The equivalent of potassium dichromate is the molar mass/6: 294,1846/6=49,307666.
For a 0,1 N solution: 49,30766/10 = 4,93076 g
volumetric flask
impossible....u want to use a low contrated solution to dilute into a higher contration solution? No way man,...
5 cubes of sugar and one teaspoon full is needed in the preparation of salt sauger solution (SSS)
Prepare HCl 1 M by HCl concentration 37 % HCl concentration 37 % have density =1.19 g/ml HCl 1 M use HCl 37 % 82.81 ml make volume with water to 1 liter
It's simple to dilute a solution, just add more water. If you have one liter of 6 molar solution, and add another 5 liters of water, it becomes a 1 molar solution. You can also use M1V1 = M2V2 formula for dilution. For example, if you want to prepare 1 M of solution in 1 litre of water, then how much volume you need from the initial 6 M solution? Simply use the equation, (6 M) x (V1) = (1 M) x (1 litre) ---> V1 = (1 M) x (1 litre)/(6 M) = 0.167 L or 167 ml
volumetric flask
it is very easy to prepare working solution from a stock solution we use the formula for this purpose which is: C1V1 = C2V2 C1 is the concentration of the stock solution V1 required volume from the stock solution C2 concentration of the working solution V2 volume of the working solution
Sodium chloride is used to prepare the 0,9 % isotonic solution.
The solute (NaCl) is dissolved in the solvent (water)
To prepare 6 nM ammonium hydroxide a 30 percent solution you need to know the volume of the 30 percent solution that you have and the volume of 6nM solution you would like to make. Then use the following formula: C1V1 = C2V2 where C = concentration in moles/Liter and V = volume in liters.
impossible....u want to use a low contrated solution to dilute into a higher contration solution? No way man,...
When you want to dissolve salt, you use water as the solvent, and salt is therefore the solute.
Denpending of the concentrations, you can use only mechanical agitation and elevate temperature for 5 to 15 minutes.
The volumetric flask is the best.
some liquid volumes are not additive, leading to potentially confusing final solution volumes.
some liquid volumes are not additive, leading to potentially confusing final solution volumes.
use the equation that is standard: 1000 ml 1 M solution= (MOLECULAR WEIGHT) X ml 0.05 M solution = ((MOLECULAR WEIGHT)*X*0.05)/1000