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All questions of Ionic Equilibrium for JEE Exam
Which of the following is more acidic? A solution with pH 5 or a solution with pH 3- a)solution with pH 5
- b)solution with pH 3
- c)both are equally acidic
- d)cannot be predicted from pH values
Correct answer is option 'B'. Can you explain this answer?
Which of the following is more acidic? A solution with pH 5 or a solution with pH 3
a)
solution with pH 5
b)
solution with pH 3
c)
both are equally acidic
d)
cannot be predicted from pH values
|
Hansa Sharma answered |
We know that pH equals to - log[H+] or the value of pH is inversely proportional to the concentration of H+. So more the value of pH, less the solution be acidic.
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 - [AIEEE-2012] - a)1 × 10-3
- b)1 × 10-5
- c)1 × 10-7
- d)3 × 10-1
Correct answer is option 'B'. Can you explain this answer?
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 - [AIEEE-2012]
a)
1 × 10-3
b)
1 × 10-5
c)
1 × 10-7
d)
3 × 10-1
|
Naina Bansal answered |
HQ will dissociate as
H2O + HQ ↔ H3O^+ + Q-
Ka = [H3O^+] [Q-] / [HQ]
-log [H3O^+] = pH
- log [H3O^+] = 3
[H3O^+] = 10^-3
[H3O+] = [Q-] = 10-3
Ka = ( 10^-3)^2 / (0.1 - 10^-3) = ( 10^-3)^2 / (0.1) = 1 x 10^-5
0.023 g of sodium metal is reacted with 100 cm3 of water. The pH of the resulting solution is ______.- a)10
- b)8
- c)9
- d)12
Correct answer is option 'D'. Can you explain this answer?
0.023 g of sodium metal is reacted with 100 cm3 of water. The pH of the resulting solution is ______.
a)
10
b)
8
c)
9
d)
12
|
|
Naina Bansal answered |
Na + H2O –> NaOH
[NaOH] = (0.023/23)0.1 = 0.01
so pH is 12
A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate Ka for the acid.- a)4.2 x 10-6
- b)3.5 x 10-8
- c)3.8 x 10-9
- d)7.0 x 10-6
Correct answer is option 'B'. Can you explain this answer?
A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate Ka for the acid.
a)
4.2 x 10-6
b)
3.5 x 10-8
c)
3.8 x 10-9
d)
7.0 x 10-6
|
Preeti Iyer answered |
Since the acid is only 0.059% ionized, therefore the concentration of ions in solution = 0.1 x 0.059 / 100 = 0.000059
Ka = [H^+] [X–] / [HX] = (0.000059)^2 / 0.1 = 3.5 x 10^-8
For HF, pKa = 3.45. What is the pH of an aqueous buffer solution that is 0.1M HF (aq) and 0.300 M KF (aq)?
a)11.03b)2.97c)10.07d)3.93 Correct answer is option 'D'. Can you explain this answer?
|
Suresh Iyer answered |
Given, pKa = 3.45
Concentration of HF = 0.1 M, concentration of KF = 0.300 M
For acidic buffer;
pH = pKa + log [salt of weak acid]/[weak acid]
= 3.45 + log0.3/0.1
= 3.45 + 0.48
= 3.93
Concentration of HF = 0.1 M, concentration of KF = 0.300 M
For acidic buffer;
pH = pKa + log [salt of weak acid]/[weak acid]
= 3.45 + log0.3/0.1
= 3.45 + 0.48
= 3.93
We eat a variety of foods still pH of our blood does not change every time. The reason is- a)Strong bases in the blood donot let pH change
- b)Stomach wall is resistant
- c)There are buffers in the blood which resist pH change
- d)Strong acids in the blood donot let pH change
Correct answer is option 'C'. Can you explain this answer?
We eat a variety of foods still pH of our blood does not change every time. The reason is
a)
Strong bases in the blood donot let pH change
b)
Stomach wall is resistant
c)
There are buffers in the blood which resist pH change
d)
Strong acids in the blood donot let pH change
|
Pooja Shah answered |
The correct answer is option C
pH of blood remains constant because of the buffer system present in the blood. Acid-base buffers confer resistance to a change in the pH of a solution when hydrogen ions (protons) or hydroxide ions are added or removed. An acid-base buffer typically consists of a weak acid, and its conjugate base (salt).It used to neutralized the extra added protons or OH- in blood.The buffer for maintaining acid-base balance in the blood is the carbonic-acid-bicarbonate buffer.So pH of blood remains even after eating spicy food.
pH of blood remains constant because of the buffer system present in the blood. Acid-base buffers confer resistance to a change in the pH of a solution when hydrogen ions (protons) or hydroxide ions are added or removed. An acid-base buffer typically consists of a weak acid, and its conjugate base (salt).It used to neutralized the extra added protons or OH- in blood.The buffer for maintaining acid-base balance in the blood is the carbonic-acid-bicarbonate buffer.So pH of blood remains even after eating spicy food.
