**Molarity of 70% (w/w) Nitric acid (HNO****3****)**

**Overview:**

- Nitric acid is a clear colourless liquid. A 70% (w/w) concentrated Nitric acid can be obtained from different suppliers.
- 70% (w/w) Nitric acid means that 100 grams of Nitric acid contains 70 grams of HNO3.
- The density of 70% (w/w)Nitric acid is 1.413 g/ml at 25°C that means that weight of the 1 ml of Nitric acid is 1.413 gram at 25°C.
- Molarity refers to number of moles of the solute present in 1 litre of solution.
- In simple words, 1 mole is equal to atomic weight of the substance. For example, 1 mole of HNO3 is equal to 63.01 grams of HNO3 (molecular weight = 63.01).

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**Calculation procedure:**

**Known values:**

Density of Nitric acid : 1.413 g/ml

Molecular weight of HNO3: 63.01 g/mole

Concentration of Nitric acid: 70% (% by mass, wt/wt)

**Step 1: Calculate the volume of 100 grams of Nitric acid.**

**Formula:**

Density = weight / volume or

Volume = weight / density or

Volume of 100 gram of Nitric acid : 100/1.413 = 70.771 ml

Note: 70% (w/w) Nitric acid means that 100 grams of Nitric acid contain 70 grams of HNO3.

**The volume of 100 grams of Nitric acid is 70.771 ml. That means 70 grams of HNO****3**** is present in 70.771 ml of Nitric acid.**

**Step 2: Calculate how many grams of HNO****3**** is present in 1000 ml of Nitric acid.**

70.771 ml of Nitric acid contain = 70 grams of HNO3

1 ml of Nitric acid will contain = 70/70.771 grams of HNO3

1000 ml of Nitric acid will contain = 1000 x 70/70.771 = 989.106 grams of HNO3

**1000 ml of Nitric acid will contain 989.106 grams of HNO****3**

**Step 3: Calculate number of moles of HNO3 present in 989,106 grams of HNO3.**

63.01 grams of HNO3 is equal to 1 mole.

1 gram of HNO3 will be equal to 1/63.01 moles.

989.106 grams will be equal to = 989.106 x 1/63.01 = 15.6976 moles

**Therefore, we can say that 1 litre of Nitric acid contains 15.6976 moles or in other words molarity of 70% (w/w) Nitric acid is equal to 15.6976 M.**