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The molar conductance of a solution, given its conductivity ($0.248\text{ S m}^{–1}$) and concentration ($0.2\text{ mol m}^{–3}$) is:
Among the following pairs of solutions, the one which is not an acidic buffer is:
A button cell used in watches functions as following: $\text{Zn}(s) + \text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) \rightleftharpoons 2\text{Ag}(s) + \text{Zn}^{2+}(aq) + 2\text{OH}^-(aq)$ If half cell potentials are: $\text{Zn}^{2+}(aq) + 2e^- \rightarrow \text{Zn}(s); E^\circ = -0.76 \text{ V}$ $\text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) + 2e^- \rightarrow 2\text{Ag}(s) + 2\text{OH}^-(aq); E^\circ = 0.34 \text{ V}$ The cell potential will be:
Kohlrausch's law states that at
The standard Emf of a galvanic cell involving cell reaction with $n = 2$ is found to be $0.295\text{ V}$ at $25^{\circ}\text{C}$. The equilibrium constant of the reaction would be: (Given $F = 96500\text{ C mol}^{-1}$; $R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$)
Given the reaction: $\text{Cu}(s) + 2\text{Ag}^+(aq) \rightarrow \text{Cu}^{2+}(aq) + 2\text{Ag}(s)$ with $E^\circ = 0.46 \text{ V}$ at $298 \text{ K}$, what is the equilibrium constant for the reaction?
On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:
Which one of the following molecular hydrides acts as a Lewis acid?
The molar conductivity of $0.007\text{ M}$ acetic acid is $20\text{ S cm}^2\text{ mol}^{-1}$. The dissociation constant of acetic acid is: ($\Lambda^o_{H^+} = 350\text{ S cm}^2\text{ mol}^{-1}$ and $\Lambda^o_{CH_3COO^-} = 50\text{ S cm}^2\text{ mol}^{-1}$)
The molar conductivity of a $0.5 \text{ mol/dm}^3$ solution of $\text{AgNO}_3$ with electrolytic conductivity of $5.76 \times 10^{-3} \text{ S cm}^{-1}$ at $298 \text{ K}$ is:
Standard electrode potential for the cell with cell reaction $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$ is $1.1\text{ V}$. Calculate the standard Gibbs energy change for the cell reaction. (Given $F = 96487\text{ C mol}^{–1}$)
Given below are two statements: Assertion (A): In the equation, $\Delta_rG = -nFE_{cell}$, value of $\Delta_rG$ depends on $n$. Reason (R): $E_{cell}$ is an intensive property and $\Delta_rG$ is an extensive property.
Mass in grams of copper deposited by passing $9.6487\text{ A}$ current through a voltmeter containing copper sulphate for $100\text{ seconds}$ is (Given: Molar mass of Cu: $63\text{ g mol}^{-1}$, $1\text{ F} = 96487\text{ C mol}^{-1}$)
Among the following, the one that is not a green house gas is
Given that the ionic product of $\text{Ni(OH)}_2$ is $2 \times 10^{-15}$. The solubility of $\text{Ni(OH)}_2$ in $0.1\text{ M}$ NaOH is:
The concentration of the $Ag^+$ ions in a saturated solution of $Ag_2C_2O_4$ is $2.2 \times 10^{-4}\text{ M}$. The solubility product of $Ag_2C_2O_4$ is:
The percentage of pyridine ($C_5H_5N$) that forms pyridinium ion ($C_5H_5NH^+$) in a 0.10 M aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is:
The $K_{sp}$ of $Ag_2CrO_4$, $AgCl$, $AgBr$ and $AgI$ are, respectively, $1.1 \times 10^{-12}$, $1.8 \times 10^{-10}$, $5.0 \times 10^{-13}$, and $8.3 \times 10^{-17}$. The salt that precipitates last if $AgNO_3$ solution is added to the solution containing equal moles of $NaCl$, $NaBr$, $NaI$ and $Na_2CrO_4$ is:
The molecule that is least likely to behave as Lewis base is:
For the reversible reaction, $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{Heat}$, the equilibrium shifts in the forward direction: