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Recent questions and answers in Equilibrium

Questions >> JEEMAIN and NEET >> Chemistry >> Equilibrium

If the solubility of $Ag_2CrO_4$ is S mole/litre. Its solubility product is

answered Feb 21, 2018 by meena.p

2 answers

$H_3BO_3$ is

answered Feb 21, 2018 by meena.p

2 answers

Percentage ionisation of a weak monobasic acid can be calculated by using the formula

answered Jan 29, 2018 by sharmaaparna1

2 answers

The pH of pure water at $80^\circ C$ will be

answered Jan 29, 2018 by sharmaaparna1

2 answers

Which of the following ionic species has the greatest protons affinity to form stable compound?

answered Jan 23, 2018 by meena.p

2 answers

Conjugate base of Hydrazoic acid is

answered Jan 23, 2018 by meena.p

2 answers

Which of the following can act both as a Bronsted acid and a Bronsted base?

answered Jan 18, 2018 by priyanka.c

2 answers

Which of the following dashed line represents the position at equilibrium for the concentration-time plot of a reaction??

answered Nov 25, 2017 by sharmaaparna1

2 answers

State True or False$S_1$ : Third group of periodic table accommodates maximum number of elements. $S_2$ : Due to presence of half filled and fully filled sub shells in electronic configuration electronegativity of atom increases. $S_3$ : The element of 13th group and 7th period will have atomic number 113. $S_4$ : diagonal relationship in 2nd and 3rd period element is found due to similar charge to size ratio.

answered Jan 18, 2016 by meena.p

1 answer

The dissociation constant of certain weak acid HA is $1 \times 10^{-4}$. The equilibrium constant for its reaction with strong base BOH is

answered Nov 29, 2013 by mosymeow_1

1 answer

The dissociation constant of $H_2S$ and $HS^-$ are respectively $10^{-7}$ and $10^{-13}$. The $pH$ of 0.1 M aqueous solution of $H_2S$ will be

answered Nov 29, 2013 by mosymeow_1

1 answer

The hydronium ion concentration in pure water is $1 \times 10^{-7}$ mol$L^{-1}$. The degree of dissociation of water is

answered Nov 29, 2013 by mosymeow_1

1 answer

$pK_b$ of $NH_3$ is 4.74. The $pH$ when 100 mL of 0.01 M $NH_3$ solution is 50% neutralised by 0.01 M HCl is,

answered Nov 29, 2013 by mosymeow_1

1 answer

$K_a$ for HCN is $5 \times 10^{-10}$ at $25^\circ C$. How much volume of 5 M KCN solution is required to be added to 10 mL of 2 M HCN in order to maintain $pH$ = 9

answered Nov 29, 2013 by mosymeow_1

1 answer

$pK_{a1}$ and $pK_{a2}$ of $H_2CO_3$ are 6.38 and 10.26 respectively. The $pH$ of 1 M and 0.1 M $NaHCO_3$ are

answered Nov 29, 2013 by mosymeow_1

1 answer

$pK_{a1}, pK_{a2}$ and $pK_{a3}$ of $H_3PO_4$ are respectively x, y and z. $pH$ of 0.1 M $Na_2HPO_4$ solution is

answered Nov 29, 2013 by mosymeow_1

1 answer

$pH$ of the solution containing 50.0 mL of 0.3 M HCl and 50.0 mL of 0.4 M $NH_3$ is

answered Nov 29, 2013 by mosymeow_1

1 answer

A weak base, B has basicity constant, $K_b = 2 \times 10^{-5}$. The $pH$ of any solution in which $[B] = [BH^+]$ is

answered Nov 29, 2013 by mosymeow_1

1 answer

$pH$ of 0.01 M $(NH_4)_2SO_4$ and 0.02 M $NH_4OH$ buffer ($pK_a$ of $NH_4^+$ = 9.26) is

answered Nov 29, 2013 by mosymeow_1

1 answer

100 mL of $pH$ =6 solution is diluted to 100 mL by water. $pH$ of the solution will increase by

answered Nov 29, 2013 by mosymeow_1

1 answer

BOH is a weak base. Molar concentration of BOH provides a [OH^-] of $1.5 \times 10^{-3}$ M is [Given $K_b$ (BOH) = $1.5 \times 10^{-3}$]

answered Nov 29, 2013 by mosymeow_1

1 answer

Which of the following solutions will have $pH$ of 4.74?

