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How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 14.0 L of a solution that has a pH of 2.12?

Respuesta :

w=0.360
p=1.18g/mL
pH=2.12
v=14.0 L
M(HCl)=36.46 g/mol
v₀-?

1) pH=-lg[H⁺]

    [H⁺]=c(HCl)=10^(-pH)

    n(HCl)=v[H⁺]=v*10^(-pH)

2) n(HCl)=m(HCl)/M(HCl)=wv₀p/M(HCl)

3) v*10^(-pH)=wv₀p/M(HCl)

    v₀=v*10^(-pH)M(HCl)/(wp)
  
    v₀=14.0*10^(2.12)*36.46/(0.360*1.18)=9.115 mL


Approximately 9.1 mL of concentrated solution required.




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