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Chapters
2: p-Block Elements - I
3: p-Block Elements - II
4: Transition and Inner Transition Elements
5: Coordination Chemistry
6: Solid State
7: Chemical Kinetics
▶ 8: Ionic Equilibrium
9: Electro Chemistry
10: Surface Chemistry
11: Hydroxy Compounds and Ethers
12: Carbonyl Compounds and Carboxylic Acids
13: Organic Nitrogen Compounds
14: Biomolecules
15: Chemistry in Everyday Life
![Samacheer Kalvi solutions for Chemistry - Volume 1 and 2 [English] Class 12 TN Board chapter 8 - Ionic Equilibrium - Shaalaa.com](/images/chemistry-volume-1-and-2-english-class-12-tn-board_6:5f2b1b2038084cf381bfa42c826a928c.jpg "Samacheer Kalvi solutions for Chemistry - Volume 1 and 2 [English] Class 12 TN Board chapter 8 - Ionic Equilibrium")
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Solutions for Chapter 8: Ionic Equilibrium
Below listed, you can find solutions for Chapter 8 of Tamil Nadu Board of Secondary Education Samacheer Kalvi for Chemistry - Volume 1 and 2 [English] Class 12 TN Board.
Samacheer Kalvi solutions for Chemistry - Volume 1 and 2 [English] Class 12 TN Board 8 Ionic Equilibrium Evaluation [Pages 28 - 31]
Choose the correct answer:
Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.24 × 10−4 mol L−1 solubility product of Ag2C2O4 is ____________.
2.24 × 10−8 mol3 L−3
2.66 × 10−12 mol3 L−3
4.5 × 10−11 mol3 L−3
5.619 × 10−12 mol3 L−3
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
iv
i
ii
iii
The solubility of BaSO4 in water is 2.42 × 10−3 g L−1 at 298 K. The value of its solubility product (Ksp) will be:
(Given molar mass of BaSO4 = 233 g mol−1)
1.08 × 10−14 mol2 L−2
1.08 × 10−12 mol2 L−2
1.08 × 10−10 mol2 L−2
1.08 × 10−8 mol2 L−2
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
0.5 × 10−15
0.25 × 10−10
0.125 × 10−15
0.5 × 10−10
Conjugate base for Bronsted acids H2O and HF are ___________.
OH– and H2FH+, respectively
H3O+ and F–, respectively
OH– and F–, respectively
H3O+ and H2F+, respectively
Which will make basic buffer?
50 mL of 0.1 M NaOH + 25 mL of 0.1 M CH3COOH
100 mL of 0.1 M CH3COOH + 100 mL of 0.1 M NH4OH
100 mL of 0.1 M HCI + 200 mL of 0.1 M NH4OH
100 mL of 0.1 M HCI + 100 mL of 0.1 M NaOH
Which of the following fluro compounds is most likely to behave as a Lewis base?
BF3
PF3
CF4
SiF4
Which of these is not likely to act as Lewis base?
BF3
PF3
CO
F–
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
acidic, acidic, basic
basic, acidic, basic
basic, neutral, basic
none of these
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5NH) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10−9) is ____________.
0.006%
0.013%
0.77%
1.6%
Equal volumes of three acid solutions of pH 1, 2 and 3 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
3.7 × 10−2
10−6
0.111
none of these
The solubility of AgCl(s) with solubility product 1.6 × 10−10 in 0.1 M NaCl solution would be ____________.
1.26 × 10−5 M
1.6 × 10−9 M
1.6 × 10−11 M
Zero
If the solubility product of lead iodide is 3.2 × 10−8, its solubility will be ____________.
2 × 10−3 M
4 × 10−4 M
1.6 × 10−5 M
1.8 × 10−5 M
MY and NY3, are insoluble salts and have the same Ksp values of 6.2 × 10−13 at room temperature. Which statement would be true with regard to MY and NY?
The salts MY and NY3 are more soluble in 0.5 M KY than in pure water
The addition of the salt of KY to the suspension of MY and NY3 will have no effect on their solubility’s
The molar solubilities of MY and NY3 in water are identical
The molar solubility of MY in water is less than that of NY3
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
2.0
3
7.0
12.65
The dissociation constant of a weak acid is 1 × 10−3. In order to prepare a buffer solution with a pH = 4, the `(["Acid"])/(["Salt"])` ratio should be ____________.
4 : 3
3 : 4
10 : 1
1 : 10
The pH of 10−5 M KOH solution will be ____________.
9
5
19
none of these
\[\ce{H2PO^-_4}\] the conjugate base of ____________.
\[\ce{PO^{3-}_4}\]
P2O5
H3PO4
\[\ce{HPO^{2-}_4}\]
Which of the following can act as Lowry – Bronsted acid as well as base?
HCl
\[\ce{SO^{2-}_4}\]
\[\ce{HPO^{2-}_4}\]
Br−
The pH of an aqueous solution is Zero. The solution is ____________.
slightly acidic
strongly acidic
neutral
basic
The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by ____________.
