Ionic Equilibrium

129 questions · Chemistry · JEE Main

Ionic Equilibrium

129 questions · Chemistry · JEE Main

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 $AY_{2}$ at 300 K ? (Given $K_{sp} ($ at 300 K ) for $AY_{2} = 5.2 \times 1 0^{- 7}$ …2025 · 2 Apr · Shift 1 · Q3 · MCQ
40 mL of a mixture of $CH_{3} COOH$ and HCl (aqueous solution) is titrated against 0.1 M NaOH solution conductometrically. Which of the following statement is correct? Includes diagram2025 · 3 Apr · Shift 2 · Q19 · MCQ
The pH of a 0.01 M weak acid $HX (K_{a} = 4 \times 1 0^{- 10})$ is found to be 5 . Now the acid solution is diluted with excess of water so that the pH of the solution changes to 6 . The new concentration of the…2025 · 4 Apr · Shift 1 · Q21 · Numerical
The molar conductance of an infinitely dilute solution of ammonium chloride was found to be $185 S cm^{2} mol^{- 1}$ and the ionic conductance of hydroxyl and chloride ions are 170 and $70 S cm^{2} mol^{- 1}$ …2025 · 4 Apr · Shift 2 · Q24 · Numerical
$x mg$ of $Mg (OH)_{2} ($ 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 mg. (Nearest integer) (Given : $Mg (OH)_{2}$ …2025 · 4 Apr · Shift 2 · Q25 · Numerical
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 $lo g 2 = 0.30)$ 2025 · 7 Apr · Shift 1 · Q1 · MCQ
The percentage dissociation of a salt $(MX_{3})$ solution at given temperature (van't Hoff factor $i = 2$ ) is %(Nearest integer)2025 · 7 Apr · Shift 1 · Q24 · Numerical
One litre buffer solution was prepared by adding 0.10 mol each of $NH_{3}$ and $NH_{4} Cl$ in deionised water. The change in pH on addition of 0.05 mol of HCl to the above solution is $\times 1 0^{- 2}$ …2025 · 7 Apr · Shift 2 · Q24 · Numerical
The molar solubility(s) of zirconium phosphate with molecular formula $(Zr^{4 +})_{3} (PO_{4}^{3 -})_{4}$ is given by relation :2025 · 22 Jan · Shift 2 · Q11 · MCQ
Which of the following happens when $NH_{4} OH$ is added gradually to the solution containing 1 M $A^{2 +}$ and $1 M B^{3 +}$ ions? Given : $K_{sp} [A (OH)_{2}] = 9 \times 1 0^{- 10}$ …2025 · 23 Jan · Shift 1 · Q13 · MCQ
If 1 mM solution of ethylamine produces $pH = 9$ , then the ionization constant $(K_{b})$ of ethylamine is $1 0^{- x}$ . The value of $x$ is (nearest integer). [The degree of…2025 · 23 Jan · Shift 1 · Q23 · Numerical
pH of water is 7 at $2 5^{\circ} C$ . If water is heated to $8 0^{\circ} C$ ., it's pH will :2025 · 23 Jan · Shift 2 · Q1 · MCQ
$K_{sp}$ for $Cr (OH)_{3}$ is $1.6 \times 1 0^{- 30}$ . What is the molar solubility of this salt in water?2025 · 24 Jan · Shift 1 · Q9 · MCQ
The observed and normal molar masses of compound $MX_{2}$ are 65.6 and 164 respectively. The percent degree of ionisation of $MX_{2}$ is %. (Nearest integer)2025 · 24 Jan · Shift 2 · Q24 · Numerical
A weak acid HA has degree of dissociation x . Which option gives the correct expression of ( pH - $pK_{a}$ )?2025 · 28 Jan · Shift 1 · Q4 · MCQ
Arrange the following in increasing order of solubility product : $Ca (OH)_{2}, AgBr, PbS, HgS$ 2025 · 28 Jan · Shift 2 · Q5 · MCQ
$K_{a}$ for $CH_{3} COOH$ is $1.8 \times 1 0^{- 5}$ and $K_{b}$ for $NH_{4} OH$ is $1.8 \times 1 0^{- 5}$ . The $pH$ of ammonium acetate solution will be …2024 · 1 Feb · Shift 1 · Q28 · Numerical
