Answer:
5.195 ml
Explanation:
Dissociation of HCl yields;
HCl(aq) ⇄ H⁺(aq) + Cl⁻(aq)
∴ [HCl] = [H⁺] = [Cl⁻]
pH = 1.9
= -log[ H⁺]
= [tex]10^{-pH}[/tex]
= [tex]10^{-1.9}[/tex]
= 0.01258 M
Moles of HCl = number of mole × volume
= 0.01258 × 4.80 L
= 0.06042 mole
Mass of HCl = number of moles of HCl × Molar mass of HCl
Mass of HCl = 0.06042 mol × 36.5 g/mol
Mass of HCl = 2.205 grams
Also, given that the density = 1.179 g/mL
Mass of HCl in the solution = 36% of the density
i.e [tex]\frac{36}{100}*1.179[/tex]
= 0.4244 grams
Volume of a concentrated HCl solution needed can now be determined as;
= [tex]\frac{2.205}{0.4244}[/tex]
= [tex]5.195 ml[/tex]
