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Nitric Acid Concentration Formula:
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Nitric acid (HNO₃) concentration refers to the amount of nitric acid present in a solution. It can be expressed as a percentage (mass/volume) or as molarity (moles per liter). Accurate concentration measurement is essential for laboratory work and industrial processes.
The calculator uses the following formulas:
For percentage concentration:
\[ C(\%) = \frac{\text{mass of HNO}_3 (\text{g})}{\text{volume (L)}} \times 100 \]For molarity:
\[ C(\text{mol/L}) = \frac{\text{mass of HNO}_3 (\text{g})}{63.01 \text{ g/mol}} \div \text{volume (L)} \]Where:
Details: Knowing the exact concentration of nitric acid is crucial for chemical reactions, industrial processes, laboratory experiments, and safety considerations. Different concentrations have different applications and handling requirements.
Tips: Enter the mass of nitric acid in grams, the total volume of solution in liters, and select whether you want the result as a percentage or molarity. All values must be positive numbers.
Q1: What's the difference between percentage and molarity?
A: Percentage concentration is mass/volume percent, while molarity is the number of moles per liter of solution.
Q2: What is the molar mass of nitric acid?
A: The molar mass of HNO₃ is approximately 63.01 g/mol (1 H + 1 N + 3 O).
Q3: What are common concentrations of nitric acid?
A: Commercial nitric acid is typically 68-70% (concentrated), while dilute solutions might be 10% or less.
Q4: Why is nitric acid concentration important?
A: Concentration affects reactivity, safety hazards, and appropriate uses in chemical processes.
Q5: How should I handle nitric acid safely?
A: Always use proper PPE (gloves, goggles), work in a fume hood, and be aware that higher concentrations are more corrosive and dangerous.