(A) In the titration of a weak acid $(CH_3COOH)$ with a strong base $(NaOH)$,the salt formed $(CH_3COONa)$ undergoes anionic hydrolysis,resulting in a

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(A) In the titration of a weak acid $(CH_3COOH)$ with a strong base $(NaOH)$,the salt formed $(CH_3COONa)$ undergoes anionic hydrolysis,resulting in a basic solution at the equivalence point $(pH > 7)$.Due to the excess of free base added beyond the equivalence point,there is a steep rise in $pH$,which is represented by the vertical portion of the titration curve.Therefore,the vertical line in the graph indicates the alkaline nature of the equivalence point.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Mix Examples-Ionic Equilibrium

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During the titration of acetic acid with an aqueous $NaOH$ solution,the neutralization graph shows a vertical line. This line indicates:

AIIMS 2007 All AIIMS

A
alkaline nature of equivalence
B
acidic nature of equivalence
C
neutral nature of equivalence
D
depends on experimental procedure

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Class 11

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6-2.Equilibrium-II (Ionic Equilibrium)

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Mix Examples-Ionic Equilibrium

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At $90 \, ^\circ C$,the concentration of $H^+$ and $OH^-$ ions in pure water is $10^{-6} \, M$. What is the value of $[H^+] + [OH^-]$ at this temperature?

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$A$ $20 \ mL$ sample of a $0.2 \ M$ solution of the weak diprotic acid $H_2A$ is titrated with $0.25 \ M \ NaOH$. Molarity of the solution at the second equivalence point is:

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At $25^{\circ} C$, the ionic product of water is $10^{-14}$. The free energy change for the self-ionization of water in $kCal \ mol^{-1}$ is close to

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Estimate the approximate $pK_a$ of $0.5 \ M$ $CH_3COOH$. Degree of dissociation (ionisation) is $0.15$ $(\log 1.32 = 0.12)$.

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The degree of dissociation of a $0.1 \, M$ $CH_3COOH$ solution is $1.32 \times 10^{-2}$. What will be its dissociation constant $(K_a)$?

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During the titration of acetic acid with an aqueous $NaOH$ solution,the neutralization graph shows a vertical line. This line indicates:

Similar Questions

At $90 \, ^\circ C$,the concentration of $H^+$ and $OH^-$ ions in pure water is $10^{-6} \, M$. What is the value of $[H^+] + [OH^-]$ at this temperature?

$A$ $20 \ mL$ sample of a $0.2 \ M$ solution of the weak diprotic acid $H_2A$ is titrated with $0.25 \ M \ NaOH$. Molarity of the solution at the second equivalence point is:

At $25^{\circ} C$, the ionic product of water is $10^{-14}$. The free energy change for the self-ionization of water in $kCal \ mol^{-1}$ is close to

Estimate the approximate $pK_a$ of $0.5 \ M$ $CH_3COOH$. Degree of dissociation (ionisation) is $0.15$ $(\log 1.32 = 0.12)$.

The degree of dissociation of a $0.1 \, M$ $CH_3COOH$ solution is $1.32 \times 10^{-2}$. What will be its dissociation constant $(K_a)$?

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