Posted by Samantha on Monday, December 17, 2012 at 7:33pm.
Available is a 5 M/liter solution. You need 100 mL of a 0.91 M solution.
In units of moles, you need 0.91 mol/liter * 0.1 liter = 0.091 moles of HNO3
0.091 moles / (5moles/liter) = 0.0182 liters of the 5 M solution.
Take 0.0182 liters of the 5 M solution, and dilute to 100 mL = 0.1 L (add 0.1 - 0.0182 = 0.0818 L = 81.8 mL of water to this solution.
Related Questions
college chemistry - Suppose you have a 0.200 M solution of the nitrogen-...
science - The concentration of commercially available concentrated nitric acid ...
Math - To conduct a scientific experiment, students need to mix 90 mL of a 3% ...
Chemistry - What will be the molarity of the resulting solutions made by mixing ...
chemistry - A 0.115-L sample of an unknown HNO3 solution required 31.1 mL of 0....
chemistry - Describe in detail, the steps a student needs to carry out to ...
Chemistry - help...If exactly 5.0 mL of HNO3 will neutralize 15 mL of 2.0 M NaOH...
Chemistry 104 - Nitric acid, HNO3, is available commercially at a concentration ...
Chem 1 - How can you prepare 2M of 200 ml HNO3 solution from 63% stock solution...
CHEMISTRY - HOW YOU PREPARE 30.0ML OF 0.800M HNO3 FROM A STOCK SOLUTION OF 4.OOM...
For Further Reading
