Asked by karen
How many milliliters of concentrated nitric acid, HNO3, 70 % (wt/wt) are required to prepare 1 liter of 0.250 M solution? The molar mass and density of HNO3 are 63.0 g/mol and 1.36 g/cm respectively.
Answers
Answered by
DrBob222
First, what is the M of the 70% HNO3. That's
1.36 g/mL x 1000 mL x 0.70 x (1/63) = ? M1
Then M1 x mL1 = M2 x mL2
M2 is 0.250; mL2 = 1000 mL, solve for mL1.
1.36 g/mL x 1000 mL x 0.70 x (1/63) = ? M1
Then M1 x mL1 = M2 x mL2
M2 is 0.250; mL2 = 1000 mL, solve for mL1.
Answered by
Nur
First, what is the M of the 70% HNO3. That's
1.36 g/mL x 1000 mL x 0.70 x (1/63) = ? M1
Then M1 x mL1 = M2 x mL2
M2 is 0.250; mL2 = 1000 mL, solve for mL1
1.36 g/mL x 1000 mL x 0.70 x (1/63) = ? M1
Then M1 x mL1 = M2 x mL2
M2 is 0.250; mL2 = 1000 mL, solve for mL1
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