JEE MAIN · CHEMISTRY · EQUILIBRIUM
JEE Main Equilibrium Questions & Solutions
67 solved questions on Equilibrium, ranging from easy to JEE-Advanced-flavour hard. Click any to see the full solution.
67 solved questions on Equilibrium, ranging from easy to JEE-Advanced-flavour hard. Click any to see the full solution.
${K_{{a_1}}}$, ${K_{{a_2}}}$ and ${K_{{a_3}}}$ are the respective ionization constants for the following reactions (a), (b) and (c). (a) $${H_2}{C_2}{O_4}…
View solution →$25.0 \mathrm{~mL}$ of $0.050 ~\mathrm{M} ~\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ is mixed with $25.0 \mathrm{~mL}$ of $0.020 ~\mathrm{M} ~\mathrm{NaF} .…
View solution →Given below are two statements : Statement (I) : Aqueous solution of ammonium carbonate is basic. Statement (II) : Acidic/basic nature of salt solution of a salt of weak acid and…
View solution →If the solubility product of PbS is 8 $\times$ 10$-$28, then the solubility of PbS in pure water at 298 K is x $\times$ 10$-$16 mol L$-$1. The value of x is __________. (Nearest…
View solution →A litre of buffer solution contains 0.1 mole of each of NH$_3$ and NH$_4$Cl. On the addition of 0.02 mole of HCl by dissolving gaseous HCl, the pH of the solution is found to be…
View solution →Two salts A2X and MX have the same value of solubility product of 4.0 $\times$ 10$-$12. The ratio of their molar solubilities i.e. ${{S({A_2}X)} \over {S(MX)}}$ = __________.…
View solution →The $\mathrm{pH}$ of an aqueous solution containing $1 \mathrm{M}$ benzoic acid $\left(\mathrm{pK}_{\mathrm{a}}=4.20\right)$ and $1 \mathrm{M}$ sodium benzoate is 4.5. The volume…
View solution →$\mathrm{K}_{\mathrm{a}}$ for butyric acid $\left(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{COOH}\right)$ is $2 \times 10^{-5}$. The $\mathrm{pH}$ of $0.2 \,\mathrm{M}$ solution of…
View solution →The pH of ammonium phosphate solution, if pka of phosphoric acid and pkb of ammonium hydroxide are 5.23 and 4.75 respectively, is ___________.
View solution →$600 \mathrm{~mL}$ of $0.01~\mathrm{M} ~\mathrm{HCl}$ is mixed with $400 \mathrm{~mL}$ of $0.01~\mathrm{M} ~\mathrm{H}_{2} \mathrm{SO}_{4}$. The $\mathrm{pH}$ of the mixture is…
View solution →$200 \mathrm{~mL}$ of $0.01 \,\mathrm{M} \,\mathrm{HCl}$ is mixed with $400 \mathrm{~mL}$ of $0.01 \,\mathrm{M} \,\mathrm{H}_{2} \mathrm{SO}_{4}$. The $\mathrm{pH}$ of the mixture…
View solution →The equilibrium $\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightleftharpoons 2 \mathrm{CrO}_4^{2-}$ is shifted to the right in :
View solution →Class XII students were asked to prepare one litre of buffer solution of $\mathrm{pH} \,8.26$ by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the…
View solution →A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of ${{[C{H_3}C{H_2}CO{O^ - }]} \over {[C{H_3}C{H_2}COOH]}}$ required to…
View solution →Arrange the following solutions in the decreasing order of pOH : (A) 0.01 M HCl (B) 0.01 M NaOH (C) 0.01 M CH3COONa (D) 0.01 M NaCl
View solution →In the titration of $\mathrm{KMnO}_{4}$ and oxalic acid in acidic medium, the change in oxidation number of carbon at the end point is ___________.
View solution →Arrange the following in increasing order of solubility product : $\mathrm{Ca}(\mathrm{OH})_2, \mathrm{AgBr}, \mathrm{PbS}, \mathrm{HgS}$
View solution →For the following Assertion and Reason, the correct option is : Assertion : The pH of water increases with increase in temperature. Reason : The dissociation of water into H+ and…
View solution →A soft drink was bottled with a partial pressure of CO2 of 3 bar over the liquid at room temperature. The partial pressure of CO2 over the solution approaches a value of 30 bar…
View solution →If the solubility product of AB2 is 3.20 $\times$ 10–11 M3, then the solubility of AB2 in pure water is _____ $\times$ 10–4 mol L–1. [Assuming that neither kind of ion…
View solution →The solubility of Ca(OH)2 in water is :[Given : The solubility product of Ca(OH)2 in water = 5.5 $\times$ 10$-$6]
View solution →50 mL of 0.1 M CH3COOH is being titrated against 0.1 M NaOH. When 25 mL of NaOH has been added, the pH of the solution will be _____________ $\times$ 10$-$2. (Nearest integer)…
View solution →At $310 \mathrm{~K}$, the solubility of $\mathrm{CaF}_{2}$ in water is $2.34 \times 10^{-3} \mathrm{~g} / 100 \mathrm{~mL}$. The solubility product of $\mathrm{CaF}_{2}$ is…
View solution →The solubility of AgCl will be maximum in which of the following?