Solubility of calcium phosphate (molecular mass, M) in water is $W_{g}$ per $100 mL$ at $2 5^{\circ} C$ . Its solubility product at $2 5^{\circ} C$ will be approximately.2024 · 1 Feb · Shift 2 · Q2 · MCQ
Consider the dissociation of the weak acid HX as given below $HX (aq) ⇌ H^{+} (aq) + X^{-} (aq), Ka = 1.2 \times 1 0^{- 5}$ [ $K_{a}$ : dissociation…2024 · 6 Apr · Shift 1 · Q23 · Numerical
The equilibrium $Cr_{2} O_{7}^{2 -} ⇌ 2 CrO_{4}^{2 -}$ is shifted to the right in :2024 · 8 Apr · Shift 2 · Q12 · MCQ
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 naturally occurring buffer solution whose $pH$ is…2024 · 8 Apr · Shift 2 · Q2 · MCQ
For a sparingly soluble salt $AB_{2}$ , the equilibrium concentrations of $A^{2 +}$ ions and $B^{-}$ ions are $1.2 \times 1 0^{- 4} M$ and $0.24 \times 1 0^{- 3} M$ , respectively. The solubility product of $AB_{2}$ …2024 · 9 Apr · Shift 2 · Q14 · MCQ
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 weak base depends on $K_{a}$ and $K_{b}$ value of acid and the…2024 · 27 Jan · Shift 1 · Q16 · MCQ
The $pH$ at which $Mg (OH)_{2} [K_{sp} = 1 \times 1 0^{- 11}]$ begins to precipitate from a solution containing $0.10 M Mg^{2 +}$ ions is .2024 · 30 Jan · Shift 1 · Q25 · Numerical
The $pH$ of an aqueous solution containing $1 M$ benzoic acid $(pK_{a} = 4.20)$ and $1 M$ sodium benzoate is 4.5. The volume of benzoic acid solution in $300 mL$ of this…2024 · 30 Jan · Shift 2 · Q26 · Numerical
The titration curve of weak acid vs. strong base with phenolphthalein as indictor) is shown below. The $K_{phenolphthalein} = 4 \times 1 0^{- 10}$ . Given: $lo g 2 = 0.3$ The number of following statement/s which is/are… Includes diagram2023 · 8 Apr · Shift 1 · Q18 · Numerical
The solubility product of $BaSO_{4}$ is $1 \times 1 0^{- 10}$ at $298 K$ . The solubility of $BaSO_{4}$ in $0.1 M K_{2} SO_{4} (aq)$ solution is $\times 1 0^{- 9} g L^{- 1}$ …2023 · 8 Apr · Shift 2 · Q16 · Numerical
$25 mL$ of silver nitrate solution (1M) is added dropwise to $25 mL$ of potassium iodide $(1.05 M)$ solution. The ion(s) present in very small quantity in the solution is/are :2023 · 11 Apr · Shift 1 · Q7 · MCQ
An analyst wants to convert $1 L HCl$ of $pH = 1$ to a solution of $HCl$ of $pH 2$ . The volume of water needed to do this dilution is $mL$ . (Nearest integer)2023 · 12 Apr · Shift 1 · Q21 · Numerical
$25.0 mL$ of $0.050 M Ba (NO_{3})_{2}$ is mixed with $25.0 mL$ of $0.020 M NaF . K_{Sp}$ of $BaF_{2}$ is $0.5 \times 1 0^{- 6}$ at $298 K$ …2023 · 13 Apr · Shift 1 · Q22 · Numerical
20 mL of $0.1 M NaOH$ is added to $50 mL$ of $0.1 M$ acetic acid solution. The $pH$ of the resulting solution is $\times 1 0^{- 2}$ (Nearest integer) Given : $pKa (CH_{3} COOH) = 4.76$ …2023 · 13 Apr · Shift 2 · Q20 · Numerical
Which of the following statement(s) is/are correct? (A) The $pH$ of $1 \times 1 0^{- 8} M HCl$ solution is 8 . (B) The conjugate base of $H_{2} PO_{4}^{-}$ is $HPO_{4}^{2 -}$ . (C) $K_{w}$ …2023 · 15 Apr · Shift 1 · Q9 · MCQ
The dissociation constant of acetic acid is $x \times 1 0^{- 5}$ . When 25 mL of 0.2 $M C H_{3} COONa$ solution is mixed with 25 mL of 0.02 $M C H_{3} COOH$ solution, the pH of the resultant solution is found to be equal to 5. The…2023 · 24 Jan · Shift 1 · Q20 · Numerical
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 integer) Includes diagram2023 · 24 Jan · Shift 2 · Q22 · Numerical
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 $\times$ 10 $^{- 3}$ (Nearest…2023 · 25 Jan · Shift 1 · Q15 · Numerical
When the hydrogen ion concentration [H $^{+}$ ] changes by a factor of 1000, the value of pH of the solution 2023 · 25 Jan · Shift 2 · Q2 · MCQ
Millimoles of calcium hydroxide required to produce 100 mL of the aqueous solution of pH 12 is $x \times 1 0^{- 1}$ . The value of $x$ is (Nearest integer). Assume complete dissociation.2023 · 29 Jan · Shift 1 · Q13 · Numerical
$600 mL$ of $0.01 M HCl$ is mixed with $400 mL$ of $0.01 M H_{2} SO_{4}$ . The $pH$ of the mixture is $\times 1 0^{- 2}$ . (Nearest integer)…2023 · 30 Jan · Shift 1 · Q16 · Numerical
The incorrect statement for the use of indicators in acid-base titration is :2023 · 31 Jan · Shift 2 · Q13 · MCQ
At $298 K$ , the solubility of silver chloride in water is $1.434 \times 1 0^{- 3} g L^{- 1}$ . The value of $- lo g K_{sp}$ for silver chloride is . (Given mass of $Ag$ …2023 · 31 Jan · Shift 2 · Q18 · Numerical
$20 mL$ of $0.1 M NH_{4} OH$ is mixed with $40 mL$ of $0.05 M HCl$ . The $pH$ of the mixture is nearest to : (Given : $K_{b} (NH_{4} OH) = 1 \times 1 0^{- 5}, lo g 2 = 0.30, lo g 3 = 0.48, lo g 5 = 0.69, lo g 7 = 0.84, lo g 11 = 1.04)$ …2022 · 25 Jul · Shift 1 · Q4 · MCQ
$K_{a_{1}}$ , $K_{a_{2}}$ and $K_{a_{3}}$ are the respective ionization constants for the following reactions (a), (b) and (c). (a) $H_{2} C_{2} O_{4} ⇌ H^{+} + H C_{2} O_{4}^{-}$ (b) $H C_{2} O_{4}^{-} ⇌ H^{+} + C_{2} O_{4}^{2 -}$ …2022 · 25 Jul · Shift 2 · Q3 · MCQ
The Ksp for bismuth sulphide ( $B i_{2} S_{3}$ ) is 1.08 $\times$ 10 $-$ 73. The solubility of $B i_{2} S_{3}$ in mol L $-$ 1 at 298 K is :2022 · 25 Jun · Shift 2 · Q4 · MCQ
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 acid/base concept. Reason R : Water acts as an acid with $N H_{3}$ …2022 · 25 Jun · Shift 2 · Q6 · MCQ
Class XII students were asked to prepare one litre of buffer solution of $pH 8.26$ by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the student in $0.2 M$ ammonia solution to make one…2022 · 26 Jul · Shift 2 · Q3 · MCQ
50 mL of 0.1 M $C H_{3} C O O H$ is being titrated against 0.1 M $N a O H$ . When 25 mL of $N a O H$ has been added, the pH of the solution will be $\times$ 10 $-$ 2. (Nearest integer) (Given : pKa ( $C H_{3} C O O H$ ) = 4.76) log 2 =…2022 · 26 Jun · Shift 1 · Q14 · Numerical
At $310 K$ , the solubility of $CaF_{2}$ in water is $2.34 \times 1 0^{- 3} g /100 mL$ . The solubility product of $CaF_{2}$ is $\times 1 0^{- 8} (mol / L)^{3}$ …2022 · 27 Jul · Shift 1 · Q19 · Numerical
In the titration of $KMnO_{4}$ and oxalic acid in acidic medium, the change in oxidation number of carbon at the end point is .2022 · 27 Jul · Shift 1 · Q21 · Numerical
The plot of $pH$ -metric titration of weak base $NH_{4} OH$ vs strong acid HCl looks like :2022 · 27 Jul · Shift 2 · Q3 · MCQ
pH value of 0.001 M NaOH solution is .2022 · 27 Jun · Shift 2 · Q19 · Numerical
$K_{a}$ for butyric acid $(C_{3} H_{7} COOH)$ is $2 \times 1 0^{- 5}$ . The $pH$ of $0.2 M$ solution of butyric acid is $\times 1 0^{- 1}$ .…2022 · 28 Jul · Shift 1 · Q17 · Numerical
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 hydrochloric acid. Reason R : Chlorine is formed as a consequence…2022 · 28 Jul · Shift 2 · Q4 · MCQ
The solubility product of a sparingly soluble salt $A_{2} X_{3}$ is 1.1 $\times$ 10 $-$ 23. If specific conductance of the solution is 3 $\times$ 10 $-$ 5 S m $-$ 1, the limiting molar conductivity of the solution is $x \times$ 10 $-$ 3 S m2…2022 · 28 Jun · Shift 1 · Q19 · Numerical
A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of $\frac{[ C H _{3} C H _{2} C O O ^{-} ]}{[ C H _{3} C H _{2} C O O H ]}$ required to make buffer is . Given : $K_{a} (C H_{3} C H_{2} C O O H) = 1.3 \times 1 0^{- 5}$ …2022 · 28 Jun · Shift 2 · Q4 · MCQ
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 Integer) [Given : $2$ = 1.41]2022 · 29 Jul · Shift 1 · Q20 · Numerical
$200 mL$ of $0.01 M HCl$ is mixed with $400 mL$ of $0.01 M H_{2} SO_{4}$ . The $pH$ of the mixture is . Given: $lo g 2 = 0.30, lo g 3 = 0.48, lo g 5 = 0.70, lo g 7 = 0.84, lo g 11 = 1.04$ …2022 · 29 Jul · Shift 2 · Q4 · MCQ
The solubility of AgCl will be maximum in which of the following?2022 · 29 Jun · Shift 1 · Q3 · MCQ
The molar solubility of $Z n (O H)_{2}$ in 0.1 M $N a O H$ solution is x $\times$ 10 $-$ 18 M. The value of x is (Nearest integer) (Given : The solubility product of $Z n (O H)_{2}$ is 2 $\times$ 10 $-$ 20)2021 · 1 Sep · Shift 2 · Q15 · Numerical
Two salts $A_{2} X$ and $M X$ have the same value of solubility product of 4.0 $\times$ 10 $-$ 12. The ratio of their molar solubilities i.e. $\frac{S ( A _{2} X )}{S ( M X )}$ = . (Round off to the Nearest Integer)2021 · 16 Mar · Shift 1 · Q15 · Numerical
Sulphurous acid ( $H_{2} S O_{3}$ ) has Ka1 = 1.7 $\times$ 10 $-$ 2 and Ka2 = 6.4 $\times$ 10 $-$ 8. The pH of 0.588 M $H_{2} S O_{3}$ is . (Round off to the Nearest Integer).2021 · 16 Mar · Shift 2 · Q22 · Numerical
Which of the following compound CANNOT act as a Lewis base?2021 · 17 Mar · Shift 1 · Q7 · MCQ
Given below are two statements : One is labelled as Assertion A and the other labelled as reason R Assertion A : During the boiling of water having temporary hardness, $M g (H C O_{3})_{2}$ is converted to $M g C O_{3}$ . Reason R : The solubility…2021 · 18 Mar · Shift 1 · Q14 · MCQ
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 acetate in the buffer is M. (Round…2021 · 18 Mar · Shift 1 · Q16 · Numerical
The solubility of $C d S O_{4}$ in water is 8.0 $\times$ 10 $-$ 4 mol L $-$ 1. Its solubility in 0.01 M $H_{2} S O_{4}$ solution is $\times$ 10 $-$ 6 mol L $-$ 1. (Round off to the Nearest Integer). (Assume that solubility is…2021 · 18 Mar · Shift 2 · Q21 · Numerical
A solution is 0.1 M in Cl $-$ and 0.001 M in CrO $_{4}^{2 -}$ . Solid $A g N O_{3}$ is gradually added to it. Assuming that the addition does not change in volume and Ksp( $A g C l$ ) = 1.7 $\times$ 10 $-$ 10 M2 and Ksp( $A g_{2} C r O_{4}$ ) = 1.9 $\times$ 10 $-$ …2021 · 20 Jul · Shift 2 · Q4 · MCQ
The solubility product of $P b I_{2}$ 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 . (Rounded off to the nearest…2021 · 24 Feb · Shift 2 · Q16 · Numerical
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 $-$ 16 and Ka(HCN) = 6.2 $\times$ 10 $-$ 10]2021 · 25 Feb · Shift 1 · Q1 · MCQ
The solubility of $C a (O H)_{2}$ in water is : [Given : The solubility product of $C a (O H)_{2}$ in water = 5.5 $\times$ 10 $-$ 6]2021 · 25 Feb · Shift 2 · Q3 · MCQ
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 : For titration of acetic acid with NaOH phenolphthalein is not a suitable indicator.…2021 · 26 Aug · Shift 1 · Q8 · MCQ
The pH of ammonium phosphate solution, if pka of phosphoric acid and pkb of ammonium hydroxide are 5.23 and 4.75 respectively, is .2021 · 26 Feb · Shift 2 · Q22 · Numerical
$A_{3} B_{2}$ is a sparingly soluble salt of molar mass M (g mol $-$ 1) and solubility x g L $-$ 1. The solubility product satisfies $K_{s p} = a (\frac{x}{M})^{5}$ . The value of a is . (Integer answer)2021 · 31 Aug · Shift 1 · Q21 · Numerical
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 integer) [log 2.5 = 0.3979]2021 · 31 Aug · Shift 2 · Q17 · Numerical
For the following Assertion and Reason, the correct option is Assertion (A): When $C u$ (II) and sulphide ions are mixed, they react together extremely quickly to give a solid. Reason (R): The equilibrium constant of $C u^{2 +}$ (aq) +…2020 · 2 Sep · Shift 1 · Q10 · MCQ
An acidic buffer is obtained on mixing :2020 · 3 Sep · Shift 1 · Q1 · MCQ
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 following graphs correctly depicts the change in pH?2020 · 3 Sep · Shift 2 · Q11 · MCQ
A soft drink was bottled with a partial pressure of $C O_{2}$ of 3 bar over the liquid at room temperature. The partial pressure of $C O_{2}$ over the solution approaches a value of 30 bar when 44 g of $C O_{2}$ is dissolved in 1 kg of water at…2020 · 5 Sep · Shift 1 · Q14 · Numerical
Arrange the following solutions in the decreasing order of pOH : (A) 0.01 M $H C l$ (B) 0.01 M $N a O H$ (C) 0.01 M $C H_{3} C O O N a$ (D) 0.01 M $N a C l$ 2020 · 6 Sep · Shift 1 · Q16 · MCQ
If the solubility product of $A B_{2}$ is 3.20 $\times$ 10–11 M3, then the solubility of $A B_{2}$ in pure water is $\times$ 10–4 mol L–1. [Assuming that neither kind of ion reacts with water]2020 · 6 Sep · Shift 2 · Q9 · Numerical
Two solutions, A and B, each of 100L was made by dissolving 4g of $N a O H$ and 9.8 g of $H_{2} S O_{4}$ in water, respectively. The pH of the resultant solution obtained from mixing 40L of solution A and 10L of solution B is :2020 · 7 Jan · Shift 1 · Q4 · Numerical
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 $\frac{1}{2}$ mL of 5 M NaOH is added. The pH of the solution is . [Given : pKa of acetic acid =…2020 · 7 Jan · Shift 2 · Q18 · Numerical
The strength of an aqueous NaOH solution is most accurately determined by titrating : (Note : consider that an appropriate indicator is used)2020 · 8 Jan · Shift 1 · Q15 · MCQ
The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively : Includes diagram2020 · 8 Jan · Shift 1 · Q17 · MCQ
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 $O H^{-}$ is an exothermic reaction.2020 · 8 Jan · Shift 2 · Q17 · MCQ
The Ksp for the following dissociation is 1.6 × 10–5 $P b C l_{2 (s)} ⇋ P b_{(a q)}^{2 +} + 2 C l_{(a q)}^{-}$ Which of the following choices is correct for a mixture of 300 mL 0.134 M $P b (N O_{3})_{2}$ and 100 mL 0.4 M $N a C l$ ?2020 · 9 Jan · Shift 1 · Q5 · MCQ
The solubility product of $C r (O H)_{3}$ at 298 K is 6.0 × 10–31. The concentration of hydroxide ions in a saturated solution of $C r (O H)_{3}$ will be :2020 · 9 Jan · Shift 2 · Q16 · MCQ
