Answer :
Answer:
You will need to dilute 7.30 ml of the concentrated solution into the 1.15 L of the diuluted one by adding water.
Explanation:
First you need to calculate how much acid you'll need in order to prepare the diluted solution. If you know the volume and the molarity, just multiply.
1.15 l * 0.1 M = 0.115 mols of HNO3
Multiplying by the molar mass you'll convert that value into grams
0.115 * 63g/mol = 7.245 g HNO3
Now you use the concentrated solution to know how much to extract.
70.3 g of HNO3 pure are in 100 g of Solution, then 7.245 are in x
X= (7.245 * 100)/ 70.3 = 10.3 grams of concentrated solution.
Using the density you convert the mass into volume:
V = m/dens --> V = 10.3 g / 1.41 g/ml --> V= 7.3 ml
You'll take 7,30 ml of the concentrated solution and add water until reach the required volume for the solution.
You will need to dilute 9.597 ml of the concentrated solution to prepare 1.15 L of 0.100 M HNO3 from the concentrated solution.
What is nitric acid?
Nitric acid is a very corrosive mineral acid also known as aqua fortis and the spirit of niter.
The pure chemical is colorless, but breakdown into nitrogen oxides and water causes older samples to turn yellow.
Given,
The percentage of nitric acid concentration is 70.03%
The density of the concentration is 1.41 g/ml
The final concentration is 0.100 m
The final volume is 1.15 L
The molar mass of nitric acid is 63.0 g/mol
To prepare the final solution, we are using the volume of the solution
[tex]\bold{V_1=\dfrac{C_2}{ C1}V_2}[/tex]
[tex]\bold{ V_1=\frac{C_2}{\dfrac{ xp}{M}} V_2}[/tex]
[tex]\bold{V_1=\dfrac{MC_2V_2}{ xp}}[/tex]
[tex]\bold{V_1=\dfrac{63.0\; g/mol\times 0.100 M\times 1.51 L}{70.3\%\times 1.41 g/ml}= 9.597\;ml }[/tex]
Thus, the volume is 9.597 ml.
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