describe two ways for preparing 10 mL of 1 M solution from a 10M stock solution in regards to equipment precision/accuracy. state pros and cons, thank you.

Please don't reject!!

A sodium sulfate solution is measured at 2.2 molal in pure water at a source company. (sodium sulfate molar mass = 142.05 g mol) The lab needs to report the concentration in molarity. What is the final molarity of the sodium sulfate solution? (density of water = 1.0 g mL¯' ; density of the solution = 1.2 g uestion 4 %3D mL-1). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Question 4 of 29> AMoving to another question will save this response. 888. P11 64 F12 eIC " 24 4 & 7\ 3 5 6. 8. %3D dele E R T Y A S D L F G K Z C N alt alt option command command option

A STOCK SOLUTION containing 0.1581 g/L K2CrO4 was prepared.In order to make the CALIBRATION STANDARD, 5 ml of the STOCK was transferredinto a 50ml volumetric flask and then diluted with an appropriate solvent.Calculate:(a) The ppm of K2CrO4 in the CALIBRATION STANDARD.(b) The molarity of K2CrO4 in the CALIBRATION STANDARD. (c) Calculate the molar absorptivity of K2CrO4 (at 371.0 nm). Assume that Beer's Law isobeyed over this concentration range.At 371.0 nm, this CALIBRATION STANDARD in a cell of path length 1.00 cm gave a %T of 59.752.