314493
Read statement-A and statement-B carefully to mark the correct options given below.
Statement A :
: A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities.
Statement B :
:Blood is naturally occurring buffer solution whose pH is maintained by
\({\mathrm{\mathrm{\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}}}}\)concentrations.
314494
When \(\mathrm{CO}_{2}\) is bubbled in excess of water, the following equilibrium is established.
\({\text{C}}{{\text{O}}_2} + 2{{\text{H}}_2}{\text{O}} \rightleftharpoons {{\text{H}}_3}{{\text{O}}^ + } + {\text{HCO}}_2^ - {\text{ ;}}\)
\({{\text{K}}_{\text{a}}}{\mkern 1mu} = {\text{3}}.{\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 7}}}},{\text{pH = 6}}\)
What would be the value of \(\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}\) ?
314496
Statement A :
Buffer system of carbonic acid and sodium bicarbonate is used for the precipitation of hydroxides of third group basic radicals.
Statement B :
Buffer system of carbonic acid and sodium bicarbonate maitains the \(\mathrm{pH}\) of blood to a constant value about 7.4.
314493
Read statement-A and statement-B carefully to mark the correct options given below.
Statement A :
: A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities.
Statement B :
:Blood is naturally occurring buffer solution whose pH is maintained by
\({\mathrm{\mathrm{\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}}}}\)concentrations.
314494
When \(\mathrm{CO}_{2}\) is bubbled in excess of water, the following equilibrium is established.
\({\text{C}}{{\text{O}}_2} + 2{{\text{H}}_2}{\text{O}} \rightleftharpoons {{\text{H}}_3}{{\text{O}}^ + } + {\text{HCO}}_2^ - {\text{ ;}}\)
\({{\text{K}}_{\text{a}}}{\mkern 1mu} = {\text{3}}.{\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 7}}}},{\text{pH = 6}}\)
What would be the value of \(\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}\) ?
314496
Statement A :
Buffer system of carbonic acid and sodium bicarbonate is used for the precipitation of hydroxides of third group basic radicals.
Statement B :
Buffer system of carbonic acid and sodium bicarbonate maitains the \(\mathrm{pH}\) of blood to a constant value about 7.4.
314493
Read statement-A and statement-B carefully to mark the correct options given below.
Statement A :
: A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities.
Statement B :
:Blood is naturally occurring buffer solution whose pH is maintained by
\({\mathrm{\mathrm{\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}}}}\)concentrations.
314494
When \(\mathrm{CO}_{2}\) is bubbled in excess of water, the following equilibrium is established.
\({\text{C}}{{\text{O}}_2} + 2{{\text{H}}_2}{\text{O}} \rightleftharpoons {{\text{H}}_3}{{\text{O}}^ + } + {\text{HCO}}_2^ - {\text{ ;}}\)
\({{\text{K}}_{\text{a}}}{\mkern 1mu} = {\text{3}}.{\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 7}}}},{\text{pH = 6}}\)
What would be the value of \(\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}\) ?
314496
Statement A :
Buffer system of carbonic acid and sodium bicarbonate is used for the precipitation of hydroxides of third group basic radicals.
Statement B :
Buffer system of carbonic acid and sodium bicarbonate maitains the \(\mathrm{pH}\) of blood to a constant value about 7.4.
314493
Read statement-A and statement-B carefully to mark the correct options given below.
Statement A :
: A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities.
Statement B :
:Blood is naturally occurring buffer solution whose pH is maintained by
\({\mathrm{\mathrm{\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}}}}\)concentrations.
314494
When \(\mathrm{CO}_{2}\) is bubbled in excess of water, the following equilibrium is established.
\({\text{C}}{{\text{O}}_2} + 2{{\text{H}}_2}{\text{O}} \rightleftharpoons {{\text{H}}_3}{{\text{O}}^ + } + {\text{HCO}}_2^ - {\text{ ;}}\)
\({{\text{K}}_{\text{a}}}{\mkern 1mu} = {\text{3}}.{\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 7}}}},{\text{pH = 6}}\)
What would be the value of \(\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}\) ?
314496
Statement A :
Buffer system of carbonic acid and sodium bicarbonate is used for the precipitation of hydroxides of third group basic radicals.
Statement B :
Buffer system of carbonic acid and sodium bicarbonate maitains the \(\mathrm{pH}\) of blood to a constant value about 7.4.
314493
Read statement-A and statement-B carefully to mark the correct options given below.
Statement A :
: A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities.
Statement B :
:Blood is naturally occurring buffer solution whose pH is maintained by
\({\mathrm{\mathrm{\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}}}}\)concentrations.
314494
When \(\mathrm{CO}_{2}\) is bubbled in excess of water, the following equilibrium is established.
\({\text{C}}{{\text{O}}_2} + 2{{\text{H}}_2}{\text{O}} \rightleftharpoons {{\text{H}}_3}{{\text{O}}^ + } + {\text{HCO}}_2^ - {\text{ ;}}\)
\({{\text{K}}_{\text{a}}}{\mkern 1mu} = {\text{3}}.{\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 7}}}},{\text{pH = 6}}\)
What would be the value of \(\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}\) ?
314496
Statement A :
Buffer system of carbonic acid and sodium bicarbonate is used for the precipitation of hydroxides of third group basic radicals.
Statement B :
Buffer system of carbonic acid and sodium bicarbonate maitains the \(\mathrm{pH}\) of blood to a constant value about 7.4.