Ionic Equilibrium · Chemistry · WB JEE
MCQ (Single Correct Answer)
Equal volume of two solutions $A$ and $B$ of a strong acid having $\mathrm{pH}=6.0$ and $\mathrm{pH}=4.0$ respectively are mixed together to form a new solution. The pH of the new solution will be in the range
Increasing order of solubility of AgCl in (i) $\mathrm{H}_2 \mathrm{O}$, (ii) 1 M NaCl (aq.), (iii) 1 M CaCl 2 (aq.) and (iv) $1 \mathrm{M}~ \mathrm{NaNO}_3$ (aq.) solution
As per the following equation, 0.217 g of HgO (molecular mass $=217 \mathrm{~g} \mathrm{~mol}^{-1}$ ) reacts with excess iodide. On titration of the resulting solution, how many mL of 0.01 M HCl is required to reach the equivalence point?
$\mathrm{HgO}+4 \mathrm{I}^{-}+\mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{HgI}_4{ }^{2-}+2 \mathrm{OH}^{-}$
At 25$$^\circ$$C, the ionic product of water is 10$$^{-14}$$. The free energy change for the self-ionization of water in kCal mol$$^{-1}$$ is close to
Equal volumes of aqueous solution of $$0.1(\mathrm{M}) \mathrm{HCl}$$ and $$0.2(\mathrm{M}) \mathrm{H}_2 \mathrm{SO}_4$$ are mixed. The concentration of $$\mathrm{H}^{+}$$ ions in the resulting solution is
Correct solubility order of $$\mathrm{AgF}, \mathrm{AgCl}, \mathrm{AgBr}, \mathrm{AgI}$$ in water is
What will be the change in acidity if
(i) $$\mathrm{CuSO}_4$$ is added in saturated $$(\mathrm{NH}_4)_2 \mathrm{SO}_4$$ solution
(ii) $$\mathrm{SbF}_5$$ is added in anhydrous $$\mathrm{HF}$$
Number of moles of ions produced by complete dissociation of one mole of Mohr's salt in water is
$$\mathrm{pH}$$ of $$10^{-8}(\mathrm{M}) \mathrm{~HCl}$$ solution is
The specific conductance $$(\mathrm{k})$$ of $$0.02(\mathrm{M})$$ aqueous acetic acid solution at $$298 \mathrm{~K}$$ is $$1.65 \times 10^{-4} \mathrm{~S} \mathrm{~cm}^{-1}$$. The degree of dissociation of acetic acid is
$$[\lambda_{\mathrm{O}^{+}}+=349.1 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1} \text { and } \lambda_{{ }^{\circ} \mathrm{CH}_3 \mathrm{COO}^{-}}=40.9 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}]$$
At STP, the dissociation reaction of water is $$\mathrm{H_2O\rightleftharpoons H^+~(aq.)+OH^-~(aq.)}$$, and the pH of water is 7.0. The change of standard free energy ($$\Delta$$G$$^\circ$$) for the above dissociation process is given by
Given : Ksp(SrCO3) = 7.0 $$ \times $$ 10-10,
Ksp(SrF2) = 7.9 $$ \times $$ 10-10
MCQ (More than One Correct Answer)
Which pair of ions among the following can be separated by precipitation method?
Which of the following mixtures act(s) as buffer solution?
1. 100 mL of 0.1 M CH3COOH + 100 mL of 0.1 MCH3COONa
(2) 100 mL of 0.1 MCH3COOH + 50 mL of 0.1 M NaOH
(3) 100 mL of 0.1 M CH3COOH + 100 mL of 0.1 M NaOH
(4) 100 mL of 0.1 MCH3COOH + 100 mL of 0.1 MNH3