# Q&A - Ask Doubts and Get Answers

Sort by :
Clear All
Q
Medical
1 week, 4 days ago

Which will make basic buffer?

• Option 1)

50 mL of 0.1 M NaOH + 25 mL of 0.1M CH3COOH

• Option 2)

100 mL of 0.1M CH3COOH + 100 mL of 0.1M NaOH

• Option 3)

100 mL of 0.1M HCl + 200 mL of 0.1M NH4OH

• Option 4)

100 mL of 0.1M HCl + 100 mL of 0.1M NaOH

View All Answers (1)

S solutionqc
Answered 1 week, 3 days ago
Basic Buffer is the solution which has salt & weak base. Option 3 is correct.Option 1)50 mL of 0.1 M NaOH + 25 mL of 0.1M CH3COOHOption 2)100 mL of 0.1M CH3COOH + 100 mL of 0.1M NaOHOption 3)100 mL of 0.1M HCl + 200 mL of 0.1M NH4OHOption 4)100 mL of 0.1M HCl + 100 mL of 0.1M NaOH
Medical
1 week, 4 days ago

pH of a saturated solution of  $Ca(OH)_2$  is 9. The solubility product $(K_{sp})$ of $Ca(OH)_2$ is:

• Option 1)

$0.5\times 10^{-15}$

• Option 2)

$0.25\times 10^{-10}$

• Option 3)

$0.125\times 10^{-15}$

• Option 4)

$0.5\times 10^{-10}$

View All Answers (1)

Answered 1 week, 3 days ago
Option 1 Given pH = 9 So,  So, And  will be               Option 1)Option 2)Option 3)Option 4)
Medical
1 week, 4 days ago

Conjugate base for Bronsted acids $H_2O$ and $HF$ are :

• Option 1)

$OH^-$ and $H_2F^+$, respectively

• Option 2)

$H_3O^+$ and $F^-$, respectively

• Option 3)

$OH^-$ and $F^-$, respectively

• Option 4)

$H_3O^+$ and $H_2F^+$, respectively

View All Answers (1)

P Plabita
Answered 1 week, 3 days ago
Option 3 Conjugate base of  and  So,  and  are the answer.Option 1) and , respectivelyOption 2) and , respectivelyOption 3) and , respectivelyOption 4) and , respectively
Medical
93 Views   |   11 months ago

If the value of an equilibrium constant for a particular reaction is 1.6 x 1012, then at equilibrium the system will contain:

• Option 1)

mostly products.

• Option 2)

similar amounts of reactants and products.

• Option 3)

all reactants.

• Option 4)

mostly reactants.

View All Answers (1)

A Ashutosh
Answered 9 months, 1 week ago
1
Medical
126 Views   |   11 months, 3 weeks ago

Which one of the following conditions will favour maximum formation of the product in the reaction,

$A_{2}(g) + B_{2}(g) \rightleftharpoons X_{2}(g) \Delta _{r}H = -X kJ$ ?

• Option 1)

High temperature and high pressure

• Option 2)

Low temperature and low pressure

• Option 3)

Low temperature and high pressure

• Option 4)

High temperature and low pressure

View All Answers (1)

S subam
Answered 11 months, 3 weeks ago
As we learnt that Effect of Pressure change - A pressure change obtained by changing the volume can affect the yield of product in case of a gaseous reaction where the total number of moles of gaseous reactant and total number of moles of gaseous product are different. -     Effect of temperature change - When a change in temperature occur, the value of equilibrium constant Kc is...
Medical
2062 Views   |   11 months, 3 weeks ago

The solubility of BaSO4 in water is 2.42 x 10-3 gL-1 at 298 K. The value of its solubility product (Ksp) will be
(Given molar mass of BaSO4 = 233 g mo1-1)

• Option 1)

1.08 x 10-14 mol2 L-2

• Option 2)

1.08 x 10-12 mol2 L-2

• Option 3)

1.08 x 10-10 mol2 L-2

• Option 4)

1.08 x 10-8 mol2 L-2

View All Answers (1)

Answered 11 months, 3 weeks ago
As we learnt that General expression of solubility product - - wherein Its solubility product is          Option 1) 1.08 x 10-14 mol2 L-2 This is incorrect. Option 2) 1.08 x 10-12 mol2 L-2 This is incorrect. Option 3) 1.08 x 10-10 mol2 L-2 This is correct. Option 4) 1.08 x 10-8 mol2 L-2 This is incorrect.
Medical
1115 Views   |   11 months, 3 weeks ago

