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The solubility of AgCl(s) with solubility product $1.6 \times 10^{-10}$ in 0.1 M NaCl solution would be?
For a reaction, $\text{BaO}_2(s) \rightleftharpoons \text{BaO}(s) + \text{O}_2(g)$; $\Delta H = +\text{ve}$. At equilibrium condition, the pressure of $\text{O}_2$ depends on the:
If a solution of $0.1 \text{ N NH}_4\text{OH}$ and $0.1 \text{ N NH}_4\text{Cl}$ has $\text{pH } 9.25$, then $pK_b$ of $\text{NH}_4\text{OH}$ is:
A compound, among the following, that cannot be classified as a protonic acid is:
The $\text{p}K_b$ of dimethylamine and $\text{p}K_a$ of acetic acid are $3.27$ and $4.77$ respectively at $T\text{ (K)}$. The correct option for the pH of dimethylammonium acetate solution is:
The following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations. pH of which one of them will be equal to 1?
Among the following, the correct order of acidity is:
Consider the nitration of benzene using mixed conc. $H_2SO_4$ and $HNO_3$. If a large amount of $KHSO_4$ is added to the mixture, the rate of nitration will be:
The value of the equilibrium constant for a particular reaction is $1.6 \times 10^{12}$. When the system is in equilibrium, it will include:
For the reversible reaction: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat}$. The equilibrium shifts in a forward direction:
Which of these is least likely to act as a Lewis base?
Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?
The equilibrium reaction that doesn't have equal values for $K_c$ and $K_p$ is:
The tendency of $BF_3$, $BCl_3$ and $BBr_3$ to behave as Lewis acid decreases in the sequence:
Which of the following molecules acts as a Lewis acid?
The pH of the solution containing $50\text{ mL}$ each of $0.10\text{ M}$ sodium acetate and $0.01\text{ M}$ acetic acid is: [Given $\text{p}K_a$ of $\text{CH}_3\text{COOH} = 4.57$]
The following equilibrium constants are given: $N_2 + 3H_2 \rightleftharpoons 2NH_3$; $K_1$ $N_2 + O_2 \rightleftharpoons 2NO$; $K_2$ $H_2 + \frac{1}{2}O_2 \rightleftharpoons H_2O$; $K_3$ The equilibrium constant for the oxidation of $NH_3$ by oxygen to give NO is:
The following pair constitutes a buffer is:
Which composition will make the basic buffer?
The incorrect statement regarding the lanthanons is: