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kaykay11
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how do I make 1000ml of 0.1M Nitric acid with 65% Nitric acide (specific gravity 1.42g) and Molecular weight 63g/mol
To calculate the amount of 65% nitric acid needed, you will first need to determine the molarity of the 65% solution. This can be done by multiplying the concentration (65%) by the density of the solution (1.42 g/ml) and dividing by the molar mass of nitric acid (63.01 g/mol). This will give you a molarity of approximately 10 M. To prepare 1000ml of 0.1M nitric acid, you will need to dilute 10ml of 65% nitric acid with enough water to make a total volume of 1000ml.
65% nitric acid is a strong acid and can cause severe burns if it comes into contact with skin. It is also corrosive to metals and can release toxic fumes if mixed with certain chemicals. It is important to wear appropriate protective gear, such as gloves, goggles, and a lab coat, when handling this acid. It should also be stored in a well-ventilated area away from other chemicals.
No, it is not recommended to use tap water to dilute 65% nitric acid. Tap water contains impurities that can react with the acid and affect the accuracy of your solution. It is best to use deionized or distilled water for dilution.
The prepared 0.1M nitric acid solution should be stored in a tightly sealed, labeled container in a cool, dry place. It is recommended to use the solution within a few days to ensure its accuracy.
Yes, you can use a different concentration of nitric acid to prepare the 0.1M solution. However, you will need to recalculate the amount needed based on the new concentration. It is important to use the correct concentration to ensure the accuracy of your solution.