View solution →The solubility product of PbI2 is 8.0 $\times$ 10$-$9. The solubility of lead iodide in 0.1 molar solution of lead nitrate is x $\times$ 10$-$6. mol/L. The value of x is…
View solution →The $\mathrm{pH}$ at which $$\mathrm{Mg}(\mathrm{OH})_2\left[\mathrm{~K}_{\mathrm{sp}}=1 \times 10^{-11}\right]$$ begins to precipitate from a solution containing $0.10…
View solution →Two solutions, A and B, each of 100L was made by dissolving 4g of NaOH and 9.8 g of H2SO4 in water, respectively. The pH of the resultant solution obtained from mixing 40L of…
View solution →The solubility product of $\mathrm{BaSO}_{4}$ is $1 \times 10^{-10}$ at $298 \mathrm{~K}$. The solubility of $\mathrm{BaSO}_{4}$ in $0.1 ~\mathrm{M} ~\mathrm{K}_{2}…
View solution →Given below are two statements : One is labelled as Assertion A and the other labelled as reason RAssertion A : During the boiling of water having temporary hardness, Mg(HCO3)2 is…
View solution →The solubility product of Cr(OH)3 at 298 K is 6.0 × 10–31. The concentration of hydroxide ions in a saturated solution of Cr(OH)3 will be :
View solution →The dissociation constant of acetic acid is $x\times10^{-5}$. When 25 mL of 0.2 $\mathrm{M~CH_3COONa}$ solution is mixed with 25 mL of 0.02 $\mathrm{M~CH_3COOH}$ solution, the pH…
View solution →When the hydrogen ion concentration [H$^+$] changes by a factor of 1000, the value of pH of the solution __________
View solution →Solubility of calcium phosphate (molecular mass, M) in water is $\mathrm{W_{g}}$ per $100 \mathrm{~mL}$ at $25^{\circ} \mathrm{C}$. Its solubility product at $25^{\circ}…
View solution →For a sparingly soluble salt $\mathrm{AB}_2$, the equilibrium concentrations of $\mathrm{A}^{2+}$ ions and $B^{-}$ ions are $1.2 \times 10^{-4} \mathrm{M}$ and $0.24 \times…
View solution →3 g of acetic acid is added to 250 mL of 0.1 M HCL and the solution made up to 500 mL. To 20 mL of this solutions ${1 \over 2}$ mL of 5 M NaOH is added. The pH of the solution is…
View solution →Consider the dissociation of the weak acid HX as given below $$\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}^{-}(\mathrm{aq}), \mathrm{Ka}=1.2…
View solution →Given below are two statements : One is labelled as Assertion A and the other is labelled as Reason R Assertion A : Permanganate titrations are not performed in presence of…
View solution →Given below are two statements : Statement (I) : A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities Statement (II) : Blood is…
View solution →The Ksp for the following dissociation is 1.6 × 10–5 $PbC{l_{2(s)}} \leftrightharpoons Pb_{(aq)}^{2 + } + 2Cl_{(aq)}^ -$ Which of the following choices is correct for a mixture…
View solution →A solution is 0.1 M in Cl$-$ and 0.001 M in CrO$_4^{2 - }$. Solid AgNO3 is gradually added to it. Assuming that the addition does not change in volume and Ksp(AgCl) = 1.7 $\times$…
View solution →$\mathrm{K}_{\mathrm{a}}$ for $\mathrm{CH}_3 \mathrm{COOH}$ is $1.8 \times 10^{-5}$ and $\mathrm{K}_{\mathrm{b}}$ for $\mathrm{NH}_4 \mathrm{OH}$ is $1.8 \times 10^{-5}$. The…
View solution →Millimoles of calcium hydroxide required to produce 100 mL of the aqueous solution of pH 12 is $x\times10^{-1}$. The value of $x$ is ___________ (Nearest integer). Assume complete…
View solution →pH of water is 7 at $25^{\circ} \mathrm{C}$. If water is heated to $80^{\circ} \mathrm{C}$., it's pH will :
View solution →The solubility product of a sparingly soluble salt A2X3 is 1.1 $\times$ 10$-$23. If specific conductance of the solution is 3 $\times$ 10$-$5 S m$-$1, the limiting molar…
View solution →20 mL of $0.1 ~\mathrm{M} ~\mathrm{NaOH}$ is added to $50 \mathrm{~mL}$ of $0.1 ~\mathrm{M}$ acetic acid solution. The $\mathrm{pH}$ of the resulting solution is ___________…
