How do you prepare 250.00 ml of 3.00 m hcl solution starting with a concentrated hcl solution which is 36.0% hcl by mass and has a density of 1.18 g/ml?

64.1 ml of concentrated is taken and (250-64.4)= 185.6 ml f water is added to make 250.00 mL of 3.00 M HCl .

Explanation:

Given : 36 g of is dissolved in 100 g of solution.

Density of solution = 1.18 g/ml

Thus volume of solution =

where,

n= moles of solute

= volume of solution

According to the dilution law,

where,

= molarity of stock solution = 11.7M

= volume of stock solution = V ml

= molarity of diluted solution = 3.00 M

= volume of diluted solution = 250.0 ml

Thus 64.1 ml of stock is taken and (250-64.4)= 185.6 ml of water is added to make 250.00 mL of 3.00 M HCl .

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.

yes the answer is total mass in unchanged   : )