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, \(\mathrm{pH}=\dfrac{1}{2} \mathrm{pK}_{\mathrm{a}}\).
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, \(\mathrm{pH}=\dfrac{1}{2} \mathrm{pK}_{\mathrm{a}}\).
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, \(\mathrm{pH}=\dfrac{1}{2} \mathrm{pK}_{\mathrm{a}}\).
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, \(\mathrm{pH}=\dfrac{1}{2} \mathrm{pK}_{\mathrm{a}}\).
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, \(\mathrm{pH}=\dfrac{1}{2} \mathrm{pK}_{\mathrm{a}}\).
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 \(\left( {{\text{pH - p}}{{\text{K}}_{\text{a}}}} \right){\text{is}}\)