Consider KA, the potassium salt of a weak acid, HA. If a sample of KA is dissolved in water, with no other substances added, which of the following statements is true (approximately)?- a)[H3O+] = [OH-]
- b)[HA] = [K+]
- c)[HA] = [OH-]
- d)[H3O+] = [A-]
Correct answer is option 'C'. Can you explain this answer?
Consider KA, the potassium salt of a weak acid, HA. If a sample of KA is dissolved in water, with no other substances added, which of the following statements is true (approximately)?
a)
[H3O+] = [OH-]
b)
[HA] = [K+]
c)
[HA] = [OH-]
d)
[H3O+] = [A-]
|
|
Suresh Iyer answered |
The correct answer is option C
[HA] = [OH–]
The reaction is: A– + H2O ⇌ HA + OH–
[HA] = [OH–]
The reaction is: A– + H2O ⇌ HA + OH–
If the value of the solubility product for AgBr is 4.0 x 10-12 at 25°C, calculate the solubility of AgBr(s) in water.- a)2.5 x 10-13
- b)2.5 x 10-6
- c)2 x 10-6
- d)5.0 x10-7
Correct answer is option 'C'. Can you explain this answer?
If the value of the solubility product for AgBr is 4.0 x 10-12 at 25°C, calculate the solubility of AgBr(s) in water.
a)
2.5 x 10-13
b)
2.5 x 10-6
c)
2 x 10-6
d)
5.0 x10-7
|
Raghav Bansal answered |
Ksp = 4.0 x 10-12
For AB type salt, Solubility = Ksp1/2
= (4.0 x 10-12)1/2
= 2 x 10-6
For AB type salt, Solubility = Ksp1/2
= (4.0 x 10-12)1/2
= 2 x 10-6
Role of NH4Cl in qualitative analysis of third group cations- a)to provide basic medium
- b)to provide acidic medium
- c)to increase the degree of dissociation of NH4OH
- d)to suppress the degree of dissociation of NH4OH
Correct answer is option 'D'. Can you explain this answer?
Role of NH4Cl in qualitative analysis of third group cations
a)
to provide basic medium
b)
to provide acidic medium
c)
to increase the degree of dissociation of NH4OH
d)
to suppress the degree of dissociation of NH4OH
|
|
Raghav Bansal answered |
The correct answer is option D
Common ion effect is observed when a solution of weak electrolyte is mixed with a solution of strong electrolyte, which provides an ion common to that provided by weak electrolyte.
The NH4OH is a weak base and it does not ionise completely. Thus, due to presence of common ion NH4+ in NH4Cl, it suppresses the ionisation of weak base NH4OH in order to decrease the OH- concentration so that higher group cations will not get precipitated.
Thus the pair NH4OH+NH4Cl shows a common ion effect.
Ammonium chloride suppresses the ionization of ammonium hydroxide
.
Common ion effect is observed when a solution of weak electrolyte is mixed with a solution of strong electrolyte, which provides an ion common to that provided by weak electrolyte.
The NH4OH is a weak base and it does not ionise completely. Thus, due to presence of common ion NH4+ in NH4Cl, it suppresses the ionisation of weak base NH4OH in order to decrease the OH- concentration so that higher group cations will not get precipitated.
Thus the pair NH4OH+NH4Cl shows a common ion effect.
Ammonium chloride suppresses the ionization of ammonium hydroxide
.
The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?- a)Sugar releases more ions in water and increases conductance
- b)Both sugar and NaCl ionises partially in water thereby increasing the conductance
- c)Both sugar and NaCl ionises completely in water thereby increasing the conductance
- d)NaCl ionises completely in water and increase in concentration of salt increases conductance.
Correct answer is option 'D'. Can you explain this answer?
The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?
a)
Sugar releases more ions in water and increases conductance
b)
Both sugar and NaCl ionises partially in water thereby increasing the conductance
c)
Both sugar and NaCl ionises completely in water thereby increasing the conductance
d)
NaCl ionises completely in water and increase in concentration of salt increases conductance.
|
|
Sanjana Bhagat answered |
As sodium chloride dissociate in water it will produce Na+ and Cl- ions which will help to conduct electricity
when the concentration is increased more ions will be produced so the conductivity Will also increase
when the concentration is increased more ions will be produced so the conductivity Will also increase
The boiling point of water at atmospheric pressure
- a)95∘C
- b)90∘C
- c)110∘C
- d)1000C
Correct answer is option 'D'. Can you explain this answer?
The boiling point of water at atmospheric pressure
a)
95∘C
b)
90∘C
c)
110∘C
d)
1000C
|
Rohit Yadav answered |
The boiling point of a liquid is the temperature at which the vapor pressure of the liquid equals the environmental pressure surrounding the liquid. The boiling point of liquids varies with and depends upon the surrounding environmental pressure.
