How do you make a 5\% nitric acid solution?
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How do you make a 5\% nitric acid solution?
The volume of 7.14 g of concentrated HNO3 can be obtained from the density V = 7.14 g / 1.42 = 5.03 mL. If you then measure 5.03 mL of the concentrated HNO3 and dilute to 100 mL with water, you would have the required 5\% solution.
What is the molarity of 70 nitric acid?
Dilutions to Make a 1 Molar Solution
| Concentrated Reagents | Density | Molarity (M) |
|---|---|---|
| Nitric acid 70\% | 1.42 | 15.8 |
| Perchloric acid 60\% | 1.54 | 9.2 |
| Perchloric acid 70\% | 1.67 | 11.6 |
| Orthophosphoric acid 85\% | 1.7 | 15.2 |
How do you calculate nitric acid?
Knowing the density of the acid to be 1.413 g/mL, we can calculate the weight of 1 L of 70\% HNO3 to be 1413 grams. Knowing that the solution is 70 wt \% would then allow the number of grams of HNO3 to be calculated: (0.700)(1413g) = 989.1 grams HNO3 per liter.
Can you dilute nitric acid with water?
Add the concentrated acid slowly to the water with stirring. Dissolution of the concentrated acid will generate heat. 5. With distilled water from the wash bottle, rinse the remaining acid from the small measuring cylinder into the solution in the large beaker.
How do you make a 1 molar solution of nitric acid?
1L contains 15.6 moles, therefore 1 mole is contained within = 1L / 15.6 moles. Add 64.1mL, or 90.4g, of SEASTAR™’s Nitric Acid to water up to 1L to make a 1 Molar Solution of Nitric Acid.
How do you make 6 molar nitric acid?
For example, to make 500 mL of 6M HCl, use 250 mL of concentrated acid and slowly dilute to 500 mL with water….Recipes for Acid Solutions.
| Name / Formula / F.W. | Concentration | Amount/Liter |
|---|---|---|
| Nitric Acid | 6 M | 380 mL |
| HNO3 | 3 M | 190 |
| F.W. 63.01 | 1 M | 63 |
| 70.0\%, 15.8 M | 0.5 M | 32 |
How do you change concentrated nitric acid to dilute nitric acid?
How do you dissolve nitric acid in water?
Dissolving 1.5 grams of nitric acid in 150 grams of water gives 1\%. This is the same as dissolving 1 mL of nitric acid in 150 mL of water. The extra 50 mL of the solution is to be poured in another container. It is also 1\% of nitric acid. Another very difficult method is to dissolve 2/3 mL of nitric acid in 100 mL of water.
How much nitric acid do I need to make a solution?
Thirdly, you would need to work out how you would pay for all that nitric acid. Given that 70\% commercial nitric is around 15.7 molar, and you wish to end up with 0.5 M, you need around 32 millilitres of the 70\% acid per litre of solution.
How much HNO3 = 32\% nitric acid?
So : 470.6 ml of 68\% HNO3 diluted to* 1000 ml ( when cooled down back to lab temp ), will give you 1 liter of 32\% nitric acid Mind you : not 470 ml plus 1000 ml of water, but 470.6 + water up to 1000 ml !
What is the density of a 69\% nitric acid?
A 69 \% weight nitric acid’s density is 1,4091 g/cm3 at 20 °C according to this data table: So 1000 cm3 of 100\% nitric acid solution is equal to 1409,1g. So you need 92,7 cm3 of 69\% solution and you need to add water to fill up a flask of one liter Assuming that you want to make a 1000cm3 1,5N solution.