For the reversible reaction $\newline N_2 (g) + 3H_2 (g) \rightleftharpoons 2NH_3 (g) +$Heat$\newline$the equilibrium shifts in forward direction

For a given exothermic reaction, $K_p$ and $K_p'$ are the equilibrium constants at temperatures $T_1$ and $T_2$ respectively. Assuming that heat of reaction is constant in temperatures range between $T_1$ and $T_2$, it is readily observed that

Acidity of diprotic acids in aqueous solutions increases in the order

Artificial sweetener which is stable under cold conditions only is

Which of the following will not be soluble in sodium hydrogen carbonate?

The K$_{sp}$ of Ag$_2$CrO$_4,$AgCl, AgBr, and AgI are respectively, $1.1 \times 10^{-12}, 1.8 \times 10^{-10}, 5.0 \times 10^{-13}$ and $8.3 \times 10^{-17}.$Which one of the following salts will precipitate last if AgNO$_3$ solution is added to the solution containing equal moles of NaCl, NaBr, NaI, and Na$_2$CrO$_4?$

Which one of the following electrolytes has the same value of van’t Hoff’s factor (i) as that of $Al_2(SO_4)_3$ if all are 100$\%$ ionized?

If the value of an equilibrium constant for a particular reaction is $1.6 \times 10^{12},$ then at equilibrium the system will contain

Which of the following statements about hydrogen is incorrect?

$MY$ and $NY_3,$ two nearly insoluble salts, have the same Ksp values of $6.2 \times 10^{-13}$ at room temperature. Which statement is true regarding their solubilities?

The pressure of H$_2$ required to make the potential of a hydrogen electrode zero in pure water at $298$ K is (in atm).

The equilibrium constants of the following are$\\ \begin{array}{c} N_2 + 3H_2 \rightleftharpoons 2NH_3 \quad K_1 \\ N_2 + O_2 \rightleftharpoons 2NO \quad K_2 \\ H_2 + \frac{1}{2} O_2 \rightleftharpoons H_2O \quad K_3 \end{array} \\$The equilibrium constant $(K)$ of the reaction$\\ 2NH_3 + \frac{5}{2} O_2 \xrightleftharpoons{K} 2NO + 3H_2O$ will be

Which one of the following statements is not correct?

A 20 L container at 400 K contains CO$_2$(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO$_2$ attains its maximum value, will be:$\\$(Given that: SrCO$_3$(s)$\rightleftharpoons$ SrO(s) + CO$_2$(g), $K_p = 1.6$ atm)

Concentration of the Ag$^+$ ions in a saturated solution of Ag$_2$C$_2$O$_4$ is $2.2 \times 10^{-4}$ mol L$^{-1}.$ Solubility product of Ag$_2$C$_2$O$_4$ is

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations:$\\$a. $60$ mL $\frac{M}{10}$ HCl $+ 40$ mL $\frac{M}{10}$ NaOH$\\$b. $55$ mL $\frac{M}{10}$ HCl $+ 45$ mL $\frac{M}{10}$ NaOH$\\$c. $75$ mL $\frac{M}{5}$ HCl $+ 25$ mL $\frac{M}{5}$ NaOH$\\$d. $100$ mL $\frac{M}{10}$ HCl $+ 100$ mL $\frac{M}{10}$ NaOH$\\$pH of which one of them will be equal to 1?

On which of the following properties does the coagulating power of an ion depend?

The solubility of BaSO$_4$ in water is $2.42 \times 10^{-3}$ g/L at 298 K. The value of its solubility product (K$_{sp})$ will be$\\$(Given molar mass of BaSO$_4 = 233$ g/mol)

Which one of the following conditions will favor maximum formation of the product in the reaction,$\\$A$_2(g) +$B$_2(g) \rightleftharpoons$X$_2(g), \Delta_r H = -X$ kJ$?$

The pH of a saturated solution of $Ca(OH)_2$ is $9.$ The solubility product $(K_{sp})$ of $Ca(OH)_2$ is:

Conjugate base for Bronsted acids $H_2O$ and $HF$ are:

Which mixture of the solutions will lead to the formation of negatively charged colloidal $[AgI] I^-$ sol.?

Which will make a basic buffer?

Which of the following is an amphoteric hydroxide?

The method used to remove temporary hardness of water is:

Find out the solubility of Ni(OH)$_2$ in 0.1 M NaOH. Given that the ionic product of Ni(OH)$_2$ is $2 \times 10^{-15}.$

A mixture of $N_2$ and Ar gases in a cylinder contains 7 g of $N_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of $N_2$ is:$\\$[Use atomic masses (in g mol$^{-1}$): $N=14, Ar=40]$

HCl was passed through a solution of CaCl$_2$, MgCl$_2$ and NaCl. Which of the following compound(s) crystallise(s)?

Statement I: Acid strength increases in the order given as$\newline HF << HCl << HBr << HI. \newline$Statement II: As the size of the elements F, Cl, Br, I increases down the group, the bond strength of HF, HCl, HBr, and HI decreases and so the acid strength increases.$\newline$In the light of the above statements, choose the correct answer from the options given below.

The pK$_b$ of dimethylamine and pK$_a$ of acetic acid are $3.27$ and $4.77$ respectively at T (K). The correct option for the pH of dimethylammonium acetate solution is:

Choose the correct option for graphical representation of Boyle’s law, which shows a graph of pressure vs. volume of a gas at different temperatures:

The pH of the solution containing $50$ mL each of $0.10 M$ sodium acetate and $0.01 M$ acetic acid is$\\$(Given $pK_a$ of $CH_3COOH = 4.57)$

What mass of $95\%$ pure $CaCO_3$ will be required to neutralize $50$ mL of $0.5 M$ HCl solution according to the following reaction?$\\ CaCO_3 (s) + 2HCl (aq) \rightarrow CaCl_2 (aq) + CO_2 (g) + 2H_2O (l)$

Statement I: In the coagulation of a negative sol, the flocculating power of the three given ions is in the order $Al^{3+} > Ba^{2+} > Na^+. \\$Statement II: In the coagulation of a positive sol, the flocculating power of the three given salts is in the order $NaCl > Na_2SO_4 > Na_3PO_4. \\$Choose the most appropriate answer from the options given below:

$3O_2(g) \rightleftharpoons 2O_3(g)$. For the above reaction at $298$ K, $K_c$ is found to be $3.0 \times 10^{-59}$. If the concentration of $O_2$ at equilibrium is $0.040$ M, then the concentration of $O_3$ in M is:

In Lassaigne’s extract of an organic compound, both nitrogen and sulphur are present, which gives blood red colour with $Fe^{2+}$ due to the formation of -

Which amongst the following options is correct graphical representation of Boyle’s Law?

The equilibrium concentrations of the species in the reaction A + B $\rightleftharpoons$ C + D are 2, 3, 10 and 6 mol L$^{-1}$, respectively at 300 K. $\Delta G^{\circ}$ for the reaction is (R = 2 cal/mol K)

Given below are two statements:$\\$Statement-I: The nutrient deficient water bodies lead to eutrophication.$\\$Statement-II: Eutrophication leads to decrease in the level of oxygen in the water bodies.