The millimoles of silver nitrate the chemist added to the flask, given that the chemist adds 70.0 mL of solution to the flask is 280 millimoles
How to calculate the millimoles of silver nitrate added to the solution?
The molarity of a solution is related to the mole of the solute and volume of the solution by the following equation:
Molarity of solution = mole of solute / volume of solution
Thus,
Mole of solute = molarity of solution × volume of solution
Using the above formula, we can calculated the millimoles of silver nitrate added to the solution. This is shown below:
- Volume of silver nitrate solution = 70 mL = 70 / 1000 = 0.07 L
- Molarity of silver nitrate solution = 4.0 M
- Millimole of silver nitrate solution added =?
Mole of solute = molarity of solution × volume of solution
= 4.0 × 0.07
= 0.28 mole
Multiply by 1000 to express in millimole
= 0.28 × 1000
= 280 millimoles
Complete question:
A chemist adds 70.0mL of a 4.0 M silver nitrate, AgNO3, solution to a reaction flask. Calculate the millimoles of silver nitrate the chemist has added to the flask. Round your answer to significant digits.