Considering acetic acid dissociates in water, its dissociation constant is 6.25 \times 10^{-5}. If 5 {\mL} of acetic acid is dissolved in 1 litre water, the solution will freeze at - {\x} \times 10^{-2}{ }^{\circ} {\C}, provided pure water freezes at 0{ }^{\circ} {\C}. {\x}= _______ . (Nearest integer) Given : ( {\K}_{ {\f}}) _{\text{water }}=1.86 {\K} {\kg} {\mol}^{-1}. density of acetic acid is 1.2 {\g} {\mol}^{-1} molar mass of water =18 {\g} {\mol}^{-1}. molar mass of acetic acid =60 {\g} {\mol}^{-1}. density of water =1 {\g} {\cm}^{-3} Acetic acid dissociates as {\CH}_3 {\COOH} ⇌ {\CH}_3 {\COO}^{⊕}+ {\H}^{⊕} [5 Apr 2024 Shift 2]

Solutions Part 2

Section: Chemistry

Question : 41 of 86

Marks: +1, -0

Considering acetic acid dissociates in water, its dissociation constant is 6.25×10−5. If 5‌mL of acetic acid is dissolved in 1 litre water, the solution will freeze at −x×10−2‌∘C, provided pure water freezes at 0‌∘C.
x= _______ . (Nearest integer)
Given : (Kf)‌water ‌=1.86K‌kg‌mol−1.
density of acetic acid is 1.2gmol−1
molar mass of water =18gmol−1.
molar mass of acetic acid =60gmol−1.
density of water =1gcm−3
Acetic acid dissociates as
CH3‌COOH⇌CH3COO⊕+H⊕

[5 Apr 2024 Shift 2]

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