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question_answer1) The equivalent conductances of sodium chloride, hydrochloric acid and sodium acetate at infinite dilution are 126.45, 426.16 and \[91.0\text{ }oh{{m}^{-1}}\text{ }c{{m}^{2}}\text{ }equi{{v}^{-1}}\], respectively at\[25{}^\circ C\]. Calculate the equivalent conductance of acetic acid at infinite dilution.
question_answer2) 2F of electricity is passed through 20 L of a solution of aqueous solution of KCl. Calculate the pH of the solution.
question_answer3) The specific conductivity of a solution containing 1.0g of anhydrous \[BaC{{l}_{2}}\] in 200 \[c{{m}^{3}}\] of the solution has been found to be\[0.0058\text{ }S\text{ }c{{m}^{-\,1}}\]. Calculate the molar conductivity of the solution. (Molecular wt. of\[BaC{{l}_{2}}=208\]).
question_answer4) The equivalent conductivities of acetic acid at 298 K at the concentrations of 0.1 M and 0.001 M are 5.20 and \[49.2\text{ }S\text{ }c{{m}^{2}}\,e{{q}^{-1}}\] respectively. Calculate the degree of dissociation of acetic acid at 0.001 M concentration. Given that: \[{{\wedge }^{\infty }}({{H}^{+}})\] and \[{{\wedge }^{\infty }}(C{{H}_{3}}CO{{O}^{-}})\] are 349.8 and \[40.9\text{ }oh{{m}^{-1}}\text{ }c{{m}^{2}}\text{ }e{{q}^{-1}}\]respectively.
question_answer5) The amount of electricity which releases 2.0 g of gold from a gold salt is same as that which dissolves 0.967g of copper anode during the electrolysis of copper sulphate solution. What is the oxidation number of gold in the gold ion? (At. mass of Cu = 63.5; Au = 197)
question_answer6) If \[{{K}_{c}}\] for the reaction \[C{{u}^{2+}}(aq)+S{{n}^{2+}}(aq)\xrightarrow{{}}\,S{{n}^{4+}}(aq)+Cu(s)\] at \[25{}^\circ C\] is represented as \[2.6\times {{10}^{y}}\] then find the value of y. (Given: \[E{{{}^\circ }_{C{{u}^{2+}}\left| Cu \right.}}=0.34V;\,\,E_{S{{n}^{4+}}\left| S{{n}^{2+}} \right.}^{{}^\circ }=0.15V\])
question_answer7) If \[\Delta G{}^\circ \] for the half cell \[MnO_{4}^{-}|Mn{{O}_{2}}\] in an acid solution is xF then find the value of x. \[(Given:\,\,E{{{}^\circ }_{MnO_{4}^{-}|M{{n}^{2+}}}}=1.5V;\,E{{{}^\circ }_{Mn{{O}_{2}}|M{{n}^{2+}}}}=1.25V)\]
question_answer8) The standard reduction potential of a silver chloride electrode (metal-sparingly soluble salt electrode) is 0.209 V and for silver electrode is 0.80 V. If the moles of AgCl that can dissolve in 10 L of a 0.01 M NaCl solution is represented as \[{{10}^{-Z}}\] then find the value of Z.
question_answer9) Molar conductivity of aqueous solution of HA is \[200\text{ }S\text{ }c{{m}^{2}}\text{ }mo{{l}^{-1}}\], pH of this solution is 4. Calculate the value of \[p{{K}_{a}}(HA)\] at \[25{}^\circ C\]. \[Given:\,\wedge _{M}^{\infty }(NaA)\,100\,Sc{{m}^{2}}\,mo{{l}^{-1}};\,\wedge _{M}^{\infty }(HCl)\] \[=425\,\,Sc{{m}^{2}}\,mo{{l}^{-1}};\] \[\wedge _{M}^{\infty }\,(NaCl)=125\,Sc{{m}^{2}}\,mo{{l}^{-1}}\]
question_answer10) A solution containing \[1M\text{ }XS{{O}_{4}}\] (aq) and \[1M\,YS{{O}_{4}}\] (aq) is electrolysed. If cone. of \[{{X}^{2+}}\] is \[{{10}^{-z}}M\] when deposition of \[{{Y}^{2+}}\]and \[{{X}^{2+}}\] starts simultaneously, calculate the value of Z. Given: \[\frac{2.\,303RT}{F}=0.06\] \[E{{{}^\circ }_{{{X}^{2+}}/X}}=-\,0.12V;\,\,E{{{}^\circ }_{{{Y}^{2+}}/Y}}=-\,0.24\,V\]
question_answer11) A solution of \[Ni\,{{(N{{O}_{3}})}_{2}}\]is electrolysed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?
question_answer12) Find the standard Gibbs energy for the given cell reaction in \[kJ\text{ }mo{{l}^{-1}}\] at 298 K \[Zn\,(s)+C{{u}^{2+}}(aq)\xrightarrow{{}}Z{{n}^{2+}}(aq)+Cu(s),\] \[E{}^\circ =2\,V\] at 298 K (Faraday's constant, \[F=96000\text{ }C\text{ }mo{{l}^{-1}}\])
question_answer13) All the energy released from the reaction \[X\to Y,{{\Delta }_{r}}G{}^\circ =-\,193\,kJ\,mol{{~}^{-1}}\] is used for oxidizing \[{{M}^{+}}\] as \[{{M}^{+}}\to {{M}^{3+}}2{{e}^{-}},E{}^\circ =-\,0.25V\] Under standard conditions, find the number of moles of \[{{M}^{+}}\] oxidized when one mole of X is converted to Y \[[F=96500\text{ }C\text{ }mo{{l}^{\,-\,1}}]\]
question_answer14) Consider the following half-cell reactions and associated standard half-cell potentials, and determine the maximum voltage that can be obtained by combination resulting in spontaneous processes : \[AuBr_{4}^{-}\,(aq)+3{{e}^{-}}\xrightarrow{{}}Au(s)+4B{{r}^{-}}(aq);\,E{}^\circ =-\,0.86\,V\] \[E{{u}^{3+}}(aq)\,+\,{{e}^{~-}}\xrightarrow{{}}E{{u}^{2+}}\,(aq);\,\,E{}^\circ \,=-\,0.43\,V\] \[S{{n}^{2+}}(aq)\,+2\,{{e}^{~-}}\xrightarrow{{}}Sn\,(s);\,\,E{}^\circ \,=-\,0.14\,V\] \[I{{O}^{-}}(aq)+{{H}_{2}}O\,(l)+2{{e}^{-}}\xrightarrow{{}}{{I}^{-}}(aq)+2O{{H}^{-}}\,(aq);\] \[E{}^\circ =+0.49\,V\]
question_answer15) The e.m.f. of the cell \[Zn|Z{{n}^{2+}}(0.01M)\,|\] \[\left| F{{e}^{2+}}(0.001M) \right|\] at 298 K is 0.2905 then the value of equilibrium constant for the cell reaction\[{{10}^{x}}\]. Find x.
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