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**Problem**: Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL.How much concentrated solution would you take to prepare 1.15 L of 0.115 M HNO3 by mixing with water?

###### FREE Expert Solution

The problem implies that we need to **calculate the volume of the concentrated solution **to be able to produce a 1.15 L of 0.115 M HNO_{3 }diluted solution.

The equation we use for** dilution** is shown below:

Where 1 and 2 are the initial (concentrated) and final (diluted) states respectively, M= molarity and V=volume.

###### Problem Details

Nitric acid is usually purchased in a concentrated form that is 70.3% HNO_{3} by mass and has a density of 1.41 g/mL.

How much concentrated solution would you take to prepare 1.15 L of 0.115 M HNO_{3} by mixing with water?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calculate Molarity concept. You can view video lessons to learn Calculate Molarity Or if you need more Calculate Molarity practice, you can also practice Calculate Molarity practice problems .

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Based on our data, we think this problem is relevant for Professor Banerjee's class at ECU.