How many mole of ${\rm{HCl}}$ are required to prepare one litre of buffer solution (containing ${\rm{NaCN}} + {\rm{HCl}}$) of ${\rm{pH}}\;{\rm{ = }}\;8.5$ using $0.01\;g$ formula weight of ${\rm{NaCN}}\left( {{K_{{\rm{HCN}}}} = 4.1 \times {{10}^{ - 10}}} \right)$?

NEET UG CHEMISTRY MCQ: Equilibrium

1 Hard

1 of 1

Application +4 | -1

How many mole of

\mathrm{HCl}

are required to prepare one litre of buffer solution (containing

\mathrm{NaCN} + \mathrm{HCl}

) of

\mathrm{pH}\;\mathrm{ = }\;8.5

using

0.01\;g

formula weight of

\mathrm{NaCN}\left( {{K_{\mathrm{HCN}}} = 4.1 \times {{10}^{ - 10}}} \right)

View answer and explanation

Correct option: A

8.85 \times {10^{ - 3}}

Option A (

8.85 \times {10^{ - 3}}

) is correct because it represents the moles of HCl required to create the buffer solution with the specified pH, considering the equilibrium between HCN and CN-.

More Questions from Equilibrium

Practice All Chapter MCQs →

Given below are two statements: One is labelled as Assertion A and the other labelled as Reason R.
Assertion A: During the boiling of water having temporary hardness,

Mg{(HC{O_3})_2}

is converted to

MgC{O_3}

.
Reason R The solubility product of

Mg{(OH)_2}

is greater than that of

MgC{O_3}

.
In the light of the above statements, choose the most appropriate answer from the options given below At a certain temperature,

K_{\mathrm{P}}

for the dissociation of solid

\mathrm{CaCO}_3

4.5 \times 10^{-2}

atm and for the reaction

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}),

the

K_{\mathrm{P}}

value is

2.0 \mathrm{~atm}.

The pressure of carbon monoxide at this temperature, when solid carbon

\mathrm{CaO}

and

\mathrm{CaCO}_3

are mixed together and allowed to attain equilibrium is Phenolphthalein shows … in acid medium. At the state of dynamic equilibrium, for solute

+

solvent

\leftrightharpoons

solution. For

\mathrm{PC}{\mathrm{l}_5}\leftrightharpoons\mathrm{PC}{\mathrm{l}_3} + \mathrm{C}{\mathrm{l}_2}

, initial concentration of each reactant and product is 1 M. If

{K_{\mathrm{eq}}} = 0.41

then Select the

\mathrm{p}{K_a}

value of the strongest acid from the following