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?

Question

Allison

Chemistry

3 April, 09:42

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?

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Answers (1)

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Kayleigh Combs · Answer 1

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.