Chemistry, 22.07.2019 19:00 tadvet5685

To what volume should you dilute 51 ml of a 13 m stock hno3 solution to obtain a 0.126 m hno3 solution?

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51 mL ${\text{HN}}{{\text{O}}_{\text{3}}}$ solution is diluted to $\boxed{{\text{5210}}{\text{.9 mL}}}$ to get the 0.126 M of solution.

Further explanation:

Molarity:

The molarity of the solution is defined as the concentration of the solution. It is equal to the number of moles of the solute dissolved in one liter of the solution.

The formula of molarity (M), volume (V), and number of moles (n) is as follows:

${\text{M}} = \frac{{\text{n}}}{{\text{V}}}$ …… (1)

Here V is a volume of solution in liters and n is a number of moles of solute.

If n is constant and is equal to k, the equation (1) will become:

${\text{MV}} = {\text{k}}$ …... (2)

If we have initial and final values of concentration and volume then the equation (2) can be modified as follows:

${{\text{M}}_{\text{1}}}{{\text{V}}_{\text{1}}}={{\text{M}}_{\text{2}}}{{\text{V}}_{\text{2}}}$ ……. (3)

Here,

${{\text{M}}_1}$ is the concentration before dilution.

${{\text{M}}_2}$ is the concentration after dilution.

${{\text{V}}_1}$ is the volume before dilution.

${{\text{V}}_2}$ is the volume after dilution.

On rearranging equation (3) for ${{\text{V}}_{\text{2}}}$ we get,

${{\text{V}}_{\text{2}}}=\frac{{{{\text{M}}_1}{{\text{V}}_1}}}{{{{\text{M}}_{\text{2}}}}}$ …… (4)

${{\text{M}}_1}$ is 13 M.

${{\text{M}}_2}$ is 0.126 M.

${{\text{V}}_1}$ is 51 mL.

Substitute the values of ${{\text{M}}_1}$ , ${{\text{M}}_2}$ and ${{\text{V}}_1}$ in equation(4).

$\begin{aligned}{{\text{V}}_{\text{2}}}&=\frac{{\left({{\text{13 M}}}\right)\times\left({{\text{51 mL}}}\right)}}{{{\text{(0}}{\text{.126}}\;{\text{M)}}}}\\&={\text{5261}}{\text{.90 mL}}\\\end{aligned}$

The volume of solution after dilution is 5261.90 mL.

The volume added to initial volume of solution is calculated as follows:

$\begin{aligned}{{\text{V}}_{{\text{added}}}}&={{\text{V}}_{\text{2}}}-{{\text{V}}_{\text{1}}} \\&={\text{5261}}{\text{.90 mL}}-{\text{51}}\;{\text{mL}}\\&={\text{5210}}{\text{.9}}\;{\text{mL}}\\\end{aligned}$

Hence, 51 mL is diluted to 5210.9 mL to get the 0.126 M of solution.

Learn more:

1. Write the equation to show how cation acts as an acid .

2. Calllculation of heat of vaporization:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Mole concept

Keywords: Number of moles, concentration, volume, volume of solution after dilution, solute, 1liter, molarity, 51 mL, 5210.9 mL, 13m, 0.126m.

Answer from: Quest

29.1-12=17.1the answer is this one

Answer from: Quest

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

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