If solublity product of $Z r_{3} (P O_{4})_{4}$ is denoted by Ksp and its molar solubility is denoted by S, then which of the following relation between S and Ksp is correct ?2019 · 8 Apr · Shift 1 · Q19 · MCQ
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 pH of the titraction mixture in this experiment? Includes diagram2019 · 9 Apr · Shift 2 · Q21 · MCQ
20 mL of 0.1 M $H_{2} S O_{4}$ solution is added to 30 mL of of 0.2 M $N H_{4} O H$ solution. The pH of the resultant mixture is : [pkb of $N H_{4} O H$ = 4.7].2019 · 9 Jan · Shift 1 · Q17 · MCQ
The pH of rain water, is approximately :2019 · 9 Jan · Shift 2 · Q19 · MCQ
Consider the following statements (a) The pH of a mixture containing 400 mL of 0.1 M $H_{2} S O_{4}$ and 400 mL of 0.1 M $N a O H$ will be approximately 1.3 (b) Ionic product of water is temperature dependent. (c) A monobasic acid with Ka = 10–5…2019 · 10 Apr · Shift 1 · Q13 · MCQ
The pH of a 0.02 M $N H_{4} C l$ solution will be : [given Kb ( $N H_{4} O H$ ) = 10–5 and log 2 = 0.301]2019 · 10 Apr · Shift 2 · Q6 · MCQ
A mixture of 100 m mol of $C a (O H)_{2}$ and 2 g of sodium sulphate was dissolved in water and the volume was made up to 100 mL. The mass of calcium sulphate formed and the concentration of OH– in resulting solution, respectively, are : (Molar…2019 · 10 Jan · Shift 1 · Q22 · MCQ
What is the molar solubility of $A l (O H)_{3}$ in 0.2 M $N a O H$ solution ? Given that, solubility product of $A l (O H)_{3}$ = 2.4 × 10–24 :2019 · 12 Apr · Shift 1 · Q20 · MCQ
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 acid (C)2019 · 12 Apr · Shift 2 · Q18 · MCQ
The molar solubility of $C d (O H)_{2}$ is 1.84 × 10–5 M in water. The expected solubility of $C d (O H)_{2}$ in a buffer solution of pH = 12 is :2019 · 12 Apr · Shift 2 · Q4 · MCQ
If Ksp of $A g_{2} C O_{3}$ is 8 $\times$ 10–12, the molar solubility of $A g_{2} C O_{3}$ in 0.1 M $A g N O_{3}$ is -2019 · 12 Jan · Shift 2 · Q9 · MCQ
Which of the following is a Lewis acid?2018 · 15 Apr · Shift 1 · Q18 · MCQ
The minimum volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution (Ksp of $P b C l_{2}$ = 3.2 $\times$ 10-8 atomic mass of Pb = 207 u ) is :2018 · 15 Apr · Shift 1 · Q25 · MCQ
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 to 1 ?2018 · 15 Apr · Shift 2 · Q19 · MCQ
Which of the following salts is the most basic in aqueous solution?2018 · Shift 0 · Q17 · MCQ
Which of the following are Lewis acids?2018 · Shift 0 · Q18 · MCQ
An aqueous solution contains 0.10 M $H_{2} S$ and 0.20 M $H C l$ . If the equilibrium constants for the formation of $H S^{-}$ from $H_{2} S$ is 1.0 $\times$ 10–7 and that of $S^{2 -}$ from $H S^{-}$ ions is 1.2 $\times$ 10–13 then the concentration of $S^{2 -}$ …2018 · Shift 0 · Q19 · MCQ
An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination?2018 · Shift 0 · Q2 · MCQ
An aqueous solution contains an unknown concentration of $B a^{2 +}$ . When 50 mL of a 1 M solution of $N a_{2} S O_{4}$ is added, $B a S O_{4}$ just begins to precipitate. The final volume is 500 mL. The solubility product of $B a S O_{4}$ is 1 $\times$ …2018 · Shift 0 · Q20 · MCQ
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 concentration in the buffer solution will be :2017 · 8 Apr · Shift 1 · Q20 · MCQ
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 :2017 · 9 Apr · Shift 1 · Q22 · MCQ
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 :2017 · Shift 0 · Q16 · MCQ
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?2013 · Shift 0 · Q2 · MCQ
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 :2012 · Shift 0 · Q6 · MCQ
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 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is :2010 · Shift 0 · Q4 · MCQ
At 25°C, the solubility product of $M g (O H)_{2}$ is 1.0 $\times$ 10–11. At which pH, will $M g^{2 +}$ ions start precipitating in the form of $M g (O H)_{2}$ from a solution of 0.001 M $M g^{2 +}$ ions?2010 · Shift 0 · Q6 · MCQ
Three reactions involving $H_{2} P O_{4}^{-}$ are given below : (i) $H_{3} P O_{4}$ + $H_{2} O$ $\to$ $H_{3} O^{+}$ + $H_{2} P O_{4}^{-}$ (ii) $H_{2} P O_{4}^{-}$ + $H_{2} O$ $\to H P O_{4}^{2 -}$ + $H_{3} O^{+}$ (iii) $H_{2} P O_{4}^{-}$ + $O H^{-}$ $\to$ $H_{3} P O_{4}$ + $O^{2 -}$ In which of the above does $H_{2} P O_{4}^{-}$ …2010 · Shift 0 · Q7 · MCQ
Solid $B a (N O_{3})_{2}$ is gradually dissolved in a 1.0 $\times$ 10-4 M $N a_{2} C O_{3}$ solution. At what concentration of $B a^{2 +}$ will a precipitate begin to form ? (Ksp for $B a C O_{3}$ = 5.1 $\times$ 10−9 )2009 · Shift 0 · Q6 · MCQ
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 be2008 · Shift 0 · Q6 · MCQ
Four species are listed below i. $H C O_{3}^{-}$ ii. $H_{3} O^{+}$ iii. $H S O_{4}^{-}$ iv. $H S O_{3} F$ Which one of the following is the correct sequence of their acid strength?2008 · Shift 0 · Q7 · MCQ
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 :2007 · Shift 0 · Q4 · MCQ
In a sautrated solution of the sparingly soluble strong electrolyte $A g I O_{3}$ (Molecular mass = 283) the equilibrium which sets in is $A g I O_{3}$ (s) $⇋$ $A g^{+}$ (aq) + $I O_{3}^{-}$ If the solubility product constant Ksp of $A g I O_{3}$ …2007 · Shift 0 · Q5 · MCQ
The first and second dissociation constants of an acid $H_{2} A$ are 1.0 $\times$ 10−5 and 5.0 $\times$ 10−10 respectively. The overall dissociation constant of the acid will be :2007 · Shift 0 · Q6 · MCQ
Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :2005 · Shift 0 · Q10 · MCQ
The solubility product of a salt having general formula $M X_{2}$ , in water is: 4 $\times$ 10-12 . The concentration of $M^{2 +}$ ions in the aqueous solution of the salt is :2005 · Shift 0 · Q6 · MCQ
What is the conjugate base of $O H^{-}$ ?2005 · Shift 0 · Q9 · MCQ
The conjugate base of $H_{2} P O_{4}^{-}$ is :2004 · Shift 0 · Q3 · MCQ
The molar solubility (in ol L-1) of a sparingly soluble salt $M X_{4}$ is "s". The corresponding solubility product is Ksp. 's' is given in term of Ksp by the relation :2004 · Shift 0 · Q7 · MCQ
Which one of the following statements is not true?2003 · Shift 0 · Q1 · MCQ
When rain is accompanied by a thunderstorm, the collected rain water will have a pH value :2003 · Shift 0 · Q10 · MCQ
The solubility in water of a sparingly soluble salt $A B_{2}$ is 1.0 $\times$ 10-5 mol L-1. Its solubility product number will be :2003 · Shift 0 · Q7 · MCQ
1 M NaCL and 1 M HCL are present in an aqueous solution. The solution is2002 · Shift 0 · Q5 · MCQ
Let the solubility of an aqueous solution of $M g (O H)_{2}$ be x then its Ksp is :2002 · Shift 0 · Q6 · MCQ
Species acting as both Bronsted acid and base is :2002 · Shift 0 · Q7 · MCQ