A concentration solution of H2so4 is 59.4% by mass (m/m) and has a density of 1.83 g/mL. How many mL of the solution would be required to prepare 1550 mL of a .30M solution of the acid

41.5 mL

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

where,

n = moles of solute

= volume of solution in L

Given : 59.4 g of in 100 g of solution  

moles of

Volume of solution =

Now put all the given values in the formula of molality, we get

To calculate the volume of acid, we use the equation given by neutralisation reaction:

where,

are the molarity and volume of stock acid which is

are the molarity and volume of dilute acid which is

We are given:

Putting values in above equation, we get:

Thus 41.5 mL of the solution would be required to prepare 1550 mL of a .30M solution of the acid

particle   p is an electron and particle q is a neutron