Following solutions were prepared by mixing different volumes of NaOH and HCI of different concentrations :
a.    60 mL —M/10 HC1 + 40 mL —M/10 NaOH
b.    55 mL M/10 HCl + 45 mL M/10 NaOH
c.    75 mL M/5 HCl + 25 mL M/5 NaOH
d.    100 mI—M/10 HCl + 100 mL —M/10 NaOH

pH of which one of them will be equal to 1 ?

• Option 1)

d

• Option 2)

a

• Option 3)

b

• Option 4)

c

View All Answers (1)

V Vakul Arora
Answered 11 months, 3 weeks ago
As we learnt that The p(H) scale - Hydronium ion concentration in molarity is more conveniently expressed on a logarithmic scale known as p(H) scale. - wherein The p(H) of a solution is defined as negative logarithm to base 10 of the activity of hydrogen ion    As N1V1 > N2V2 so acid left at the end of reaction     Option 1) d This is incorrect. Option 2) a This is incorrect. Option...
Medical
86 Views   |   1 year ago

In a buffer solution containing equal concentration of $B^{-}$ and HB, the $k_b \ for \ B^{-}$ is $10^{-10}$ . The pH of buffer soluction is:

• Option 1)

10

• Option 2)

7

• Option 3)

6

• Option 4)

4

View All Answers (1)

Answered 1 year ago
As learnt in Value of Kb - - wherein     Option 1) 10 This option is incorrect Option 2) 7 This option is incorrect Option 3) 6 This option is incorrect Option 4) 4 This option is correct
Medical
112 Views   |   1 year ago

In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains $Ag^{+}$ and $Pb^{2+}$ at a  concentration of 0.10M. Aqueous HCl is added to this solution until the $Cl^{-}$ concentration is 0.10M. What will the concentration of $Ag^{+}$ and $Pb^{2+}$ be at equilibrium?

$\left ( K_{sp}\ for AgCl=1.8\times 10^{-10},\ K_{sp}\ for PbCl_{2}=1.7\times 10^{-5} \right )$

• Option 1)

$[Ag^{+}]=1.8\times 10^{-7} M; [Pb^{2+}]=1.7\times 10^{-6}M$

• Option 2)

$[Ag^{+}]=1.8\times 10^{-11} M; [Pb^{2+}]=8.5\times 10^{-5}M$

• Option 3)

$[Ag^{+}]=1.8\times 10^{-9} M; [Pb^{2+}]=1.7\times 10^{-3}M$

• Option 4)

$[Ag^{+}]=1.8\times 10^{-11} M; [Pb^{2+}]=8.5\times 10^{-4}M$

View All Answers (1)

D Divya Saini
Answered 1 year ago
As learnt in General expression of solubility product - - wherein Its solubility product is        Option 1) This option is incorrect Option 2) This option is incorrect Option 3) This option is correct Option 4) This option is incorrect
Medical
115 Views   |   1 year ago

If pH of a saturated solution of $Ba\left ( OH \right )_2$  is 12, the value of its $K_{\left ( sp \right )}$ is

• Option 1)

$4.00\times 10^{-6}M^{3}$

• Option 2)

$4.00\times 10^{-7}M^{3}$

• Option 3)

$5.00\times 10^{-6}M^{3}$

• Option 4)

$5.00\times 10^{-7}M^{3}$

View All Answers (1)

Answered 1 year ago
As learnt in General expression of solubility product - - wherein Its solubility product is       We know that,                                  S                 2S                  Option 1) This option is incorrect Option 2) This option is incorrect Option 3) This option is incorrect Option 4) This option is correct
Medical
100 Views   |   1 year ago

Which one of the following pairs of solution is not an acidic buffer?