The normal boiling of a liquid is the special case in which the vapor pressure of the liquid equals the defined atmospheric pressure at sea level i.e., at 1 atmosphere (atm) is 100ºC.
The normal boiling of a liquid is the special case in which the vapor pressure of the liquid equals the defined atmospheric pressure at sea level i.e., at 1 atmosphere (atm) is 100ºC.
Value of pH is determined by- a)pH electrode
- b)pH detector
- c)pH balancer
- d)pH spectrometer
Correct answer is option 'A'. Can you explain this answer?
Value of pH is determined by
a)
pH electrode
b)
pH detector
c)
pH balancer
d)
pH spectrometer
|
|
Baby Ghosh answered |
The outcome of PH measurement is determined by a consideration between the number of H+ ions and the number of hydroxy ions(OH-).
When the number of H+ ions equals the number of hydroxy ions(OH-),then H2O becomes neutral .It will than have a PH of about 7.The PH of water9 can vary between 0 to 14.
When the number of H+ ions equals the number of hydroxy ions(OH-),then H2O becomes neutral .It will than have a PH of about 7.The PH of water9 can vary between 0 to 14.
In a sample of pure water, only one of the following statements is always true at all conditions of temperature and pressure.- a)[OH–] = 1.0 x 10-14 M
- b)[H3O+] = 1.0 x 10-7 M
- c)[OH–] = 1.0 x 10-7 M
- d)[H3O+] = [OH–]
Correct answer is option 'D'. Can you explain this answer?
In a sample of pure water, only one of the following statements is always true at all conditions of temperature and pressure.
a)
[OH–] = 1.0 x 10-14 M
b)
[H3O+] = 1.0 x 10-7 M
c)
[OH–] = 1.0 x 10-7 M
d)
[H3O+] = [OH–]
|
Lalit Yadav answered |
The correct answer is Option D.
The concentration of OH- will always equal the concentration of H3O+.
PV = nRT, where R is a constant, and n is the quantity of gas measured in mols. The pH of a substance is related to the concentration of H+,
so if we raise or lower the Temperature or Pressure of pure water, we will alter the Volume (or concentration) of H3O+ and OH- ions. As we alter the concentrations we alter the pH and pOH. The only answer that is true no matter what the volume or concentration may be is D
The concentration of OH- will always equal the concentration of H3O+.
PV = nRT, where R is a constant, and n is the quantity of gas measured in mols. The pH of a substance is related to the concentration of H+,
so if we raise or lower the Temperature or Pressure of pure water, we will alter the Volume (or concentration) of H3O+ and OH- ions. As we alter the concentrations we alter the pH and pOH. The only answer that is true no matter what the volume or concentration may be is D
In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (molecular mass = 283) the equilibrium which sets in is -AgIO3(s) 
Ag+(aq) + IO3¯(aq)If the solubility product Ksp of AgIO3 at a given temperature is 1.0 x 10-8, what is the mass of AgIO3 contained in 100 ml of its saturated solution ? [AIEEE-2007]- a)28.3 x 10-2 g
- b)2.83 x 10-3 g
- c)1.0 x 10-7 g
- d)1.0 x 10-4 g
Correct answer is option 'B'. Can you explain this answer?
In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (molecular mass = 283) the equilibrium which sets in is -
AgIO3(s) Ag+(aq) + IO3¯(aq)
Ag+(aq) + IO3¯(aq)If the solubility product Ksp of AgIO3 at a given temperature is 1.0 x 10-8, what is the mass of AgIO3 contained in 100 ml of its saturated solution ?
[AIEEE-2007]
a)
28.3 x 10-2 g
b)
2.83 x 10-3 g
c)
1.0 x 10-7 g
d)
1.0 x 10-4 g
|
|
Suresh Reddy answered |
is 1.0 ×10-11. At which pH, will 
ions start precipitating in the form of 
from a solution of 0.001 M 
ions ? [AIEEE-2010] 
Three reactions involving 
are given below: (i) 
(ii) 
(iii) 
In which of the above does 
act as an acid?[AIEEE-2010]- a) (i) Only
- b)(ii) Only
- c)(ii) and (iii)
- d)(iii) only
Correct answer is option 'B'. Can you explain this answer?
Three reactions involving are given below:
are given below: (i)
(ii)
(iii)
In which of the above does act as an acid?
act as an acid?[AIEEE-2010]
a)
(i) Only
b)
(ii) Only
c)
(ii) and (iii)
d)
(iii) only
|
|
Raghav Bansal answered |
Acids are those substances which gives H+. Here in reaction ii only, H2PO4- acts as an acid.
BF3does not have proton but still acts as an acid and reacts with NH3. Why is it so? What type of bond is formed between the two?
- a)BF3 is a Lewis acid and coordinate bond is formed
- b)BF3 is a Brönsted base and coordinate bond is formed
- c)BF1 is a Brönsted acid and coordinate bond is formed
- d)none
Correct answer is option 'A'. Can you explain this answer?
BF3does not have proton but still acts as an acid and reacts with NH3. Why is it so? What type of bond is formed between the two?
a)
BF3 is a Lewis acid and coordinate bond is formed
b)
BF3 is a Brönsted base and coordinate bond is formed
c)
BF1 is a Brönsted acid and coordinate bond is formed
d)
none
|
Malavika Roy answered |
BF3 is an electron deficient compound. Hence, it acts as Lewis acid. NH3 has a lone pair of electrons. Hence, acts as Lewis base. A coordinate bond is formed between the two.
H3N: →BF3
H3N: →BF3
The ionization constant of acetic acid is 1.74 x 10−5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.- a)0.00193M and pH 3.03
- b)0.00203M and pH 3.03
- c)0.00093M and pH 3.03
- d)0.00013M and pH 3.03
Correct answer is option 'C'. Can you explain this answer?
The ionization constant of acetic acid is 1.74 x 10−5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.
a)
0.00193M and pH 3.03
b)
0.00203M and pH 3.03
c)
0.00093M and pH 3.03
d)
0.00013M and pH 3.03
|
Milan Roy answered |
Calculate the hydrogen ion concentration in the human blood whose pH is 7.38.- a)3.19x10(−8)M
- b)6.33x10(−8)M
- c)4.17x10(−8)M
- d)5.16x10(−8)M
Correct answer is option 'C'. Can you explain this answer?
Calculate the hydrogen ion concentration in the human blood whose pH is 7.38.
a)
3.19x10(−8)M
b)
6.33x10(−8)M
c)
4.17x10(−8)M
d)
5.16x10(−8)M
|
Keerthana Datta answered |
-8)
To calculate the hydrogen ion concentration (H+), we can use the equation:
pH = -log[H+]
Rearranging the equation, we get:
[H+] = 10^(-pH)
Substituting the given pH value of 7.38 into the equation:
[H+] = 10^(-7.38)
Calculating this using a calculator, we find that the hydrogen ion concentration in the human blood is approximately 3.98 x 10^(-8) M.
To calculate the hydrogen ion concentration (H+), we can use the equation:
pH = -log[H+]
Rearranging the equation, we get:
[H+] = 10^(-pH)
Substituting the given pH value of 7.38 into the equation:
[H+] = 10^(-7.38)
Calculating this using a calculator, we find that the hydrogen ion concentration in the human blood is approximately 3.98 x 10^(-8) M.
How many litres of water must be added to litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2? [AIEEE-2013] - a)2.0 L
- b)9.0 L
- c)0.1 L
- d)0.9 L
Correct answer is option 'B'. Can you explain this answer?
How many litres of water must be added to litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?
[AIEEE-2013]
a)
2.0 L
b)
9.0 L
c)
0.1 L
d)
0.9 L
|
Anmol Nair answered |
Correct answer is option B.
0.1*1=(1+v)*0.01
1+v=10
v=10−1=9.0L
The solubility product of a salt having general formula MX2, in water is 4x10-12. The concentration of M2+ ions in the aqueous solution of the salt is - [AIEEE-2005] - a)1.0 x 10-4
- b)2.0 x 10-6 M
- c)4.0 x 10-10 M
- d)1.6 x 10-4 M
Correct answer is option 'A'. Can you explain this answer?
The solubility product of a salt having general formula MX2, in water is 4x10-12. The concentration of M2+ ions in the aqueous solution of the salt is - [AIEEE-2005]
a)
1.0 x 10-4
b)
2.0 x 10-6 M
c)
4.0 x 10-10 M
d)
1.6 x 10-4 M
|
|
Rahul Bansal answered |
When the value of Kc is very small then- a)reaction is at start
- b)reactant conc. Is maximum
- c)reactant conc. Is minimum
- d)reaction is completed
Correct answer is option 'B'. Can you explain this answer?
When the value of Kc is very small then
a)
reaction is at start
b)
reactant conc. Is maximum
c)
reactant conc. Is minimum
d)
reaction is completed
|
|
Rutuja Desai answered |
When the value of Kc is very small, it indicates that the equilibrium position of the reaction lies towards the left side, meaning that the concentration of the reactants is relatively high compared to the concentration of the products.
Let's understand this in detail:
Equilibrium Constant (Kc):
The equilibrium constant, Kc, is a measure of the extent of a chemical reaction at equilibrium. It is defined as the ratio of the product concentrations to the reactant concentrations, each raised to their respective stoichiometric coefficients, at equilibrium, with each concentration term raised to the power equal to its stoichiometric coefficient in the balanced chemical equation.
Kc = [Products]^n / [Reactants]^m
Where [Products] and [Reactants] represent the concentrations of the products and reactants at equilibrium, respectively, and n and m are the stoichiometric coefficients of the products and reactants, respectively.
Interpretation of a Very Small Kc Value:
When the value of Kc is very small, it means that the numerator (concentration of products) is much smaller compared to the denominator (concentration of reactants).
This implies that the concentration of the reactants is significantly higher than the concentration of the products at equilibrium.
Explanation of Correct Answer (Option B):
The correct answer, "reactant conc. is maximum," indicates that when the value of Kc is very small, the concentration of the reactants is at its maximum.
This is because the equilibrium position favors the reactants, and the reaction is not proceeding significantly towards the product side. As a result, the concentration of the reactants remains high, while the concentration of the products is relatively low.
In other words, the reaction is not proceeding to a significant extent, and the reactants are dominant in the equilibrium mixture.
Therefore, when the value of Kc is very small, it signifies that the reaction is at the start, and the concentration of the reactants is maximum.
Let's understand this in detail:
Equilibrium Constant (Kc):
The equilibrium constant, Kc, is a measure of the extent of a chemical reaction at equilibrium. It is defined as the ratio of the product concentrations to the reactant concentrations, each raised to their respective stoichiometric coefficients, at equilibrium, with each concentration term raised to the power equal to its stoichiometric coefficient in the balanced chemical equation.
Kc = [Products]^n / [Reactants]^m
Where [Products] and [Reactants] represent the concentrations of the products and reactants at equilibrium, respectively, and n and m are the stoichiometric coefficients of the products and reactants, respectively.
Interpretation of a Very Small Kc Value:
When the value of Kc is very small, it means that the numerator (concentration of products) is much smaller compared to the denominator (concentration of reactants).
This implies that the concentration of the reactants is significantly higher than the concentration of the products at equilibrium.
Explanation of Correct Answer (Option B):
The correct answer, "reactant conc. is maximum," indicates that when the value of Kc is very small, the concentration of the reactants is at its maximum.
This is because the equilibrium position favors the reactants, and the reaction is not proceeding significantly towards the product side. As a result, the concentration of the reactants remains high, while the concentration of the products is relatively low.
In other words, the reaction is not proceeding to a significant extent, and the reactants are dominant in the equilibrium mixture.
Therefore, when the value of Kc is very small, it signifies that the reaction is at the start, and the concentration of the reactants is maximum.
Acidity of BF3can be explained on the basis of which of the following concepts?- a)Arrhenius concept
- b)Bronsted Lowry concept
- c)Lewis concept
- d)Bronsted Lowry as well as Lewis concept
Correct answer is option 'C'. Can you explain this answer?
Acidity of BF3can be explained on the basis of which of the following concepts?
a)
Arrhenius concept
b)
Bronsted Lowry concept
c)
Lewis concept
d)
Bronsted Lowry as well as Lewis concept
|
Nitin Nair answered |
Sol: (c) According to Lewis concept, a positively charged or an electron deficient species acts as Lewis acid. BF3 is an electron deficient compound with B having 6 electrons only.
A catalyst increases the rate of the chemical reaction for the conversion of reactants to products by- a)lowering the equilibrium composition of a reaction mixture
- b)increasing the activation energy for the forward reaction
- c)making available a new low energy pathway
- d)lowering the temperature
Correct answer is option 'C'. Can you explain this answer?
A catalyst increases the rate of the chemical reaction for the conversion of reactants to products by
a)
lowering the equilibrium composition of a reaction mixture
b)
increasing the activation energy for the forward reaction
c)
making available a new low energy pathway
d)
lowering the temperature
|
Avi Chawla answered |
Catalyst changes the course of reaction by decreasing low Ea energy pathway.
Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume? PCl5(g) 
PCl3 (g) + Cl2 (g)- a)increase
- b)decrease largely
- c)remain the same
- d)decrease
Correct answer is option 'A'. Can you explain this answer?
Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
PCl5(g) PCl3 (g) + Cl2 (g)
PCl3 (g) + Cl2 (g)a)
increase
b)
decrease largely
c)
remain the same
d)
decrease
|
Amrutha Chaudhary answered |
When pressure is decreased , volume of reaction system will increase. So reaction will move in a direaction where there will be more number of moles. So reaction will move in forward direaction and moles of product will increase.
Which of the following is an example of basic buffer?- a)A mixture of HCl and NaOH
- b)A mixture of NH4Cl and NH4OH
- c)A mixture of CH3COOH and OH3COONa
- d)1M solution of NaOH
Correct answer is option 'B'. Can you explain this answer?
Which of the following is an example of basic buffer?
a)
A mixture of HCl and NaOH
b)
A mixture of NH4Cl and NH4OH
c)
A mixture of CH3COOH and OH3COONa
d)
1M solution of NaOH
|
|
Nandini Iyer answered |
Acidic buffer solution contains equimolar quantities of a weak acid and its salt with strong base. For example: an acetic acid, CH3COOH and sodium acetate I.e. CH3COONa. Basic buffer solution contains equimolar quantities of a weak base and its salt with strong acid.
The dynamic nature of chemical equilibrium can be demonstrated in the synthesis of ammonia by Haber.s process. Choose the appropriate option given below- a)by using sulphur isotope
- b)by using deuterium isotope
- c)by using hydrogen isotope
- d)by maintaining high temperature and low pressure
Correct answer is option 'B'. Can you explain this answer?
The dynamic nature of chemical equilibrium can be demonstrated in the synthesis of ammonia by Haber.s process. Choose the appropriate option given below
a)
by using sulphur isotope
b)
by using deuterium isotope
c)
by using hydrogen isotope
d)
by maintaining high temperature and low pressure
|
Saikat Dasgupta answered |
Dynamic nature can be studied by deuterium isotope.
Solid Ba(NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form ? (Ksp for Ba CO3 = 5.1 × 10-9) [AIEEE-2009] - a)5.1 × 10-5 M
- b)8.1 × 10-8 M
- c)8.1 × 10-7 M
- d)4.1 × 10-5 M
Correct answer is option 'A'. Can you explain this answer?
Solid Ba(NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form ? (Ksp for Ba CO3 = 5.1 × 10-9) [AIEEE-2009]
a)
5.1 × 10-5 M
b)
8.1 × 10-8 M
c)
8.1 × 10-7 M
d)
4.1 × 10-5 M
|
Madhurima Dasgupta answered |
Solubility product of silver bromide is 5.0 x 10-13. The quantity of potassium bromide (molar mass taken as 120 g mol-1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is [AIEEE-2010] - a)5.0 x 10-8 g
- b)1.2 x 10-10 g
- c)1.2 x 10-9 g
- d)6.2 x 10-5 g
Correct answer is option 'C'. Can you explain this answer?
Solubility product of silver bromide is 5.0 x 10-13. The quantity of potassium bromide (molar mass taken as 120 g mol-1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is [AIEEE-2010]
a)
5.0 x 10-8 g
b)
1.2 x 10-10 g
c)
1.2 x 10-9 g
d)
6.2 x 10-5 g
|
Stuti Joshi answered |
To start the precipitation of AgBr, we need to add an appropriate amount of potassium bromide (KBr) to a solution of silver nitrate (AgNO3). The solubility product of silver bromide (AgBr) is given as 5.0 x 10^-13.
Let's calculate the number of moles of Ag+ ions in 1 liter of 0.05 M silver nitrate solution.
Number of moles of Ag+ = Molarity x Volume
= 0.05 mol/L x 1 L
= 0.05 mol
Since the solubility product of AgBr is given as 5.0 x 10^-13, we can write the equilibrium expression for the precipitation of AgBr as follows:
Ag+ + Br- → AgBr
According to the stoichiometry of the reaction, 1 mole of Ag+ reacts with 1 mole of Br-. Therefore, the concentration of Br- ions in the solution will be equal to the concentration of Ag+ ions, which is 0.05 mol/L.
Now, let's calculate the number of moles of KBr required to provide the necessary Br- ions.
Number of moles of KBr = Moles of Br- ions required
= 0.05 mol
The molar mass of KBr is given as 120 g/mol. Using this information, we can calculate the mass of KBr required.
Mass of KBr = Number of moles x Molar mass
= 0.05 mol x 120 g/mol
= 6 g
However, we need to convert this mass to grams because the options are given in grams. The conversion factor between grams and micrograms is 1 g = 10^6 µg.
Therefore, the mass of KBr required in micrograms is:
Mass of KBr = 6 g x 10^6 µg/g
= 6 x 10^6 µg
Comparing this with the given options, we can see that option C is the closest value:
Option C) 1.2 x 10^-9 g
Hence, the correct answer is option C) 1.2 x 10^-9 g.
Let's calculate the number of moles of Ag+ ions in 1 liter of 0.05 M silver nitrate solution.
Number of moles of Ag+ = Molarity x Volume
= 0.05 mol/L x 1 L
= 0.05 mol
Since the solubility product of AgBr is given as 5.0 x 10^-13, we can write the equilibrium expression for the precipitation of AgBr as follows:
Ag+ + Br- → AgBr
According to the stoichiometry of the reaction, 1 mole of Ag+ reacts with 1 mole of Br-. Therefore, the concentration of Br- ions in the solution will be equal to the concentration of Ag+ ions, which is 0.05 mol/L.
Now, let's calculate the number of moles of KBr required to provide the necessary Br- ions.
Number of moles of KBr = Moles of Br- ions required
= 0.05 mol
The molar mass of KBr is given as 120 g/mol. Using this information, we can calculate the mass of KBr required.
Mass of KBr = Number of moles x Molar mass
= 0.05 mol x 120 g/mol
= 6 g
However, we need to convert this mass to grams because the options are given in grams. The conversion factor between grams and micrograms is 1 g = 10^6 µg.
Therefore, the mass of KBr required in micrograms is:
Mass of KBr = 6 g x 10^6 µg/g
= 6 x 10^6 µg
Comparing this with the given options, we can see that option C is the closest value:
Option C) 1.2 x 10^-9 g
Hence, the correct answer is option C) 1.2 x 10^-9 g.
The first and second dissociation constants of an acid H2A are 1.0 x 10-5 & 5.0 x 10-10 respectively. The overall dissociation constant of the acid will be -[AIEEE-2007] - a)5.0 x 10-5
- b)5.0 x 1015
- c)5.0 x 10-15
- d)0.2 x 105
Correct answer is option 'C'. Can you explain this answer?
The first and second dissociation constants of an acid H2A are 1.0 x 10-5 & 5.0 x 10-10 respectively. The overall dissociation constant of the acid will be -
[AIEEE-2007]
a)
5.0 x 10-5
b)
5.0 x 1015
c)
5.0 x 10-15
d)
0.2 x 105
|
|
Ruchi Dasgupta answered |
In order to decide what course the reaction adopts and make a qualitative prediction about the effect of a change in conditions on equilibrium we use- a)Brönsted-Lowry theory,
- b)Arrhenius theory,
- c)Le Chatelier's principle
- d)Lewis theory
Correct answer is option 'C'. Can you explain this answer?
In order to decide what course the reaction adopts and make a qualitative prediction about the effect of a change in conditions on equilibrium we use
a)
Brönsted-Lowry theory,
b)
Arrhenius theory,
c)
Le Chatelier's principle
d)
Lewis theory
|
Anand Khanna answered |
Le Chaterlier principle is used.
A particular ratio of product to reactant helps in predicting the direction in which a given reaction will proceed at any stage. is called- a)reaction quotient,
- b)molecular constant
- c)active mass constant
- d)equilibrium constant
Correct answer is option 'A'. Can you explain this answer?
A particular ratio of product to reactant helps in predicting the direction in which a given reaction will proceed at any stage. is called
a)
reaction quotient,
b)
molecular constant
c)
active mass constant
d)
equilibrium constant
|
Tejas Chawla answered |
A mixture of NH4Cl and NH4OH shows no change in pH upon addition small amount of HCl. This is because it is- a)A neutral solution
- b)A buffer
- c)A basic solution due to presence of NH4OH
- d)An acidic solution due to presence of NH4Cl
Correct answer is option 'B'. Can you explain this answer?
A mixture of NH4Cl and NH4OH shows no change in pH upon addition small amount of HCl. This is because it is
a)
A neutral solution
b)
A buffer
c)
A basic solution due to presence of NH4OH
d)
An acidic solution due to presence of NH4Cl
|
Rajat Patel answered |
A mixture of weak base and its salt with a strong acid serves as an basic buffer which resists changes in pH upon addition of small amount of acid or base.
Which one of the following is the approximate pH of 0.01 M solution of Na OH at 298 k?- a)10-2
- b)2.5
- c)12
- d)2
Correct answer is option 'C'. Can you explain this answer?
Which one of the following is the approximate pH of 0.01 M solution of Na OH at 298 k?
a)
10-2
b)
2.5
c)
12
d)
2
|
|
Rajeev Saxena answered |
First off, since NaOH is a strong base, it will dissociate completely into Na+ and OH-. Thus, we know that we have 0.01 M OH-.
However, we do not know anything about the concentration of H+. Fortunately, we do not need to, as pH + pOH = 14. So, if we find pOH, we can solve for pH. p is a mathematical function equivalent to -log. So, pH actually means -log[H+] (Note that brackets indicate concentration of).
pOH = -log 0.01M OH-
pOH = 2
pH + 2 = 14
pH = 12
This result makes sense, since a solution of strong base should have a high pH.
Ionic product of water is- a)constant above boiling point of water
- b)constant at a particular temperature
- c)constant below freezing point of water
- d)constant at all temperatures
Correct answer is option 'B'. Can you explain this answer?
Ionic product of water is
a)
constant above boiling point of water
b)
constant at a particular temperature
c)
constant below freezing point of water
d)
constant at all temperatures
|
Mira Sharma answered |
The product of concentrations of H1 and OH ions in water at a particular temperature is known as ionic product of water. The value of Kw increases with the increase of temperature, i.e., the concentration of H+ and OH- ions increases with increase in temperature. The value of Kw at 25degreeC is 1 x 10-14.
