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 .

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

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