• Option 1)

$HClO_{4}\ and\ NaClO_{4}$

• Option 2)

$CH_3COOH\ and\ CH_3COONa$

• Option 3)

$H_2CO_3\ and\ Na_2CO_3$

• Option 4)

$H_3PO_4\ and\ Na_3PO_4$

View All Answers (1)

V Vakul Arora
Answered 1 year ago
Law of Chemical equilibrium - At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value. - wherein are equilibrium concentration    Acidic Buffer is a...
Medical
102 Views   |   1 year ago

The $K_{sp} \ of \ Ag_{2}CrO_{4}, Agcl, AgBr\ and\ AgI$ are respectively, $1.1\times 10^{-12}, 1.8\times 10^{-10}, 5.0\times 10^{-13}, 8.3\times 10^{-17}$. Which one of the following salts will precipitate last if $AgNO_{3}$ solution is added to the solution containing equal moles of NaCl, NaBr, Nal, and $Na_{2}CrO_{4}$?

• Option 1)

AgCl

• Option 2)

AgBr

• Option 3)

$Ag_{2}CrO_{4}$

• Option 4)

AgI

View All Answers (1)

V Vakul Arora
Answered 1 year ago
General expression of solubility product - - wherein Its solubility product is        AgCrO4     1.1X10-12= 4 S3           1.8X10-10= S2               AgBr     5X1013 = S2                  AgI        8.3 X10-17 =  S2            Thus Ag2Cr04  will be precipitated last. Option 1) AgCl incorrect Option 2) AgBr incorrect Option 3) correct Option 4) AgI incorrect
Medical
101 Views   |   1 year ago

The $K_{sp} \ of \ Ag_{2}CrO_{4}, Agcl, AgBr\ and\ AgI$ are respectively, $1.1\times 10^{-12}, 1.8\times 10^{-10}, 5.0\times 10^{-13}, 8.3\times 10^{-17}$. Which one of the following salts will precipitate last if $AgNO_{3}$ solution is added to the solution containing equal moles of NaCl, NaBr, Nal, and $Na_{2}CrO_{4}$?

• Option 1)

AgCl

• Option 2)

AgBr

• Option 3)

$Ag_{2}CrO_{4}$

• Option 4)

AgI

View All Answers (1)

V Vakul Arora
Answered 1 year ago
General expression of solubility product - - wherein Its solubility product is        AgCrO4     1.1X10-12= 4 S3           1.8X10-10= S2               AgBr     5X1013 = S2                  AgI        8.3 X10-17 =  S2            Thus Ag2Cr04  will be precipitated last. Option 1) AgCl incorrect Option 2) AgBr incorrect Option 3) correct Option 4) AgI incorrect
Medical
95 Views   |   1 year ago

Consider the nitration of bezene using mixed conc of $H_{2}SO_{4}$ and $HNO_{3}$. If a large amount of $KHSO_{4}$ is added to the mixture, tne rate of nitration will be

• Option 1)

faster

• Option 2)

slower

• Option 3)

unchanged

• Option 4)

doubled

View All Answers (1)

P Plabita
Answered 1 year ago
Effect of concentration change on equilibrium - When the concentration of any of the reactants or products in a reaction at equilibrium is changed, the composition of the equilibrium mixture changes so as to minimize the effect of concentration change. If we add reactant, the equilibrium shift towards right. -   In the nitration of benzene in the presence of conc. H2SO4 and HNO3, benzene is...
Medical
136 Views   |   1 year ago

MY and $NY_3$, two  nearly insoluble salts, have the same $K_{sp}$ value of $6.2\times 10^{-13}$ at room temperature. Which statement would be true in regard to MY and $NY_3$?

• Option 1)

The molar solubilities of MY and $NY_3$ in water are identical.

• Option 2)

The molar solubility of MY in water is less than that of $NY_3$

• Option 3)

The salts MY and $NY_3$ are more soluble in 0.5M KY than in pure water

• Option 4)

The addition of the salt of KY to solution of MY and $NY_3$ will have no effect on their solubilities

View All Answers (1)

Answered 1 year ago
General expression of solubility product - - wherein Its solubility product is       For MY Ksp= Option 1) The molar solubilities of MY and in water are identical. incorrect Option 2) The molar solubility of MY in water is less than that of correct Option 3) The salts MY and are more soluble in 0.5M KY than in pure water incorrect Option 4) The addition of the salt of KY to...
Medical
111 Views   |   1 year ago

What is the pH of the resulting solution when equal  volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

• Option 1)

12.65

• Option 2)

2.0

• Option 3)

7.0

• Option 4)

1.04

View All Answers (1)

P prateek
Answered 1 year ago
Relation between Ka and Kb -     - wherein    .01 mole of NaOH will be completely neutralised by .01 mole of HCl. Hence remaining part of NaOH is .09 mole. as equal volume is mixed [OH-]=.04514 P(H) = 14- P(OH) = 14-log [OH-] =12.65   Option 1) 12.65 correct Option 2) 2.0 incorrect Option 3) 7.0 incorrect Option 4) 1.04 incorrect
Medical
88 Views   |   1 year ago

Which of the following statements is correct for a reversible process in a state of equilibrium?

