You need 58,44 mg of ultrapure NaCl; dissolve in demineralized water, at 20 0C, in a thermostat, using a class A volumetric flask of 1 L.
A 0.0% NaCl solution is a solution with absolutely no NaCl.
The concentration of NaCl in a solution that contains 0.9 NaCl is 0.9 grams of NaCl per 100 grams of solution.
If 10 is 10 molar for you, this is a saturated solution of NaCl.
To determine the amount of NaCl in the solution, you first need to calculate the moles of NaCl present. Using the given molarity (2.48 M) and the volume of the solution (assumed to be 806 g = 806 ml for water), you can find the moles of NaCl. Then, you convert the moles of NaCl to grams using the molar mass of NaCl (58.44 g/mol) to find the amount of NaCl in the solution.
In order to determine this, it is necessary to know what solution we are looking at. One we know that we can look at the grams in a mole of the substance and determine the percentages based on molecular weight.
Pure solide NaCl is not electrically conductive. The water solution of NaCl is an electrolyte and is conductive.
Sodium chloride is a salt; the water solution is neutral.
0,4 mol NaCl is 23,376 g.2,85 mol NaCl is 166,554 g to 1L.140 mL solution NaCl 2,85 M contain 0,4 mol NaCl.
Because the sodium chloride solution in this case is isotonic.
Yes, because the solution of NaCl is an electrolyte.
It depends on the final solution Volume you want to prepare. For 100ml of a 6M NaCL solution, you add 35.1g of NaCl to water until you reach 100ml. Dissolve and autoclave for 15 mins.
To determine this, you need the concentration of the NaCl solution. Once you have that, you can use the stoichiometry of the reaction between AgNO3 and NaCl to calculate the volume of 0.117 M AgNO3 needed. The balanced chemical equation for this reaction is: AgNO3 + NaCl → AgCl + NaNO3.