`["H"^+] = "K"_"a"(["acid"])/(["salt"])`
[H+] = Ka [salt]
[H+] = Ka [acid]
`["H"^+] = "K"_"a"(["salt"])/(["acid"])`
Which of the following relation is correct for degree of hydrolysis of ammonium acetate?
h = `sqrt(("K"_"h")/"C")`
h = `sqrt(("K"_"a")/("K"_"b"))`
h = `sqrt(("K"_"h")/("K"_"a"."K"_"b"))`
h = `sqrt(("K"_"a"."K"_"b")/"K"_"h")`
Dissociation constant of NH4OH is 1.8 × 10−5 the hydrolysis constant of NH4Cl would be ____________.
1.8 × 10−19
5.55 × 10−10
5.55 × 10−5
1.80 × 10−5
Answer the following questions:
What are Lewis acids and bases? Give two examples for each.
Discuss the Lowry – Bronsted concept of acids and bases.
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{HS^-_{( aq)} + HF ⇌ F^-_{( aq)} + H2S_{(aq)}}\]
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{HPO^{2-}_4 + SO^{2-}_3 ⇌ PO^{3-}_4 + HSO^-_3}\]
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{NH^+_4 + CO^{2-}_3 ⇌ NH3 + HCO^-_3}\]
Account for the acidic nature of HClO4 in terms of Bronsted – Lowry theory, identify its conjugate base.
When aqueous ammonia is added to CuSO4 solution, the solution turns deep blue due to the formation of tetramminecopper (II) complex, \[\ce{[Cu(H2O)6]^{2+}_{( aq)} + 4NH3_{( aq)} ⇌ [Cu(NH3)4]^{2+}_{( aq)}}\], among HO2 and NH3 Which is stronger Lewis base.
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
A lab assistant prepared a solution by adding a calculated quantity of HCl gas at 25°C to get a solution with [H3O+]= 4 × 10−5 M. Is the solution neutral (or) acidic (or) basic.
Calculate the pH of 0.04 M HNO3 solution.
Define Solubility product.
Define the ionic product of water. Give its value at room temperature.
Explain the common ion effect with an example.
Derive an expression for Ostwald’s dilution law.
Define pH.
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that Ka = Kb = 1.8 × 10−5
Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.
Solubility product of Ag2CrO4 is 1 × 10−12. What is the solubility of Ag2CrO4 in 0.01 M AgNO3 solution?
Write the expression for the solubility product of Ca3(PO4)2.
A saturated solution, prepared by dissolving CaF2(s) in water, has [Ca2+] = 3.3 × 10−4 M What is the Ksp of CaF2?
Ksp of AgCl is 1.8 × 10−10. Calculate molar solubility in 1 M AgNO3.
A particular saturated solution of silver chromate Ag2CrO4 has [Ag+] = 5 × 10−5 and [CrO4]2− = 4.4 × 10−4 M. What is the value of Ksp for Ag2CrO4?
Write the expression for the solubility product of Hg2Cl2.
Ksp of Ag2CrO4 is 1.1 × 10−12. what is the solubility of Ag2CrO4 in 0.1 M K2CrO4?
Will a precipitate be formed when 0.150 L of 0.1 M Pb(NO3)2 and 0.100 L of 0.2 M NaCl are mixed? Ksp (PbCl2) = 1.2 × 10−5.
Ksp of Al(OH)3 is 1 × 10−15 M. At what pH does 1.0 × 10−3 M Al3+ precipitate on the addition of buffer of NH4Cl and NH4OH solution?
Solutions for 8: Ionic Equilibrium
Samacheer Kalvi solutions for Chemistry - Volume 1 and 2 [English] Class 12 TN Board chapter 8 - Ionic Equilibrium
Shaalaa.com has the Tamil Nadu Board of Secondary Education Mathematics Chemistry - Volume 1 and 2 [English] Class 12 TN Board Tamil Nadu Board of Secondary Education solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. Samacheer Kalvi solutions for Mathematics Chemistry - Volume 1 and 2 [English] Class 12 TN Board Tamil Nadu Board of Secondary Education 8 (Ionic Equilibrium) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
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Concepts covered in Chemistry - Volume 1 and 2 [English] Class 12 TN Board chapter 8 Ionic Equilibrium are Acids and Bases, Strength of Acids and Bases, Ionisation of Water, The pH Scale, Ionisation of Weak Acids, Common Ion Effect, Buffer Solutions, Salt Hydrolysis, Solubility product.
Using Samacheer Kalvi Chemistry - Volume 1 and 2 [English] Class 12 TN Board solutions Ionic Equilibrium exercise by students is an easy way to prepare for the exams, as they involve solutions arranged chapter-wise and also page-wise. The questions involved in Samacheer Kalvi Solutions are essential questions that can be asked in the final exam. Maximum Tamil Nadu Board of Secondary Education Chemistry - Volume 1 and 2 [English] Class 12 TN Board students prefer Samacheer Kalvi Textbook Solutions to score more in exams.
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