• Option 1)

$\Delta G=2.30\ RT\ log \ K$

• Option 2)

$\Delta G^{o}=-2.30\ RT\ log \ K$

• Option 3)

$\Delta G^{o}=2.30\ RT\ log \ K$

• Option 4)

$\Delta G=-2.30\ RT\ log \ K$

View All Answers (1)

D Divya Saini
Answered 1 year ago
As we discussed in concept Relation between Gibbs energy and reaction Quotient -     - wherein is standard Gibbs energy.       Option 1) This option is incorrect. Option 2) This option is correct. Option 3) This option is incorrect. Option 4) This option is incorrect.
Medical
88 Views   |   1 year ago

The reaction $2A_{\left ( g \right )}+B_{\left ( g \right )}\rightleftharpoons 3C_{\left ( g \right )}+D_{\left ( g \right )}$ is begun with the concentrations of A and B both at an initial value of 1.00M. When equilibrium is reached, the concentrations of D is measured and found to be 0.25M. The value for the equilibrium constant for this reaction is given by the expression

• Option 1)

$[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.75 \right )^{2}\left ( 0.25 \right )]$

• Option 2)

$[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 1.00 \right )^{2}\left ( 1.00 \right )]$

• Option 3)

$[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.50 \right )^{2}\left ( 0.75 \right )]$

• Option 4)

$[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.50 \right )^{2}\left ( 0.25 \right )]$

View All Answers (1)

D Divya Saini
Answered 1 year ago
As we discussed in concept Law of Chemical equilibrium - At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value. - wherein are equilibrium...
Medical
87 Views   |   1 year ago

In which  of the following equilibrium $K_{c}$ and $K_{p}$ are not equal?

• Option 1)

$2NO_{\left ( g \right )}\rightleftharpoons N_{2\left ( g \right )}+O_{2\left ( g \right )}$

• Option 2)

$SO_{2\left ( g \right )}+NO_{2\left ( G \right )}\rightleftharpoons SO_{3\left ( g \right )}+NO_{\left ( g \right )}$

• Option 3)

$H_{2\left ( g \right )}+I_{2\left ( g \right )}\rightleftharpoons 2HI_{\left ( g \right )}$

• Option 4)

$2C_{\left ( s \right )}+O_{2\left ( g \right )}\rightleftharpoons 2CO_{2\left ( g \right )}$

View All Answers (1)

Answered 1 year ago
As we discussed in concept Relation between Kp and Kc - while calculating the value of Kp , pressure should be expressed in bar. - wherein  = (number of moles of gaseous products) - (number of moles gaseous reaction)     In 1), 2) and 3) In 4)   Option 1) This option is incorrect. Option 2) This option is incorrect. Option 3) This option is incorrect. Option 4) This option is correct.
Medical
96 Views   |   1 year ago

For the reaction $N_{2}\left ( g \right )+O_{2}\left ( g \right )\rightleftharpoons 2NO\left ( g \right )$, the equilibrium constant is $K_{1}$. The equilibrium constant is $K_{2}$ for the reaction

$2NO\left ( g \right )+O_{2}\rightleftharpoons 2NO_{2}\left ( g \right )$

What is K for the reaction

$NO_{2}(g)\rightleftharpoons \frac{1}{2}N_{2}(g)+O_{2}(g)?$

• Option 1)

$1/\left ( 2K_{1}K_{2} \right )$

• Option 2)

$1/\left ( 4K_{1}K_{2} \right )$

• Option 3)

$[1/K_{1}K_{2}]^{\frac{1}{2}}$

• Option 4)

$1/\left ( K_1 K_2 \right )$

View All Answers (1)

P Plabita
Answered 1 year ago
As we discussed in concept Law of Chemical equilibrium - At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value. - wherein are equilibrium...
Exams
Articles
Questions