Question

How much concentrated solution would you take to prepare 1.15 L of 0.105 M HNO3 by mixing with water?

Answer 1

Answer:

7.67578 ml

Explanation:

assuming the missing information

Conc. of nitric acid = 70.3% by mass

density =1.41 g/ml

Now, moles of HNO3 required = final volume× final conc.

= 1.15×0.105= 0.12075 mol

Mass of HNO3 required = moles×molar mass of HNO3

= 0.12075×63.01=7.6084575 g

mass of solution = 100/70.3 of 7.6084575

=10.82284 g

therefore, volume of the solution = mass/density

= 10.82285/1.41

= 7.67578 ml

Answer 2

The amount of concentrated solution will be 7.67578 ml.

what is $\bold{HNO_3}$?

$\bold{HNO_3}$, nitric acid is a colorless pure compound which is also known as aqua fortis, and it is a highly corrosive mineral.

Calculation:

$\begin{aligned}\bold{Moles\;of\;HNO_3&=Volume \times concentration\\&=1.15\times 0.105\\&=0.12075}\end{aligned}$

$\begin{aligned}\bold{M\;of\;HNO_3&=Moles\times Molar\; mass\\&=0.12075\times 63.01\\&= 7.6084575}\end{aligned}$

$\bold{Mass\; of\; solution= \dfrac{100}{70.3}\times 7.6084574= 10.822849}$

$\bold{Therefore\; the\; Volume = \dfrac{m}{D} = \dfrac{10.82285}{1.41} = 7.67578\; ml}$

Thus, the concentration is 7.67578 ml.

Learn more about solution, here:

https://brainly.com/question/7932885