mL 20.72 mL 0.83 mL What was the total number of moles of H2SO4 in their second titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).

A student measured the mass of an empty micropicnometer to be 2.000g. A student places 0.500mL of citric acid solution into a micropicnometer. The student reweighed the micropicnometer and found the mass of the citric acid solution and micropicnometer to be 2.525g.    A student titrates 0.101mL of citric acid solution using the standardized 0.1M solution (use the exact concentration calculated from the previous titration problem). The sample required 0.819mL of NaOH solution to reach the end point.   Given the following chemical equation.   NaOH   +  H3C6H5O7 →  Na+ +   H2O  +   C6H5O73-   Given the above information. Calculate the mass of citric acid in the 0.101mL citric acid solution.    Given the above information. Calculate the total mass of the 0.101mL citric acid solution.