Molar conductance of a 1.5 M solution of an electrolyte is found to be \[138.9\text{ }S\text{ }c{{m}^{2}}\]. The specific conductance of this solution is
Equivalent conductivity of \[BaC{{l}_{2}},{{H}_{2}}S{{O}_{4}}\] and HCl are \[{{y}_{1}},{{y}_{2}}\] and \[{{y}_{3}}S\,c{{m}^{-1}}e{{q}^{-1}}\] at infinite dilution. If conductivity of saturated \[BaS{{O}_{4}}\] solution is \[y\,S\,c{{m}^{-1}},\] then find \[{{K}_{sp}}\] of \[BaS{{O}_{4}}\].
A current of 2.0 A when passed for 5 hours through a molten metal salt deposits 22.2 g of metal of atomic weight 177. The oxidation state of the metal in the metal salt is
A current of 0.250 A is passed through 400 mL of a 2, 0 M solution of NaCl for 35 minutes. What will be the pH of the solution after the current is turned off?
Equivalent conductance of saturated \[BaS{{O}_{4}}\] is \[400\,{{\Omega }^{-1}}\,c{{m}^{2}}eq{{u}^{-1}}\] and specific conductance is\[8\times {{10}^{-5}}\,{{\Omega }^{-1}}\,c{{m}^{-1}}\]. Hence, \[{{K}_{sp}}\] of \[BaS{{O}_{4}}\] is
On electrolyzing the molten chloride of metal \[725\text{ }ml\] of \[C{{l}_{2}}\] liberated at \[25{}^\circ C\] and 740 mm Hg pressure at anode for every one gm of metal deposite at cathode. The formula of metal chloride is (GAM of metal \[=52.01\])
The standard electrode potential for the following reaction is + 1.33 V. What is the potential at pH = 2? \[C{{r}_{2}}O_{7}^{2-}(aq1M)+14{{H}^{\oplus }}(aq)+6{{e}^{-}}\]\[\xrightarrow{\,}\,2C{{r}^{3+}}(aq1M)+7{{H}_{2}}O(l)\]
Molar conductance's of \[BaC{{l}_{2}},{{H}_{2}}S{{O}_{4}}\] and HCl at infinite dilutions are \[{{x}_{1}},{{x}_{2}}\] and \[{{x}_{3}}\] respectively. Equivalent conductance of \[BaS{{O}_{4}}\] at infinite dilution will be:
The resistance of 0.1N acetic acid when measured in a cell with cell constant \[1.5\,c{{m}^{-1}}\] is \[5.250\,\Omega \]. The value of \[{{\lambda }_{eq}}\] of \[0.1\,N\,AcOH\] is
Given the following molar conductivities at \[{{250}^{o}}C;HCl,425\,{{\Omega }^{-1}}c{{m}^{2}}mo{{l}^{-1}};\]\[NaCl\,\,125{{\Omega }^{-1}}\]\[c{{m}^{2}}mo{{l}^{-1}}\]NaC (sodium crotonate), \[82\,{{\Omega }^{-1}}c{{m}^{2}}mo{{l}^{-1}};\] what is the ionisation constant of crotonic acid? If the conductivity of a 0.001 M crotonic acid solution is \[3.82\times {{10}^{-4}}{{\Omega }^{-1}}c{{m}^{-1}}\]?
3F of electricity passes through three electrolytic cells connected in series containing \[A{{g}^{+}},C{{a}^{2+}}\] and \[A{{l}^{3+}}\] ions, respectively. The molar ratio in which the three metal ions are liberated at the electrodes is
Salts of A (atomic weight: 7), B (atomic weight: 27), and C (atomic weight: 48) were electrolyzed under identical condition using the same quantity of electricity. It was found that when 2.1 got A was deposited, the weights of B and C deposited were 2.7 and 7.2 g, respectively. The valencies of A, B and C, respectively are:
The current efficiency of the process is 80%. What volume of gases would be produced at \[\text{27}{}^\circ \text{C}\] and 740 torr, if the current of 0.5 A is passed through the solution for 96.45 min?
A hydrogen electrode placed in a buffer solution of \[C{{H}_{3}}COONa\] and acetic acid in the ratio x : y and y : x has electrode potential value \[{{E}_{1}}\] volts and \[{{E}_{2}}\] volts, respectively at \[\text{25}{}^\circ \text{C}\]. The \[p{{K}_{a}}\] value of acetic acid is (\[{{E}_{1}}\] and \[{{E}_{2}}\] are oxidation potential):
Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100 ohm. The conductivity of this solution is 1.29 S/m. Resistance of the same cell filled with 0.02 M of the same solution if the electrolyte is 520 ohm. The molar conductivity of 0.02 M solution of electrolyte would be:
The standard electrode potential for the following reaction is +1.33V. What is the potential at \[pH=2.0\]? \[C{{r}_{2}}{{O}_{7}}^{2-}(aq.1M)+14\,{{H}^{+}}(aq)+6{{e}^{-}}\xrightarrow{{}}\] \[2C{{r}^{3+}}(aq.\,1\,M)+7{{H}_{2}}O(\ell )\]
Zn-Hg is prepared by electrolysis of aqueous \[ZnC{{l}_{2}}\] using Hg cathode (9g). How much current is to be passed through \[ZnC{{l}_{2}}\] solution for 1000 s to prepare a Zn-Hg with 25% Zn by weight (Zn = 65.4):
For the cell \[Pt|{{H}_{2}}(g)|\] solution \[X||KCI\] (saturated) \[|H{{g}_{2}}C{{l}_{2}}|Hg|\,Pt\] the observed EMF at \[25{}^\circ C\] was \[600\text{ }mV.\] When solution X was replaced by a standard phosphate buffer with \[pH=7.00,\] the EMF was \[777\text{ }mV\]. Find the pH of solution X.
The same quantity of electricity was passed through two electrolytic cells containing a salt of metal X and zinc sulphate solution respectively using platinum electrode. 0.468 g of metal X and 1.532 g of Zn were deposited. The equivalent mass of X is (At. wt. of Zn is 65.4 u)
The standard EMF of a cell having one electron change is found to be 0.591 V at \[\text{25}{}^\circ \text{C}\]. The equilibrium constant of the reaction is: