Ionic Equilibrium · Chemistry · JEE Main

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}...

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 S...

The equilibrium $$\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightleftharpoons 2 \mathrm{CrO}_4^{2-}$$ is shifted to the right in :

Solubility of calcium phosphate (molecular mass, M) in water is $\mathrm{W_{g}}$ per $100 \mathrm{~mL}$ at $25^{\circ} \mathrm{C}$. Its solubility pro...

Given below are two statements : Statement (I) : Aqueous solution of ammonium carbonate is basic. Statement (II) : Acidic/basic nature of salt solutio...

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 conj...

$$25 \mathrm{~mL}$$ of silver nitrate solution (1M) is added dropwise to $$25 \mathrm{~mL}$$ of potassium iodide $$(1.05 \mathrm{M})$$ solution. The i...

The incorrect statement for the use of indicators in acid-base titration is :

When the hydrogen ion concentration [H$$^+$$] changes by a factor of 1000, the value of pH of the 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...

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 pe...

The plot of $$\mathrm{pH}$$-metric titration of weak base $$\mathrm{NH}_{4} \mathrm{OH}$$ vs strong acid HCl looks like :

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 chl...

$${K_{{a_1}}}$$, $${K_{{a_2}}}$$ and $${K_{{a_3}}}$$ are the respective ionization constants for the following reactions (a), (b) and (c). (a) $${H_2}...

$$20 \mathrm{~mL}$$ of $$0.1\, \mathrm{M} \,\mathrm{NH}_{4} \mathrm{OH}$$ is mixed with $$40 \mathrm{~mL}$$ of $$0.05 \mathrm{M} \mathrm{HCl}$$. The $...

The solubility of AgCl will be maximum in which of the following?

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}...

The Ksp for bismuth sulphide (Bi2S3) is 1.08 $$\times$$ 10$$-$$73. The solubility of Bi2S3 in mol L$$-$$1 at 298 K is :...

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 ...

Given below are two statements.Statement I : In the titration between strong acid and weak base methyl orange is suitable as an indicator.Statement II...

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 vo...

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 tem...

Which of the following compound CANNOT act as a Lewis base?

The solubility of Ca(OH)2 in water is :[Given : The solubility product of Ca(OH)2 in water = 5.5 $$\times$$ 10$$-$$6]...

The solubility of AgCN in a buffer solution of pH = 3 is x. The value of x is : [Assume : No cyano complex is formed; Ksp(AgCN) = 2.2 $$\times$$ 10$$-...

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 ...

100 mL of 0.1 M HCl is taken in a beaker and to it 100 mL of 0.1 M NaOH is added in steps of 2 mL and the pH is continuously measured. Which of the fo...

An acidic buffer is obtained on mixing :

For the following Assertion and Reason, the correct option is Assertion (A): When Cu (II) and sulphide ions are mixed, they react together extremely q...

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 :...

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 cho...

For the following Assertion and Reason, the correct option is : Assertion : The pH of water increases with increase in temperature. Reason : The disso...

The strength of an aqueous NaOH solution is most accurately determined by titrating : (Note : consider that an appropriate indicator is used)

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively : ...

The molar solubility of Cd(OH)2 is 1.84 × 10–5 M in water. The expected solubility of Cd(OH)2 in a buffer solution of pH = 12 is : ...

The decreasing order of electrical conductivity of the following aqueous solutions is : 0.1 M Formic acid (A), 0.1 M Acetic acid (B), 0.1 M Benzoic ac...

What is the molar solubility of Al(OH)3 in 0.2 M NaOH solution ? Given that, solubility product of Al(OH)3 = 2.4 × 10–24 :...

The pH of a 0.02 M NH4Cl solution will be : [given Kb (NH4OH) = 10–5 and log 2 = 0.301]

Consider the following statements (a) The pH of a mixture containing 400 mL of 0.1 M H2SO4 and 400 mL of 0.1 M NaOH will be approximately 1.3 (b) Ioni...

In an acid-base titration, 0.1 M HCl solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of...

If solublity product of Zr3(PO4)4 is denoted by Ksp and its molar solubility is denoted by S, then which of the following relation between S and Ksp i...

If Ksp of Ag2CO3 is 8 $$ \times $$ 10–12, the molar solubility of Ag2CO3 in 0.1 M AgNO3 is - ...

A mixture of 100 m mol of Ca(OH)2 and 2 g of sodium sulphate was dissolved in water and the volume was made up to 100 mL. The mass of calcium sulphate...

The pH of rain water, is approximately :

20 mL of 0.1 M H2SO4 solution is added to 30 mL of of 0.2 M NH4OH solution. The pH of the resultant mixture is : [pkb of NH4OH = 4.7]....

Which of the following salts is the most basic in aqueous solution?

An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination?

An aqueous solution contains an unknown concentration of Ba2+. When 50 mL of a 1 M solution of Na2SO4 is added, BaSO4 just begins to precipitate. The ...

Which of the following are Lewis acids?

An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the formation of HS– from H2S is 1.0 $$\times$$ 10–7 and that...

Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of them will be equal t...

Which of the following is a Lewis acid?

The minimum volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution (Ksp of PbCl2 = 3.2 $$ \times $$ 10-8 atomic ma...

50 mL of 0.2 M ammonia solution is treated with 25 mL of 0.2 M HCl. If pKb of ammonia solution is 4.75, the pH of the mixture will be :

Additin of sodium hydroxide solution to a weak acid (HA)results in a buffer of pH 6. If ionition constant of HA is 10$$-$$5, the ratio of salt to acid...

pKa of a weak acid (HA) and pKb of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is :

How many litres of water must be added to 1 litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of this acid is :

Three reactions involving $$H_2PO_4^−$$ are given below : (i) H3PO4 + H2O $$\to$$ H3O+ + $$H_2PO_4^−$$ (ii) $$H_2PO_4^−$$ + H2O $$\to$$ $$HPO_4^{2−}$$...

Solubility product of silver bromide is 5.0 $$\times$$ 10–13. The quantity of potassium bromide (molar mass taken as 120g of mol–1) to be added to 1 l...

At 25°C, the solubility product of Mg(OH)2 is 1.0 $$\times$$ 10–11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solu...

Solid Ba(NO3)2 is gradually dissolved in a 1.0 $$\times$$ 10-4 M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form ? (Ks...

Four species are listed below i. $$HCO_3^−$$ ii. $$H_3O^+$$ iii. $$HSO_4^−$$ iv. $$HSO_3F$$ Which one of the following is the correct sequence of th...

The pKa of a weak acid, HA, is 4.80. The pKb of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be...

The first and second dissociation constants of an acid H2A are 1.0 $$\times$$ 10−5 and 5.0 $$\times$$ 10−10 respectively. The overall dissociation co...

The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is :

In a sautrated solution of the sparingly soluble strong electrolyte AgIO3 (Molecular mass = 283) the equilibrium which sets in is AgIO3(s) $$\leftrig...

The solubility product of a salt having general formula MX2, in water is: 4 $$\times$$ 10-12 . The concentration of M2+ ions in the aqueous solution o...

Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :

What is the conjugate base of OH-?

The conjugate base of H2PO4- is :

The molar solubility (in ol L-1) of a sparingly soluble salt MX4 is "s". The corresponding solubility product is Ksp. 's' is given in term of Ksp by t...

The solubility in water of a sparingly soluble salt AB2 is 1.0 $$\times$$ 10-5 mol L-1. Its solubility product number will be :...

Which one of the following statements is not true?

When rain is accompanied by a thunderstorm, the collected rain water will have a pH value :

Species acting as both Bronsted acid and base is :

Let the solubility of an aqueous solution of Mg(OH)2 be x then its Ksp is :

1 M NaCL and 1 M HCL are present in an aqueous solution. The solution is

Consider the dissociation of the weak acid HX as given below $$\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}^{-}(...

$\mathrm{K}_{\mathrm{a}}$ for $\mathrm{CH}_3 \mathrm{COOH}$ is $1.8 \times 10^{-5}$ and $\mathrm{K}_{\mathrm{b}}$ for $\mathrm{NH}_4 \mathrm{OH}$ is $...

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}$...

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 solut...

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 re...

$$25.0 \mathrm{~mL}$$ 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}...

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 o...

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 ~\ma...

The titration curve of weak acid vs. strong base with phenolphthalein as indictor) is shown below. The $$\mathrm{K}_{\text {phenolphthalein }}=4 \time...

At $298 \mathrm{~K}$, the solubility of silver chloride in water is $1.434 \times 10^{-3} \mathrm{~g} \mathrm{~L}^{-1}$. The value of $-\log \mathrm{K...

$$600 \mathrm{~mL}$$ of $$0.01~\mathrm{M} ~\mathrm{HCl}$$ is mixed with $$400 \mathrm{~mL}$$ of $$0.01~\mathrm{M} ~\mathrm{H}_{2} \mathrm{SO}_{4}$$. T...

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 ___________ (...

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...

If the pKa of lactic acid is 5, then the pH of 0.005 M calcium lactate solution at 25$$^\circ$$C is ___________ $$\times$$ 10$$^{-1}$$ (Nearest intege...

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 $$\mat...

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. T...

$$\mathrm{K}_{\mathrm{a}}$$ for butyric acid $$\left(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{COOH}\right)$$ is $$2 \times 10^{-5}$$. The $$\mathrm{pH}$$...

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 prod...

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 ___________....

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 ...

pH value of 0.001 M NaOH solution is ____________.

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$...

The molar solubility of Zn(OH)2 in 0.1 M NaOH solution is x $$\times$$ 10$$-$$18 M. The value of x is _________ (Nearest integer)(Given : The solubili...

The pH of a solution obtained by mixing 50 mL of 1 M HCl and 30 mL of 1 M NaOH is x $$\times$$ 10$$-$$4. The value of x is ____________. (Nearest inte...

A3B2 is a sparingly soluble salt of molar mass M (g mol$$-$$1) and solubility x g L$$-$$1. The solubility product satisfies $${K_{sp}} = a{\left( {{x ...

The solubility of CdSO4 in water is 8.0 $$\times$$ 10$$-$$4 mol L$$-$$1. Its solubility in 0.01 M H2SO4 solution is __________ $$\times$$ 10$$-$$6 mol...

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, ...

Sulphurous acid (H2SO3) has Ka1 = 1.7 $$\times$$ 10$$-$$2 and Ka2 = 6.4 $$\times$$ 10$$-$$8. The pH of 0.588 M H2SO3 is __________. (Round off to the ...

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)} ...

The pH of ammonium phosphate solution, if pka of phosphoric acid and pkb of ammonium hydroxide are 5.23 and 4.75 respectively, is ___________....

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$$-$$...

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. [Assumin...

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 ...

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 ad...

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 obt...