View solution →$25 \mathrm{~mL}$ of silver nitrate solution (1M) is added dropwise to $25 \mathrm{~mL}$ of potassium iodide $(1.05 \mathrm{M})$ solution. The ion(s) present in very small…
View solution →An analyst wants to convert $1 \mathrm{~L} \mathrm{~HCl}$ of $\mathrm{pH}=1$ to a solution of $\mathrm{HCl}$ of $\mathrm{pH} ~2$. The volume of water needed to do this dilution is…
View solution →In order to prepare a buffer solution of pH 5.74, sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is 1.0 M, the concentration of sodium…
View solution →pH value of 0.001 M NaOH solution is ____________.
View solution →If 1 mM solution of ethylamine produces $\mathrm{pH}=9$, then the ionization constant $\left(\mathrm{K}_{\mathrm{b}}\right)$ of ethylamine is $10^{-x}$. The value of $x$ is…
View solution →The observed and normal molar masses of compound $\mathrm{MX}_2$ are 65.6 and 164 respectively. The percent degree of ionisation of $\mathrm{MX}_2$ is __________%. (Nearest…
View solution →The pH of a 0.01 M weak acid $\mathrm{HX}\left(\mathrm{K}_a=4 \times 10^{-10}\right)$ is found to be 5 . Now the acid solution is diluted with excess of water so that the pH of…
View solution →$x \mathrm{mg}$ of $\mathrm{Mg}(\mathrm{OH})_2($ molar mass $=58)$ is required to be dissolved in 1.0 L of water to produce a pH of 10.0 at 298 K . The value of $x$ is ________…
View solution →The molar conductance of an infinitely dilute solution of ammonium chloride was found to be $185 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and the ionic conductance of…
View solution →The percentage dissociation of a salt $\left(\mathrm{MX}_3\right)$ solution at given temperature (van't Hoff factor $\mathrm{i}=2$ ) is ___________ %(Nearest integer)
View solution →One litre buffer solution was prepared by adding 0.10 mol each of $\mathrm{NH}_3$ and $\mathrm{NH}_4 \mathrm{Cl}$ in deionised water. The change in pH on addition of 0.05 mol of…
View solution →The strength of an aqueous NaOH solution is most accurately determined by titrating : (Note : consider that an appropriate indicator is used)
View solution →For the following Assertion and Reason, the correct option is Assertion (A): When Cu (II) and sulphide ions are mixed, they react together extremely quickly to give a solid.…
View solution →Which of the following compound CANNOT act as a Lewis base?
View solution →Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R : Assertion A : The amphoteric nature of water is explained by using Lewis…
View solution →The incorrect statement for the use of indicators in acid-base titration is :
View solution →Which of the following statement(s) is/are correct? (A) The $\mathrm{pH}$ of $1 \times 10^{-8}~ \mathrm{M} ~\mathrm{HCl}$ solution is 8 . (B) The conjugate base of $\mathrm{H}_{2}…
View solution →Which of the following happens when $\mathrm{NH}_4 \mathrm{OH}$ is added gradually to the solution containing 1 M $\mathrm{A}^{2+}$ and $1 \mathrm{M} \mathrm{B}^{3+}$ ions? Given…
View solution →$\mathrm{K}_{\mathrm{sp}}$ for $\mathrm{Cr}(\mathrm{OH})_3$ is $1.6 \times 10^{-30}$. What is the molar solubility of this salt in water?
View solution →A weak acid HA has degree of dissociation x . Which option gives the correct expression of ( pH - $\mathrm{pK}_{\mathrm{a}}$)?
View solution →If equal volumes of $A B_2$ and $X Y$ (both are salts) aqueous solutions are mixed, which of the following combination will give a precipitate of $\mathrm{AY}_2$ at 300 K ? (Given…
View solution →An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would $($ Given $\log 2=0.30)$
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