How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce

Question

fiasKO [112]

4 years ago

13

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?

Chemistry

1 answer:

poizon [28] · Answer 1 · 2022-01-22T19:39:37+03:00

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.