Ionic Equilibrium

Given is a concentrated solution of a weak electrolyte $A_x B_y$ of concentration ' $c$ ' and dissociation constant ' K '. The degree of dissociation is given by :

Arrange the following resultant mixtures in increasing order of their pH values
A. $10 \mathrm{~mL} 0.2 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_2+25 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{HCl}$
B. $10 \mathrm{~mL} 0.01 \mathrm{M} \mathrm{H}_2 \mat...

Given below are two statements :
Statement I : Sodium dichromate and potassium dichromate are classified as primary standards in titrimetric analysis.
Statement II : Phenolphthalein is a weak base, therefore it dissociates in acidic medium....

$\mathrm{M}_3 \mathrm{~A}_2$ is a sparingly soluble salt of molar mass $y \mathrm{~g} \mathrm{~mol}^{-1}$ and solubility $x \mathrm{~g} \mathrm{~L}^{-1}$. The ratio of the molar concentration of the anion $\left(\mathrm{A}^{3-}\right)$ to t...

The pH of a solution obtained by mixing 5 mL of $0.1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ solution with 250 mL of $0.1 \mathrm{M} \mathrm{NH}_4 \mathrm{Cl}$ solution is $\_\_\_\_$ $\times 10^{-2}$.(Nearest integer) Given: $\mathrm{pK}_{\ma...

20 mL of a solution of acetic acid required 28.4 mL of 0.1 M NaOH for its neutralization. A solution (X) was prepared by mixing 20 mL of the above acetic acid and 14.2 mL of 0.1 M NaOH solution. What is the pH of the solution $(\mathrm{X})$...

The solubility product constants of $\mathrm{Ag_2CrO_4}$ and $\mathrm{AgBr}$ are $32x$ and $4y$ respectively at 298 K.The value of \(\left( \frac{\text{molarity of } \mathrm{Ag_2CrO_4}}{\text{molarity of } \mathrm{AgBr}} \right)\) can be e...

At 25°C, 20.0 mL of 0.2 M weak monoprotic acid HX is titrated against 0.2 M NaOH. The pH of the solution (a) at the start of the titration (when NaOH has not been added) and (b) when 10 mL of NaOH is added respectively, are :Given :$K_a = 5...

The first and second ionization constants of a weak dibasic acid H2A are $8.1 \times 10^{-8}$ and $1.0 \times 10^{-13}$ respectively. 0.1 mol of H2A was dissolved in 1 L of 0.1 M HCl solution. The concentration of HA- in the resultant solut...

Consider the dissociation equilibrium of the following weak acid
\(\mathrm{HA} \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{A}^{-}(\mathrm{aq})\)
If the pKa of the acid is 4 , then the pH of 10 mM HA solution is $\_\_\_\_$ .(Nea...

Consider a weak base ' B ' of $\mathrm{pK}_{\mathrm{b}}=5.699$. ' $x$ ' mL of 0.02 M HCl and ' y ' mL of 0.02 M weak base ' B ' are mixed to make 100 mL of a buffer of pH 9 at $25^{\circ} \mathrm{C}$. The values of ' $x$ ' and ' $y$ ' respe...

Consider two Group IV metal ions $\mathrm{X}^{2+}$ and $\mathrm{Y}^{2+}$.
A solution containing $0.01 \mathrm{M} \mathrm{X}^{2+}$ and $0.01 \mathrm{M} \mathrm{Y}^{2+}$ is saturated with $\mathrm{H}_2 \mathrm{~S}$. The pH at which the metal ...

Which of the following mixture gives a buffer solution with $\mathrm{pH}=9.25$ ?
Given : $\mathrm{pK}_{\mathrm{b}}\left(\mathrm{NH}_4 \mathrm{OH}\right)=4.75$

The first and second ionization constants of H2X are $2.5 \times 10^{-8}$ and $1.0 \times 10^{-13}$ respectively.The concentration of ${X^{2-}}$ in $0.1\ \mathrm{M}$ H2X solution is ______ $\times 10^{-15}\ \mathrm{M}$. (Nearest Integer)

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)

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 $\log 2=0.30)$

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 HCl to the above solution is ______________ $\times 10^{-2}$.
...

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 the solution changes to 6 . The new concentration of the dilute...

$x \mathrm{mg}$ 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 ________ mg. (Nearest integer)
(Given : $\mathrm{Mg}(\mathrm{OH})_2$ is ...

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 hydroxyl and chloride ions are 170 and $70 \mathrm{~S} \mathrm{~cm}...

40 mL of a mixture of $\mathrm{CH}_3 \mathrm{COOH}$ and HCl (aqueous solution) is titrated against 0.1 M NaOH solution conductometrically. Which of the following statement is correct?

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 $\mathrm{K}_{\mathrm{sp}}\left(\right.$ at 300 K ) for $\mat...

A weak acid HA has degree of dissociation x . Which option gives the correct expression of ( pH - $\mathrm{pK}_{\mathrm{a}}$)?

Arrange the following in increasing order of solubility product :
$\mathrm{Ca}(\mathrm{OH})_2, \mathrm{AgBr}, \mathrm{PbS}, \mathrm{HgS}$

$\mathrm{K}_{\mathrm{sp}}$ for $\mathrm{Cr}(\mathrm{OH})_3$ is $1.6 \times 10^{-30}$. What is the molar solubility of this salt in water?

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 integer)

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 : $\mathrm{K}_{\text {sp }}\left[\mathrm{A}(\mathrm{OH})_2\ri...

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 _________ (nearest integer).
[The degree of ionization of ethylamin...

pH of water is 7 at $25^{\circ} \mathrm{C}$. If water is heated to $80^{\circ} \mathrm{C}$., it's pH will :

The molar solubility(s) of zirconium phosphate with molecular formula $\left(\mathrm{Zr}^{4+}\right)_3\left(\mathrm{PO}_4^{3-}\right)_4$ is given by relation :

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 \(0.24 \times 10^{-3} \mathrm{M}\), respectively. The solubility product...

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 \(\mathrm{pH}\) is main...

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

Consider the dissociation of the weak acid HX as given below
\(\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}^{-}(\mathrm{aq}), \mathrm{Ka}=1.2 \times 10^{-5}\)
[\(\mathrm{K}_{\mathrm{a}}\) : dissociation...

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 \(0.10 \mathrm{~M} \mathrm{~Mg}^{2+}\) ions is __________.

The \(\mathrm{pH}\) of an aqueous solution containing \(1 \mathrm{M}\) benzoic acid \(\left(\mathrm{pK}_{\mathrm{a}}=4.20\right)\) and \(1 \mathrm{M}\) sodium benzoate is 4.5. The volume of benzoic acid solution in \(300 \mathrm{~mL}\) of t...

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 th...

$\mathrm{K}_{\mathrm{a}}$ 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 $\mathrm{pH}$ of ammonium acetate solution will be _________.

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 $25^{\circ} \mathrm{C}$ will be approximately.

The titration curve of weak acid vs. strong base with phenolphthalein as indictor) is shown below. The \(\mathrm{K}_{\text {phenolphthalein }}=4 \times 10^{-10}\).
Given: \(\log 2=0.3\)

The number of following statement/s which is/are corr...

The solubility product of \(\mathrm{BaSO}_{4}\) is \(1 \times 10^{-10}\) at \(298 \mathrm{~K}\). The solubility of \(\mathrm{BaSO}_{4}\) in \(0.1 ~\mathrm{M} ~\mathrm{K}_{2} \mathrm{SO}_{4}(\mathrm{aq})\) solution is ___________ $$\times 10...

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 $-\log \mathrm{K}_{\mathrm{sp}}$ for silver chloride is _________.

(Given mass of $\mathrm{Ag}$ is $107.9...

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

\(600 \mathrm{~mL}\) 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 ___________ \(\times 10^{-2}\). (Nearest integer)
[Gi...

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 dissociation.

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 integer)
[Gi...

When the hydrogen ion concentration [H\(^+\)] changes by a factor of 1000, the value of pH of the 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 of the resultant solution is found to be equal to 5. Th...

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)

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 $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$ is $\mathrm{HPO}_{4}^{2-}$.
(C) $\mathr...