Which one of the following is correct for a solution in which [H+] = 10-8 M.- a)6, basic
- b)-6, basic
- c)8, basic
- d)-8, neutral
Correct answer is option 'C'. Can you explain this answer?
Which one of the following is correct for a solution in which [H+] = 10-8 M.
a)
6, basic
b)
-6, basic
c)
8, basic
d)
-8, neutral
|
Rishu Singh answered |
U should tell what is here no. representing. If PH-->
PH= -log[H+] = -log 10^-8=8
PH>7So, it is basic.
PH= -log[H+] = -log 10^-8=8
PH>7So, it is basic.
When the soda bottle is opened, some of the dissolved carbon dioxide gas escapes because of- a)some of the undissolved carbon dioxide gas in the soda bottle
- b)difference in solubility of carbon dioxide at different temperatures.
- c)to reach a new equilibrium condition required for the higher pressure,
- d)difference in solubility of carbon dioxide at different pressures.
Correct answer is option 'D'. Can you explain this answer?
When the soda bottle is opened, some of the dissolved carbon dioxide gas escapes because of
a)
some of the undissolved carbon dioxide gas in the soda bottle
b)
difference in solubility of carbon dioxide at different temperatures.
c)
to reach a new equilibrium condition required for the higher pressure,
d)
difference in solubility of carbon dioxide at different pressures.
|
Aravind Nambiar answered |
As P decreases solubility of gas also decreases (Henrys Law)
For liquid ⇌vapour equilibrium, at a given temperature, the constant is- a)mass of a gas
- b)solubility
- c)vapour pressure
- d)mass of a solvent
Correct answer is option 'C'. Can you explain this answer?
For liquid ⇌vapour equilibrium, at a given temperature, the constant is
a)
mass of a gas
b)
solubility
c)
vapour pressure
d)
mass of a solvent
|
Ashish Roy answered |
Explanation:
Equilibrium in Liquid-Vapor System:
- In a liquid-vapor system, equilibrium is established between the liquid phase and the vapor phase.
- This equilibrium is governed by the relationship between the liquid phase and the vapor phase at a given temperature.
Constant for Liquid-Vapor Equilibrium:
- The constant that is associated with liquid-vapor equilibrium at a given temperature is the vapor pressure.
- Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system.
Significance of Vapor Pressure:
- Vapor pressure is a measure of a substance's tendency to vaporize.
- It represents the pressure exerted by the vapor when the liquid and vapor are in equilibrium.
- At equilibrium, the rate of condensation of vapor molecules to the liquid phase is equal to the rate of evaporation of liquid molecules to the vapor phase.
Relation to Temperature:
- Vapor pressure is dependent on temperature.
- As the temperature increases, the vapor pressure also increases due to higher kinetic energy of molecules in the liquid phase leading to more molecules escaping into the vapor phase.
Conclusion:
- In conclusion, the constant associated with liquid-vapor equilibrium at a given temperature is the vapor pressure. It plays a crucial role in determining the equilibrium between the liquid and vapor phases in a system.
The following equilibrium exists in aqueous solutionCH3COOH 
CH3COO- + H+
If dilute HCl is added:- a)Acetate ion concentration will increase
- b)Acetate ion concentration will decrease
- c)The equilibrium constant will decrease
- d)The equilibrium constant will increase.
Correct answer is option 'B'. Can you explain this answer?
The following equilibrium exists in aqueous solution
CH3COOH CH3COO- + H+
If dilute HCl is added:
CH3COO- + H+If dilute HCl is added:
a)
Acetate ion concentration will increase
b)
Acetate ion concentration will decrease
c)
The equilibrium constant will decrease
d)
The equilibrium constant will increase.
|
|
Sahana Marigoudar answered |
H+ concentration increases which makes the reaction to proceed through reverse direction due to which acetic acid concentration increases.
If we place solid iodine in a closed vessel, after sometime the vessel gets filled up with violet vapour. When equilibrium is attained, the intensity of colour will be- a)no colour at all
- b)constant
- c)ecreases
- d)increases
Correct answer is option 'B'. Can you explain this answer?
If we place solid iodine in a closed vessel, after sometime the vessel gets filled up with violet vapour. When equilibrium is attained, the intensity of colour will be
a)
no colour at all
b)
constant
c)
ecreases
d)
increases
|
Mihir Patel answered |
since at eqm conc of reactant and product doesnot change therefore intensity of color did not change.
Given
(i) 
(ii) 
These equilibria show the following order of the relative base strength,- a)
- b)
- c)
- d)
Correct answer is option 'B'. Can you explain this answer?
Given
(i)
(ii)
These equilibria show the following order of the relative base strength,
(i)
(ii)
These equilibria show the following order of the relative base strength,
a)
b)
c)
d)
|
Tarun Kaushik answered |
The more is the value of equilibrium constant, the more is the completion of reaction or more is the concentration of products i.e. the order of relative strength would be
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