Table of Contents
- 1 How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2 M HNO3 the concentrated acid is 70\% w/w HNO3 NEET 2013?
- 2 What is the volume of 63 HNO3 density?
- 3 What weight is 70 of HNO3?
- 4 What volume of water should be added to 50 ml of HNO3 having density 1.5 gram per ml?
- 5 What is HNO3 molarity?
- 6 How many molars is concentrated nitric acid?
- 7 How many grams of nitric acid are there in 100\% HNO3?
- 8 How do you convert moles to grams of HNO3?
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2 M HNO3 the concentrated acid is 70\% w/w HNO3 NEET 2013?
We now calculate the weight of \[HNO_3\] in 250 mL of solution. is present in 100g of solution. Hence, Option (D) 45.0g of conc. \[HNO_3\] is the correct answer.
What is the volume of 63 HNO3 density?
Density is 1.4 g/mL. Molarity of the solution is 1.2 M. 63\% weight means 63 gm of $HN{O_3}$ is present in 100 g of solution.
What weight is 70 of HNO3?
The density of 70\% (w/w)Nitric acid is 1.413 g/ml at 25°C which means that the weight of the 1 ml of Nitric acid is 1.413 gram at 25°C….Known values.
| Known values | |
|---|---|
| Molecular weight of HNO3 | 63.01 g/mole |
| Concentration of Nitric acid | 70\% (\% by mass, wt/wt) |
How do you make a 2 nitric acid solution?
For a 2\% solution the final weight of solution will be 13.4/. 02=670 grams. Therefore add 670–13.4=656.6 g of H2O, giving 670 g of 2\% HNO3.
How do you calculate moles of HNO3?
Divide the amount of HNO3 by 63 to determine how many moles there are in the amount of HNO3 you are using for your calculations. For example, if there are 1,000 grams of HNO3, divide 1000 by 63; the result will be the number of moles contained in 1,000 grams of HNO3, which is 15.87 moles.
What volume of water should be added to 50 ml of HNO3 having density 1.5 gram per ml?
Answer: Volume of water to be added to 50ml of HNO3 having density 1.5g/ml and 63\% by weight to have one molar solution is 700 ml.
What is HNO3 molarity?
Using 70\% concentrated nitric acid as an example: 70\% nitric acid means that 100 grams of this acid contains 70 grams of HNO3. Dividing the grams of HNO3 by the molecular weight of HNO3 (63.01 g/mole) gives the number of moles of HNO3 / L or Molarity, which is 15.7 M.
How many molars is concentrated nitric acid?
Dilutions to Make a 1 Molar Solution
| Concentrated Reagents | Density | Molarity (M) |
|---|---|---|
| Hydrochloric acid 36\% | 1.18 | 11.65 |
| Hydrochloric acid 32\% | 1.16 | 10.2 |
| Hydrofluoric acid 40\% | 1.13 | 22.6 |
| Nitric acid 70\% | 1.42 | 15.8 |
How do you prepare 250 ml of concentrated HNO3 solution?
The concentrated acid is 70\% HNO3. So 1000 ml.of Solution contains=700 g. To prepare 250 ml.of 2.0M HNO3 we require= 250 x 2/11.11= 45.0045 ml. (Or) 45 ml.of 70\% HNO3. 70\% HNO3 will contain 700 gm/L of the acid.
How many grams of concentrated nitric acid should be used to prepare?
Thus 45.0 g conc. H N O3 of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M H N O3
How many grams of nitric acid are there in 100\% HNO3?
31.5gms of HNO3 contains in (100/70) *31.5 ml=45ml. 70\% Conc.HNO3 means, it contains 70 gm. HNO3 in 100 ml.of the solution. So 1000 ml.of the 70\% HNO3 contains 700 gm of nitric acid. So 11.11 x V=250 x 3.
How do you convert moles to grams of HNO3?
Step2: Convert the moles of HNO3 into mass. Mass = moles x molar mass = 0.50 moles x 63.01g/mole = 31.5 g HNO3. Thus, 31.5 g HNO3 will be present in 100g x 31.5 g HNO3/70g = 45g solution.
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