25.00 mL of a sulfuric acid solution was standardized by titrating it with 0.2500 M NaOh using phenolphthalein indicator. 30.52 ml of the NaOH was required. Calculate the molarity of the sulfuric acid.

The molarity of the sulfuric acid is 0.1526 M

Explanation:

Step 1: Given data

Sulfuric acid = H2SO4

Volume of H2SO4 = 25.00 mL = 0.0250 L

Molarity of NaOH = 0.250 M

Volume of NaOH = 30.52 mL = 0.03052 L

Step 2: The balanced equation

H2SO4 + 2NaOH = Na2SO4 + 2H2O

Step 3: Calculate molarity of H2SO4

b*Ca*Va = a*Cb*Vb

⇒with b = the coefficient of NaOH = 2

⇒with Ca = the concentration of H2SO4 = TO BE DETERMINED

⇒with Va = the volume of H2SO4 = 25.00 mL = 0.0250 L

⇒with a = the coefficient of H2SO4 = 1

⇒with Cb = the concentration of NaOH = 0.250 M

⇒with Vb= the volume of NaOH = 30.52 mL = 0.03052 L

2*Ca * 0.0250 L = 0.250 M * 0.03052 L

Ca = (0.250 * 0.03052) / (2*0.0250)

Ca = 0.1526 M

The molarity of the sulfuric acid is 0.1526 M

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

yes it is balanced