Nitric acid is usually purchased in a concentrated form that is 70.3% hno3 by mass and has a density of 1.41 g/ml. how much concentrated solution would you take to prepare 1.15 l of 0.115m hno3 by mixing with water?

to prepare a 0.115 M HNO3 solution, 11.85 mL of the concentrate solution is needed and water is added until the desired volume of 1.15 L is reached

Explanation:

%w/w = 70.3% = g HNO3/g sln * 100

⇒ 0.703 = g HNO3/g sln

let g sln = 1000g:

⇒ g HNO3 = 0.703 * 1000g = 703g HNO3

⇒ mol HNO3 = 703g * ( mol/63.01g HNO3) = 11.157 mol HNO3

for 1 L of solution:

⇒ C HNO3 = 11.157 mol/ L

dilution formula:

V1*C1 = V2*C2

∴ C1= 11.157 mol/L

∴ C2 = 0.115 mol/L

∴ V2 = 1.15 L

⇒ V1 = V2*C2 / C1

⇒ V1 = ((1.15 L)*(0.115 mol/L)) / 11.157 mol/L

⇒ V1 = 0.01185 L (11.85 mL)

That result from subduction of oceanic plates beneath lighter continental plates. most of the earth's volcanoes are located around the pacific ring of fire because that the location of most of the earth's subduction zones.

And a) oxygen i believe