Determine the molarity (in mol/L) of NO2− ions in solution when 9.77×101 g of sodium nitrite is added to enough water to prepare 3.94×102 mL of the solution.
To determine the molarity of NO2− ions in solution, you need to follow these steps:
1. Convert the mass of sodium nitrite (NaNO2) to moles.
- The molar mass of NaNO2 is calculated by adding the atomic masses of sodium (Na), nitrogen (N), and two oxygen atoms (O).
- Na: 22.99 g/mol
- N: 14.01 g/mol
- O: 16.00 g/mol
Therefore, the molar mass of NaNO2 is (22.99 + 14.01 + 16.00 + 16.00) g/mol = 68.00 g/mol
To convert from grams to moles, divide the given mass by the molar mass:
Moles of NaNO2 = 9.77×101 g / 68.00 g/mol
2. Convert the volume of the solution from milliliters to liters.
To convert from milliliters to liters, divide the given volume by 1000:
Volume of solution = 3.94×102 mL / 1000 L/mL
3. Calculate the molarity (M) of NO2− ions.
Molarity is defined as the number of moles of solute (NO2− ions) divided by the volume of the solution in liters.
Molarity (M) = Moles of NaNO2 / Volume of solution
By following the above steps and plugging in the values in the equation, you should be able to calculate the molarity of NO2− ions in the solution.