Question

What is the final volume, in milliliters, when $25.0mL$. of each of the following solutions is diluted to provide the given concentration? $\left(9.5\right)$

a. $10.0\%\left(m/v\right)HCI$solution to give a $2.50\%\left(m/v\right)HCI$solution

b. $5.00MHCI$solution to give a $1.00MHCI$solution

c. $6.00MHCI$solution to give a $0.500MHCI$solution

Short answer

To get the saturated solution, dilute the following approach:

a. $10.0\%\left(m/v\right)HCI$solution to give a $2.50\%\left(m/v\right)HCI$solution

b. $5.00MHCI$solution to give a $1.00MHCI$solution

c. $6.00MHCI$solution to give a $0.500MHCI$solution

Step-by-step solution

Introduction:

Adding excess salt water to the titrated aqueous phase will reduce the saturation of the solution. This is related to the reason that the mole fraction of osmotic pressure does not change with increasing final volume.

Given:

The final volume, in milliliters, of each of the following solutions is diluted to provide the given concentration.

a. $100\%\left(m/v\right)HCI$solution to give a $2.50\%\left(m/v\right)HCI$solution

b. $5.00MHCI$solution to give a $1.00MHCI$solution

c. $6.00MHCI$solution to give a$0.500MHCI$ solution

part(a) Definition of Molarity and Density

Molarity:

The number of moles of solute per liter of solution is known as molarity of the solution. It symbolized by $M$. Molarity of any solution is a ratio of moles of solutes per liter of solution. It expressed by the following formula:

Molarity $\left(M\right)$=\frac{\text { moles of solutes }}{\text { liter of solution }}$