315026 Calculate the percent dissociation of $\mathrm{HOCl}$ of $0.08\mathrm{M}$ solution of hypochlorous acid. The ionisation constant of the acid is $2.5\times {10}^{-5}$.

315027 Which of the following statement(s) is/are correct?
(A) The pH of $1\times {10}^{-8}\mathrm{MHCl}$ solution is 8 .
(B) The conjugate base of ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ is ${\mathrm{HPO}}_4^{-2}$.
(C) ${\mathrm{K}}_{\mathrm{w}}$ increases with increase in temperature.
(D) When solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point, $\mathrm{pH}={\displaystyle \frac{1}{2}}{\mathrm{pK}}_{\mathrm{a}}$.
Choose the correct answer from the options given below :

315028 Aspirin is a pain reliever with $\text{p}{\text{K}}_{\text{a}}\text{ = 2}$.
Two tablets each containing $0.09\mathrm{g}$ of aspirin are dissolved in $100\mathrm{mL}$ solution. $\mathrm{pH}$ will be

315029 The degree of ionisation of a $0.1\mathrm{M}$ bromoacetic acid solution is 0.132. Calculate the $\mathrm{pH}$ of the solution.

315030 A weak acid HA has degree of dissociation $x$. Thus $\left(\text{pH - p}{\text{K}}_{\text{a}}\right)\text{is}$

315026 Calculate the percent dissociation of $\mathrm{HOCl}$ of $0.08\mathrm{M}$ solution of hypochlorous acid. The ionisation constant of the acid is $2.5\times {10}^{-5}$.

315027 Which of the following statement(s) is/are correct?
(A) The pH of $1\times {10}^{-8}\mathrm{MHCl}$ solution is 8 .
(B) The conjugate base of ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ is ${\mathrm{HPO}}_4^{-2}$.
(C) ${\mathrm{K}}_{\mathrm{w}}$ increases with increase in temperature.
(D) When solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point, $\mathrm{pH}={\displaystyle \frac{1}{2}}{\mathrm{pK}}_{\mathrm{a}}$.
Choose the correct answer from the options given below :

315028 Aspirin is a pain reliever with $\text{p}{\text{K}}_{\text{a}}\text{ = 2}$.
Two tablets each containing $0.09\mathrm{g}$ of aspirin are dissolved in $100\mathrm{mL}$ solution. $\mathrm{pH}$ will be

315029 The degree of ionisation of a $0.1\mathrm{M}$ bromoacetic acid solution is 0.132. Calculate the $\mathrm{pH}$ of the solution.

315030 A weak acid HA has degree of dissociation $x$. Thus $\left(\text{pH - p}{\text{K}}_{\text{a}}\right)\text{is}$

315026 Calculate the percent dissociation of $\mathrm{HOCl}$ of $0.08\mathrm{M}$ solution of hypochlorous acid. The ionisation constant of the acid is $2.5\times {10}^{-5}$.

315027 Which of the following statement(s) is/are correct?
(A) The pH of $1\times {10}^{-8}\mathrm{MHCl}$ solution is 8 .
(B) The conjugate base of ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ is ${\mathrm{HPO}}_4^{-2}$.
(C) ${\mathrm{K}}_{\mathrm{w}}$ increases with increase in temperature.
(D) When solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point, $\mathrm{pH}={\displaystyle \frac{1}{2}}{\mathrm{pK}}_{\mathrm{a}}$.
Choose the correct answer from the options given below :

315028 Aspirin is a pain reliever with $\text{p}{\text{K}}_{\text{a}}\text{ = 2}$.
Two tablets each containing $0.09\mathrm{g}$ of aspirin are dissolved in $100\mathrm{mL}$ solution. $\mathrm{pH}$ will be

315029 The degree of ionisation of a $0.1\mathrm{M}$ bromoacetic acid solution is 0.132. Calculate the $\mathrm{pH}$ of the solution.

315030 A weak acid HA has degree of dissociation $x$. Thus $\left(\text{pH - p}{\text{K}}_{\text{a}}\right)\text{is}$

315026 Calculate the percent dissociation of $\mathrm{HOCl}$ of $0.08\mathrm{M}$ solution of hypochlorous acid. The ionisation constant of the acid is $2.5\times {10}^{-5}$.

315027 Which of the following statement(s) is/are correct?
(A) The pH of $1\times {10}^{-8}\mathrm{MHCl}$ solution is 8 .
(B) The conjugate base of ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ is ${\mathrm{HPO}}_4^{-2}$.
(C) ${\mathrm{K}}_{\mathrm{w}}$ increases with increase in temperature.
(D) When solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point, $\mathrm{pH}={\displaystyle \frac{1}{2}}{\mathrm{pK}}_{\mathrm{a}}$.
Choose the correct answer from the options given below :

315028 Aspirin is a pain reliever with $\text{p}{\text{K}}_{\text{a}}\text{ = 2}$.
Two tablets each containing $0.09\mathrm{g}$ of aspirin are dissolved in $100\mathrm{mL}$ solution. $\mathrm{pH}$ will be

315029 The degree of ionisation of a $0.1\mathrm{M}$ bromoacetic acid solution is 0.132. Calculate the $\mathrm{pH}$ of the solution.

315030 A weak acid HA has degree of dissociation $x$. Thus $\left(\text{pH - p}{\text{K}}_{\text{a}}\right)\text{is}$

315026 Calculate the percent dissociation of $\mathrm{HOCl}$ of $0.08\mathrm{M}$ solution of hypochlorous acid. The ionisation constant of the acid is $2.5\times {10}^{-5}$.

315027 Which of the following statement(s) is/are correct?
(A) The pH of $1\times {10}^{-8}\mathrm{MHCl}$ solution is 8 .
(B) The conjugate base of ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ is ${\mathrm{HPO}}_4^{-2}$.
(C) ${\mathrm{K}}_{\mathrm{w}}$ increases with increase in temperature.
(D) When solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point, $\mathrm{pH}={\displaystyle \frac{1}{2}}{\mathrm{pK}}_{\mathrm{a}}$.
Choose the correct answer from the options given below :

315028 Aspirin is a pain reliever with $\text{p}{\text{K}}_{\text{a}}\text{ = 2}$.
Two tablets each containing $0.09\mathrm{g}$ of aspirin are dissolved in $100\mathrm{mL}$ solution. $\mathrm{pH}$ will be

315029 The degree of ionisation of a $0.1\mathrm{M}$ bromoacetic acid solution is 0.132. Calculate the $\mathrm{pH}$ of the solution.

315030 A weak acid HA has degree of dissociation $x$. Thus $\left(\text{pH - p}{\text{K}}_{\text{a}}\right)\text{is}$