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How To Prep 10 Nitric Acid The best method to organize food shortages, which is why you will have food stored up and wont have any need to be out fighting the crazed Black Friday Shoppers for that last can of soup on the shelf, is to start filling your pantry at this moment. How To Prep 10 Nitric Acid These diets are also very easy cooking.
To solve this problem, we basically have 2 equations and 2unknowns. The unknowns are the (volume of water) & the (volumeof 70 wt%) nitric acid to add.
* This problem will assume that you are interested in making 1 L(or 1000 mL) of 5 wt% nitric acid solution.
Equation 1: (volume of water) + (volume of 70 wt% nitric acid) =1000 mL
Equation 2: mass of nitric acid / [mass of water + mass of 70wt% nitric acid solution] = 0.05 (0.05 is 5 wt%)
* Remember that mass = density * volume
* Remember that 70 wt% nitric acid solution mean that for 100grams (gm) of this acid, then there's 70 grams of HNO3
* Remember that density of 70 wt% nitric acid solution is 1.413gm/cm^3
* Remember that density of water is 1 gm/cm^3
Equation 2 is now re-written as: [(density of 70 wt% nitric acidsoln)*(volume of 70 wt% nitric acid)*0.70] / [(volumewater)*(1gm*cm^3) + (volume of 70 wt% nitric acid)*(1.413gm/cm^3)]= 0.05
Solving for the 2 equations gives answer to the 2 unknowns:
Answer: To make 1000 mL of 5 wt% nitric acid solution, add
![Acid Acid](/uploads/1/2/5/7/125720481/521781005.jpg)
1) 51.63 mL of 70 wt% nitric acid solution
2) 948.37 mL of water
How do you prepare 5 percent nitric acid solution from 55 percent nitric acid?
Mix 5 parts acid 55 % with 50 parts distilled water.
What type of compound is HNO3 aq?
Is nitric acid an element compound or mixture?
What is the compound element HNO 3?
HNO3 (nitric acid) is a compound. It consists of the non-metallic elements hydrogen, nitrogen and oxygen. Nitric acid is a strong acid in solution with pH 1 to 2.
What is the compound name of HNO3AQ?
How do you prepare 10 percent of nitric acid?
how to prepare 10% nitric acid from 55% nitric acid
Is nitric acid a molecular compound?
What is nitric acid organic or non organic?
Nitric acid is an inorganic compound; no carbon in the molecule.
How do you prepare a solution of a 5mM nitric acid from glacial acetic acid?
It is impossible to transform the acetic acid in nitric acid.
What is the difference between concentrated nitric acid and nitric acid?
Nitric acid refers to the chemical in any form. 'Concentrated' specifically defines it in a concentrated solution.
Comparison between dilute solution of nitric acid and a concentrated nitric acid?
The diluted solution has a slight hint of red as the other is just clear
Is ammonium nitric acid a ionic or covalent?
There is no compound called ammonium nitric acid. Ammonium nitrate is ionic.
Is nitric acid a dilute acid?
Nitric acid can be dilute or concentrated. This is simply a matter of how much of it you have in a given amount of a solution, which is variable.
How do you prepare 1 percent nitric acid solution?
You would dissolve 1 part HNO3 into 99 parts of your solvent.
Compound that does not contain carbon?
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 the65 % 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 ofthe operator
How do you prepare 5 N HNO3 Solution?
You put 5 moles of HNO3 in a total volume of 1 liter of water.
How do you prepare a solution of 6N acetic acid from glacial acetic acid?
Since glacial acetic acid is 17.4N, you just use (M1)(V1) = (M2)(V2). Example: If you want to prepare 100mL of 6N: (17.4N)(x mL) = (6N)(100 mL). So, you need 34.5 mL of glacial, dilute to 100 mL with water.
How do you prepare 1 percent nitric acid solution?
You would dissolve 1 part HNO3 into 99 parts of your solvent.
What is -6n-2n16?
If you mean: -6n-2n = 16 then -8n = 16 and the solution to the equation is n = -2
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.
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?
If you apply the equation for a dilution (C1V1 = C2V2), and use 11.4 M HNO3 as the C1 value, 0.500 L as the V2 value and 0.470 M HNO3 as the C2 value, you should be able to solve for V1
How many milliliters of a stock solution of 11.1 m hno3 would be needed to prepare 0.500 l of 0.500 m hno3?
Simple C1V1 = C2V2 equality will do here. (0.500 L = 500 ml) (11.1 M HNO3)(X ml) = (O.500 M HNO3)(500 ml) 11.1X = 250 X = 22.5 milliliters
How prepare 6N NaOH solution into 0.275N NaOH solution?
Use the simple formula M1V1=M2V2. M being Molarity which is the same as Normality for NaOH. Say you want to make 500 mL of the 0.275N solution: 6N(x)=(0.275N)(500mL) Solve for X, X=23mL Check yourself: 23mL(6N)/500mL = 0.276N With these numbers it is difficult to find the exact amount for a standard pipet and volumetric flask so if you need that type of precision you will need to use an auto-pipetter.
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.
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 pH of a 0.200 M solution of HNO3?
What is the concentration of HNO3 in a solution with pH3.4?
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
HNO3 is an example of a mixture or a solution?
What volume of 16 m HNO3 will be needed to prepare 250 ml of 0.50 m HNO3?
Using the (M1*V1)=(M2*V2) equation, we can calculate the necessary volume of concentrated acid to make the diluted acid: [(16M HNO3)*(x mL HNO3)] = [(0.50M HNO3)*(250 mL HNO3)] Solve for x: x = [(0.50M HNO3)*(250 mL HNO3)] / (16M HNO3) x = 7.813 mL (of 16 M HNO3)
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