How many liters of a $12\%(m/v)KOH$solution would you need to obtain $86.0gofKOH$?$(9.4)$

It has a variety of industrial and niche applications, the majority of which take advantage of its caustic nature and acid reactivity.

The molar mass of a solution is defined as the molar concentration per litre of solution.$M$ indicates it. A solution's molarity is described as the amount of units of solute molecules per litre of solution. The following formula explains it:

$Molarity\left(M\right)=\frac{molesofsolutes}{literofsolution}$

A substance's density is simply the ratio of its weight to its volume. A substance's density can be measured as its grams per cubic centimeter.

$\text{density}\left(\mathrm{g}/{\mathrm{cm}}^3\right)=\frac{\mathrm{mass}\left(\mathrm{g}\right)}{\text{volume}\left({\mathrm{cm}}^3\right)}\text{or}\frac{\text{mass}\left(\mathrm{g}\right)}{\text{volume}\left(\mathrm{mL}\right)}$

The mass percent calculator will help decide the mass of an element in a substance in proportion to the overall amount of substance.

Mass percentage is a concentration expression for a solute that can be estimated of the optimizer mass. The following formula defines it:

$masspercentageofsolute=\frac{gramsofsolute}{gramsofsolution}\times 100\%$

The weight of the solute present provides the mass percentage (m/v).

$Masspercentinm/v=\left(\frac{massofsolute}{volumeofsolution}\right)\times 100\%$

$Masspercentinm/v=\left(\frac{massofsolute}{volumeofsolution}\right)\times 100\%$

$12\%=\left(\frac{86.0g}{volumeofsolutioninmL}\right)\times 100\%$

$VolumeofsolutioninmL=\frac{86}{12}\times 100$

$=716mLor0.716L$

To produce $86.0gofKOH$, $0.716L$of a $12\%ofKOH$solution was required.