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Answer :
Final answer:
To calculate the molarity of hydroiodic acid with a density of 1.70 g/cc, convert the mass of 1 L of the acid to moles using its molar mass, and then divide by the volume in liters. Assuming the solution is pure hydroiodic acid, the result is approximately 6.67 M.
Explanation:
Calculating the Molarity of Hydroiodic Acid
To calculate the molarity of a liquid hydroiodic acid with a density of 1.70 g/cc, we need to follow these steps:
- Use the density to find the mass of 1 L of the hydroiodic acid (since 1 cc is equivalent to 1 mL, and there are 1000 mL in 1 L).
- Convert the mass of the liquid hydroiodic acid to moles using the molar mass of hydroiodic acid (HI), which is approximately 127.9 g/mol for H plus 126.9 g/mol for I, totaling approximately 254.8 g/mol.
- Divide the moles of hydroiodic acid by the volume of the solution in liters to get the molarity.
For instance, 1 L of hydroiodic acid with a density of 1.70 g/cc will have a mass of 1700 g. To convert this mass to moles, you would calculate 1700 g HI / 254.8 g/mol HI which gives approximately 6.67 moles of HI. Therefore, the molarity of the acid would be 6.67 moles per 1 L, or 6.67 M.
Note that this calculation assumes the solution is made up solely of hydroiodic acid and does not account for the presence of any other substances.
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