Considering acetic acid dissociates in water, its dissociation constant is 6.25 × 10⁻⁵. If 5 ~mL 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: (K f) 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 CH₃ COOH CH₃ COO^()+H^()

JEE Main 2024 Solutions Question with Answer (5 Apr Evening shift, Q19)

JEE Main 20245 Apr, Evening shiftChemistryHardSolutions71× since 2002

Considering acetic acid dissociates in water, its dissociation constant is

6.25 \times 10^{-5}

. If

5 \mathrm{~mL}

of acetic acid is dissolved in 1 litre water, the solution will freeze at

-x \times 10^{-2}{ }^{\circ} \mathrm{C}

, provided pure water freezes at

0{ }^{\circ} \mathrm{C}

x=

_________. (Nearest integer)

\begin{aligned} \text{Given :} \quad & \left(\mathrm{K}_{\mathrm{f}}\right)_{\text {water }}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}-1 \\ & \text { density of acetic acid is } 1.2 \mathrm{~g} \mathrm{~mol}^{-1} \text {. } \\ & \text { molar mass of water }=18 \mathrm{~g} \mathrm{~mol}^{-1} \text {. } \\ & \text { molar mass of acetic acid= } 60 \mathrm{~g} \mathrm{~mol}^{-1} \text {. } \\ & \text { density of water }=1 \mathrm{~g} \mathrm{~cm}^{-3} \end{aligned}

Acetic acid dissociates as

\mathrm{CH}_3 \mathrm{COOH} \rightleftharpoons \mathrm{CH}_3 \mathrm{COO}^{\ominus}+\mathrm{H}^{\oplus}

Your answerType your answer. Integers and decimals are accepted.