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The tendency of $BF_3$, $BCl_3$ and $BBr_3$ to behave as Lewis acid decreases in the sequence:
The end product in the below-mentioned reaction is: $\text{H}_3\text{C-Br} \xrightarrow{\text{KCN}} \text{A} \xrightarrow{\text{H}_3\text{O}^+} \text{B} \xrightarrow{\text{LiAlH}_4\text{, Ether}} \text{C}$
Molar conductivities ($\Lambda^{\circ}_m$) at infinite dilution of $NaCl$, $HCl$, and $CH_3COONa$ are $126.4$, $425.9$, and $91.0\text{ S cm}^2\text{ mol}^{-1}$ respectively. $\Lambda^{\circ}_m$ for $CH_3COOH$ will be:
The weight of silver (atomic weight = $108$) displaced by a quantity of electricity which displaces $5600 \text{ mL}$ of $\text{O}_2$ at STP will be :
A compound $\text{BA}_2$ has $K_{sp} = 4 \times 10^{-12}$. Solubility of this compound will be:
Predict the order of reactivity of the following four isomers towards $\text{S}_\text{N}2$ reaction. (I) $\text{CH}_3\text{CH}_2\text{CH}_2\text{CH}_2\text{Cl}$ (II) $\text{CH}_3\text{CH}_2\text{CH}(\text{Cl})\text{CH}_3$ (III) $(\text{CH}_3)_2\text{CHCH}_2\text{Cl}$ (IV) $(\text{CH}_3)_3\text{CCl}$
Aqueous solution of which of the following compounds is the best conductor of electric current?
What is the molarity of the saturated solution if the solubility product for a salt of type AB is $4 \times 10^{-8}$?
In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains $\text{Ag}^+$ and $\text{Pb}^{2+}$ at a concentration of $0.10 \text{ M}$. Aqueous $\text{HCl}$ is added to this solution until the $\text{Cl}^-$ concentration is $0.10 \text{ M}$. What will the concentration of $\text{Ag}^+$ and $\text{Pb}^{2+}$ at equilibrium? ($K_{sp}$ for $\text{AgCl} = 1.8 \times 10^{-10}$, $K_{sp}$ for $\text{PbCl}_2 = 1.7 \times 10^{-5}$)
The correct expression that represents the equivalent conductance at infinite dilution of $Al_2(SO_4)_3$ is: (Given that $\Lambda^{\circ}_{Al^{3+}}$ and $\Lambda^{\circ}_{SO_4^{2-}}$ are the equivalent conductances at infinite dilution of the respective ions)
The value of equilibrium constant of the reaction $HI(g) \rightleftharpoons \frac{1}{2} H_2(g) + \frac{1}{2} I_2(g)$ is $8.0$. The equilibrium constant of the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$ will be:
For the reaction $2\text{A} \rightleftharpoons \text{B} + \text{C}$; $K_c = 4 \times 10^{-3}$. At a given time, the composition of the reaction mixture is: $[\text{A}] = [\text{B}] = [\text{C}] = 2 \times 10^{-3}\text{ M}$. In light of the above facts, which of the following is correct?
Given below is a reaction sequence: $\text{CH}_3\text{CH}_2\text{Cl} \xrightarrow{\text{NaCN}} X \xrightarrow{\text{H}_2/\text{Ni}} Y \xrightarrow{\text{Acetic Anhydride}} Z$ The product '$Z$' in the above reaction is:
Match the redox conversions in List-I with the corresponding number of Faradays required in List-II. **List-I (Redox Conversion)** A. $1\text{ mol}$ of $\text{H}_2\text{O}$ to $\text{O}_2$ B. $1\text{ mol}$ of $\text{MnO}_4^-$ to $\text{Mn}^{2+}$ C. $1.5\text{ mol}$ of $\text{Ca}$ from molten $\text{CaCl}_2$ D. $1\text{ mol}$ of $\text{FeO}$ to $\text{Fe}_2\text{O}_3$ **List-II (Number of Faraday required)** I. $3\text{F}$ II. $2\text{F}$ III. $1\text{F}$ IV. $5\text{F}$
The molar solubility of $\text{CaF}_2$ ($K_{sp} = 5.3 \times 10^{-11}$) in $0.1\text{ M}$ solution of NaF will be:
Which of the following statements is correct for a reversible process in a state of equilibrium?
A compound, among the following, that cannot be classified as a protonic acid is:
At $25^\circ\text{C}$, molar conductance of $0.1 \text{ molar}$ aqueous solution of ammonium hydroxide is $9.54 \text{ ohm}^{-1}\text{cm}^2\text{mol}^{-1}$ and at infinite dilution, its molar conductance is $238 \text{ ohm}^{-1}\text{cm}^2 \text{mol}^{-1}$. The degree of ionization of ammonium hydroxide at the same concentration and temperature is:
Given that the equilibrium constant for the reaction $2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)$ has a value of $278$ at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be: $\text{SO}_3(g) \rightleftharpoons \text{SO}_2(g) + \frac{1}{2} \text{O}_2(g)$
The dipole moment of compound AB is 10.92 D and that of compound CD is 12.45 D. If the bond length of AB is 2.72 $\text{\AA}$ and that of CD is 2.56 $\text{\AA}$, then for these compounds the correct statement is: