Question

Generally commercial hydrochloric acid is prepared by heating NaCl with concentrated H2SO4. How much H2SO4 solution containing 96 % H2SO4 by mass is required for the production 1000 kg of concentrated hydrochloric acid containing 43.8 % HCl by weight)​

Answer 1

612.5 kg of 96% sulfuric acid solution will be needed.

Explanation:

Mass by mass percentage :

$(m/m)\%=\frac{\text{Mass of solute}}{\text{Mass of solution}}\times 100$

Mass of 43.8 % HCl solution = 1000 kg

Mass of HCl = x

$43.8\%=\frac{x}{1000 kg}\times 100$

x = 438 kg

Mass of HCl = 438 kg = 438,000 g ( 1kg =1000g)

Moles of HCl = $\frac{438,000 g}{36.5 g/mol}=12,000 mol$

$2NaCl+H_2SO_4\rightarrow 2HCl+Na_2SO_4$

According to reaction, 2 moles of HCl are obtained from 1 mole of sulfuric acid ,then 12,000 moles of HCl will be obtained from :

$\frac{1}{2}\times 12,000mol=6,000 mol$ of sulfuric acid

Mass of 6,000 moles of sulfuric acid :

6,000 mol × 98g/mol = 588,000 g = 588 kg

Mass of 96% sulfuric acid solution = m

$96\%=\frac{588 kg}{m}\times 100$

m = 612.5 kg

612.5 kg of 96% sulfuric acid solution will be needed.

Learn more about: Mass by mass percentage and mole concept

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