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Example: starting fom nitric acid 65 %
For 1 000 mL nitric acid solution 6 N:
- put in a clean conical volumetric flask of 1L, 581,6 mL of the 65 % acid
- add slowly demineralized water to the mark, at 20 0C
- attach the cap of the flask
- stir the flask
- attach a label with HNO3 6 N, the date of preparation, name of the operator
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∙ 10y ago
Sudhakar
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What is the molarity of a solution dissolve 0.31 grams of HNO3 in 300ml of water?
Molarity = moles of solute/Liters of solution ( get moles of HNO3 and 300 ml = 0.300 Liters ) 0.31 grams Nitric acid (1 mole HNO3/63.018 grams) = 0.004919 moles HNO3 Molarity = 0.004919 moles HNO3/0.300 Liters = 0.0164 M HNO3
What is the molarity of a solution prepared by dissolving 0.31g of HNO3 in 300ml of water?
This value is 0,0164 M.
How do you we prepare cresol with soap solution?
cresol is prepared with soap solution as it is more soluble in the soap solution than water . moreover soap solution enhances its detergent and disinfectant properties.
Prepare a working solution from a stock solution?
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
How do you prepare polyethylene glycol solution?
PEG
How many moles of hno3 are needed to prepare 5.0 of a 2.0 m solution of hno3?
10
How do you prepare 1 percent nitric acid solution?
You would dissolve 1 part HNO3 into 99 parts of your solvent.
How do you prepare 6n ammonium hydroxide from 30 percent solution?
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.
What is -6n-2n16?
If you mean: -6n-2n = 16 then -8n = 16 and the solution to the equation is n = -2
How many moles of HNO3 are needed to prepare 5.0 liters of 2.0m soultion of HNO3?
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of SolutionVolume of Solution required = 5.00LWe can say therefore that:Number of Moles of NaOH needed to prepare the solution= Concentration of NaOH * Volume of Solution requiredTherefore:Number of Moles of NaOH needed to prepare the solution= 0.025M * 5.00L= 0.125molesFrom this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
How prepare 6N ammonium hydroxide?
6N ammonium hydroxide (NH4OH) is the same as 6 M NH4OH. The molar mass of NH4OH is 35 g/mole. Dissolve 6 x 35 g = 210 g NH4OH in enough H2O to make 1 liter of solution.
How many milliliters of a stock solution of 11.4 m hno3 would you have to use to prepare 0.500 l of 0.470 m hno3?
500 x .50/1000 x 1/1 x 1000/6.0 = 41.7 = 42 mL HNO3
What is the molarity of a solution dissolve 0.31 grams of HNO3 in 300ml of water?
Molarity = moles of solute/Liters of solution ( get moles of HNO3 and 300 ml = 0.300 Liters ) 0.31 grams Nitric acid (1 mole HNO3/63.018 grams) = 0.004919 moles HNO3 Molarity = 0.004919 moles HNO3/0.300 Liters = 0.0164 M HNO3
What is the concentration of HNO3 in a solution with pH3.4?
1/103.4= 4.0 x 10 -4 M HNO3==============
HNO3 is an example of a mixture or a solution?
Neither, it is a compound.
What is the solution to 6n-4-3 equals 3n plus 10 plus 4n?
6n - 4 - 3 = 3n + 10 + 4n -7 = 7n - 6n + 10 -17 = n
What volume of a 4.0 m stock solution of hno3 is needed to prepare 4.5 l of a 2.5 m hno3 solution?
Applying the equation for a dilution (c1.V1 = c2.V2) gives4.0(mol/L)*V1(L) = 2.5(mol/L)*4.5(L) so V1 = 2.5*4.5/4.0 = 2.813 L = 2.8 litres
