Question

if 25 ml of a h2so4 solution reacts completely with 1.06g of pure na2co3 what is the normality of this acid solution

Answer 1

Answer:-  0.80 N.

Solution:- sulfuric acid and sodium carbonate reacts as given below:

$Na_2CO_3+H_2SO_4\rightarrow Na_2SO_4+H_2O+CO_2$

From this equation, they react in 1:1 mol ratio. Grams of sodium carbonate are converted to moles and then using mol ratio we calculate the moles of sulfuric acid. mL are divided to liters and the moles of sulfuric acid are divided by the liters to get the molarity. Basicity of sulfuric acid is 2 as one mol of it gives two moles of hydrogen ions.

normality = molarity*basicity

The calculations are shown below:

$1.06gNa_2CO_3(\frac{1mol}{106g})(\frac{1molH_2SO_4}{1molNa_2CO_3})$

= $0.01molH_2SO_4$

Volume of sulfuric acid used is 25 mL.  Let's convert it to Liters.

$25mL(\frac{1L}{1000mL})$ = 0.025 L

molarity of sulfuric acid = [tex]\frac{0.01mol}{0.025L}

= 0.40 M

Normality = 2(0.40) = 0.80 N

So, the normality of sulfuric acid solution is 0.80 N.