answered Nov 29, 2013 by mosymeow_1

1 answer

For the reaction $S_2O_3^{2-} (aq) + 2H_3O^+ (aq) \rightleftharpoons S (s) + H_2SO_3 (aq) + H_2O(l)$; Rate = $k [H_3O^+][S_2O_3^{2-}]$. Reaction is fastest in

answered Nov 29, 2013 by mosymeow_1

1 answer

Both $HCOOH$ and $CH_3COOH$ solutions have equal $pH$. If $\frac{K_1}{K_2}$ (ratio of acid ionisation constants) of these acids is 4, their molar concentration ratio will be

answered Nov 29, 2013 by mosymeow_1

1 answer

$pH$ of $Ca(OH)_2$ solution is 12. Millimoles of ($Ca(OH)_2$) present in 100 mL of solution will be

answered Nov 29, 2013 by mosymeow_1

1 answer

Assuming 100% ionization in case of strong electrolytes which of the following will have minimum $pH$?

answered Nov 29, 2013 by mosymeow_1

1 answer

To prepare a buffer of $pH$ 8.26 amount of $(NH_4)_2SO_4$ to be added into 50 mL of 0.01 M $NH_4OH$ solution is [$pK_a (NH_4^+)$ = 9.26]

answered Nov 29, 2013 by mosymeow_1

1 answer

Which of the following mixtures will act as a buffer solution when dissolved in 50 mL of water?

answered Nov 29, 2013 by mosymeow_1

1 answer

$pH$ at which an acidic indicator with $K_{in} = 1 \times 10^{-5}$ changes colour when the indicator is $1 \times 10^{-3}$ M is

answered Nov 29, 2013 by mosymeow_1

1 answer

To 10 mL of aqueous solution some strong acid having $pH$ = 2 is mixed with $pH$ = 4.0. The $pH$ of resulting solution is

answered Nov 29, 2013 by mosymeow_1

1 answer

The $pH$ of 0.1 M solution of $NH_4OH$ (having dissociation constant $K_b = 1.0 \times 10^{-5})$ is equal to

answered Nov 29, 2013 by mosymeow_1

1 answer

A solution was prepared by dissolving 0.0005 mol of $Ba(OH)_2$ in 100 mL of the solution. If the base is assumed to ionise completely, the $pOH$ of the solution will be

answered Nov 29, 2013 by mosymeow_1

1 answer

The $pH$ of a solution is 5.00. To this solution, sufficient acid is added to lower the $pH$ to 2.00. The corresponding increase in $H_3O^+$ ion concentration is

answered Nov 29, 2013 by mosymeow_1

1 answer

$M_2SO_4$ ($M^+$ is monovalent metal ion) has a $K_{sp}$ of $3.2 \times 10^{-5}$ at 298 K. The maximum concentration of $SO^{2-}_4$ ion that could be attained in a saturated solution of this solid at 289 K is

answered Nov 29, 2013 by mosymeow_1

1 answer

The value of $K^{sp}$ of $HgCl_2$ at room temperature is $4 \times 10^{-15}$. The concentration of $Cl^-$ ion in its aqueous solution at saturation point is

answered Nov 29, 2013 by mosymeow_1

1 answer

The dissociation constants of two acids $HA_1$ and $HA_2$ are $3.0 \times 10^{-4}$ and $1.8 \times 10^{-5}$ respectively. The relative strengths of the acids will be

answered Nov 29, 2013 by mosymeow_1

1 answer

At a certain temperature, dissociation constant of formic acid and acetic acid are $1.8 \times 10^{-4}$ and $1.8 \times 10^{-5}$ respectively. At what concentration of acetic solution, the $H_3O^+$ ion concentration is same as that in 0.001 M fromic acid solution

answered Nov 29, 2013 by mosymeow_1

1 answer

$pH$ of a mixture of 1 M benzoic acid ($pK_a$ = 4.20) and 1 M solution benzoate is 4.5. In 300 mL of buffer solution, volume of benzoic acid solution is

answered Nov 29, 2013 by mosymeow_1

1 answer

If freezing point of 0.1 M aqueous weak monobasic acid is $-0.2046^\circ C$, then $pH$ of solution is [$K_f (H_2O) = 1.86 kg mol^{-1}$]

answered Nov 29, 2013 by mosymeow_1

1 answer

If equilibrium constant of the reaction of weak acid $HA$ with $NaOH$ is $10^9$, then $pH$ of $0.1\; M\; NaA$ is

answered Nov 29, 2013 by mosymeow_1

1 answer

Equal volume of the follwing $Ca^{2+}$ and $F^-$ solutions are mixed. In which of the follwing solutions will precipitation occur?

answered Nov 29, 2013 by mosymeow_1

1 answer

For a concentrated solution of a weak electrolytic $A_xB_y$ of concentration C, the degree of dissociation $\alpha$ is given by

answered Nov 29, 2013 by mosymeow_1

1 answer

Ammonium acetate which is 0.01 M, is hydrolysed to 0.001 M concentration. Calculate the change in $pH$ in 0.001 M solution, if initially $pH = pK_a$

answered Nov 28, 2013 by mosymeow_1

1 answer

The dissociation constants of four monobasic acids HA, HX, HY and HD are respectively $6 \times 10^{-4}, 5 \times 10^{-5}, 3.6 \times 10^{-6}, 7 \times 10^{-10}$. The $pH$ values of their 0.1 M aqueous solutions is

answered Nov 28, 2013 by mosymeow_1

1 answer

Three sparingly solube salts $M_2V, MX and MX_3$ have same value of solubility product. Their solubilities follow the order

answered Nov 28, 2013 by mosymeow_1

1 answer

If $K_1$ and $K_2$ are respective equilibrium constants of two reactions: $XeF_6 (g) + H_2O(g) \rightleftharpoons XeOF_4 (g) + 2HF(g)$ and $XeO_4 (g) + XeF_6(g) \rightleftharpoons XeOF_4 (g) + 2XeO_3F_2(g)$ Then equilibrium constant for the reaction $XeO_4(g) + 2HF(g) \rightleftharpoons XeO_3F_2(g) + H_2O(g)$ will be

answered Nov 28, 2013 by mosymeow_1

1 answer

The $pH$ value of gastric juice in human stomach is about 1.8 and in the small intestine it is about 7.8. The $pK_a$ value of aspirin is 3.5. Aspirin will be

answered Nov 28, 2013 by mosymeow_1

1 answer

The rapid change of $pH$ near the stoichiometric point of an acid-base titration is the basis of indicator detection. $pH$ of the solution is related to ratio of the concentration of the conjugated acid(HIn) and base (In) form of the indicator by the expression

answered Nov 27, 2013 by mosymeow_1

1 answer

What is the correct relationship between the $pH$s of isomolar solutions of sodium oxide ($pH_1$), sodium sulphide ($pH_2$), sodium selenide ($pH_3$) and sodium telluride ($pH_4$)?

answered Nov 27, 2013 by mosymeow_1

1 answer

The $pK_a$ of weak acid (HA) is 4.5 . The $pOH$ of an aqueous buffered solution of HA in which 50% of acid is ionized is

asked Nov 27, 2013 by mosymeow_1

1 answer

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