Answer:
Explanation:
HCl ⇄ H⁺ + Cl⁻
HCl is a strong electrolyte so it will ionize completely .
moles of Cl⁻ in 100 mL of .1 HCl = .1 x .1 = .01 gram - ion .
CaCl₂ = Ca⁺² + 2 Cl⁻
1 mole 2 mole
moles of CaCl₂ in 200 mL of .1 M CaCl₂ = .2 x .1 = .02 gram mole .
.02 gram mole of CaCl₂ will give 2 x .02 = .04 gram-ion of Cl⁻ ion .
Total gram - ion of Cl⁻ = .01 + .04 = .05 gram-ion .
Total volume = 300mL = .3 L
molarity of Cl⁻ = .05 / .3 = .167 M .
HCl ⇄ H⁺ + Cl⁻
moles of H⁺ = moles of Cl⁻ = .01 gram-ion .
volume of solution = .3 L
molarity of H⁺ = .01 / .3 = 33.33 x 10⁻³ M .
[ H⁺] [ OH⁻] = 10⁻¹⁴
33.33 x 10⁻³ [ OH⁻] = 10⁻¹⁴
[ OH⁻] = 3 x 10⁻¹³
pOH = - log[OH⁻] = - log3 x 10⁻¹³
13-log3
= 13 - .477
12.52
or ,
pH = - log[H⁺] = - log33.33 x 10⁻³
3 - log 33.33
= 3 - 1.52
= 1.48
pOH = 14 - 1.48 = 12.52
