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1. Weigh 58,44 g ultrapure NaCl dried at 110 0C for 30 min.
2. Transfer NaCl in a clean 1 L volumetric flask using a funnel. 3. Wash the funnel with 0,9 L demineralized water.
4. Put the flask in a thermostat and maintain 30 min at 20 0C.
5. Add demineralized water up to the mark.
6. Stir vigorously and transfer in a clean bottle with stopper.
7. Add a label with necessary information.
What else can I help you with?
How do you prepare approximately 100 ml of 1.0 m NaCl?
To prepare 100 ml of 1.0 M NaCl solution, you would need to dissolve 5.84 g of NaCl in enough water to reach a final volume of 100 ml. Measure out the required amount of NaCl, add it to a beaker, and then add water while stirring until the final volume reaches 100 ml.
What mass of sodium chloride will be required to prepare 100 cm3 of 0.0282 M of sodium chloride?
The answer is 0,1648 g NaCl.
What final volume would be needed in order to prepare a 0.50 M NaCl solution from 10.0 g of NaCl?
To determine the final volume needed to prepare a 0.50 M NaCl solution from 10.0 g of NaCl, you first need to calculate the number of moles in 10.0 g of NaCl using its molar mass. Then, use the formula C = n/V (concentration = moles/volume) to find the final volume, where n is the number of moles you calculated and C is the desired concentration.
What volume of water should be added to 23.4 g of NaCl to make 100.0 mL of 4.00 M solution?
To prepare a 4.00 M NaCl solution, first calculate the moles of NaCl in 23.4 g. Then, determine the volume of water needed to make a total volume of 100.0 mL minus the volume of NaCl solution. Add the water to the NaCl to make a 100.0 mL solution.
How many ml of 1 M stock solution of Na Cl are needed to prepare 200 ml of a 0.05 M solution?
Molartiy = moles of solute/Liters of solution200 mL X (1 Liter/10^2)= 0.200 Liters0.200 Liters x (0.05 M)= .01 moles of NaOH.01 moles of NaOH x (40 g NaOH/ 1 mole NaOH)= 0.4 g NaOH are required
What is 5 M of NaCl equivalent to?
5 M of NaCl is equivalent to 292,2 grams.
How many ml of 5 M are required to prepare 1000 ml of 0.02 M NaCl solution what is the dilution factor of this solution?
To prepare 1000 ml of 0.02 M NaCl solution, you would need 40 ml of 5 M NaCl solution, which you can calculate using the formula C1V1 = C2V2, where C1 is the concentration of the stock solution, V1 is the volume of the stock solution needed, C2 is the desired concentration, and V2 is the final volume. The dilution factor in this case would be 25, as you are diluting the 5 M solution 25 times to achieve the desired 0.02 M concentration.
What is the total dilution factor from 1.00 M NaCl to 1.00 M NaCl solution?
The concentration is the same !
preparation of 0.1 m of NaCL ML SOLUTION AND ITS LAP REPORT?
A solution of NaCl 1 M.
How would you prepare 400ml of a 0.24M NaCl solution?
We first calculate the amount, in moles, of NaCl that we will need.Amount of NaCl needed = 0.24 x 400/100 = 0.096mol. Mass of NaCl needed = (23.0 + 35.5) x 0.096 = 5.616g So to produce 400ml of 0.24M NaCl solution, accurately add 5.616 grams of NaCl to 400ml of deionised water.
How do you prepare 1 liter of 100ppm NaCl solution?
To prepare a 1 liter of 100ppm NaCl solution, you would dissolve 0.1 grams of NaCl in 1 liter of water. This concentration is achieved by mixing 0.1 grams of NaCl in 1 liter of water.
Calculate the isotonic coefficient for NaCl if a 07M of NaCl solution equaled the hemolysis of14M glucose solution?
i = isotonic molar [glucose] / isotonic molar [NaCl] i = 14 M / 7 M = 2 i = isotonic molar [glucose] / isotonic molar [NaCl] i = 14 M / 7 M = 2 i = isotonic molar [glucose] / isotonic molar [NaCl] i = 14 M / 7 M = 2 i = isotonic molar [glucose] / isotonic molar [NaCl] i = 14 M / 7 M = 2
