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Chapters
2: Solutions
▶ 3: Ionic Equilibria
4: Chemical Thermodynamics
5: Electrochemistry
6: Chemical Kinetics
7: Elements of Groups 16, 17 and 18
8: Transition and Inner transition Elements
9: Coordination Compounds
10: Halogen Derivatives
11: Alcohols, Phenols and Ethers
12: Aldehydes, Ketones and Carboxylic acids
13: Amines
14: Biomolecules
15: Introduction to Polymer Chemistry
16: Green Chemistry and Nanochemistry
![Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 3 - Ionic Equilibria - Shaalaa.com](/images/chemistry-english-12-standard-hsc_6:74400b801d4c44ef8e058ff9d9dfe964.jpg "Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 3 - Ionic Equilibria")
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Solutions for Chapter 3: Ionic Equilibria
Below listed, you can find solutions for Chapter 3 of Maharashtra State Board Balbharati for Chemistry [English] 12 Standard HSC.
Balbharati solutions for Chemistry [English] 12 Standard HSC 3 Ionic Equilibria Exercises [Pages 61 - 62]
Choose the most correct answer:
The pH of 10-8 M of HCl is ______.
8
7
less than 7
greater than 7
Choose the most correct answer:
Which of the following solution will have a pH value equal to 1.0?
50 mL of 0.1M HCl + 50mL of 0.1M NaOH
60 mL of 0.1M HCl + 40mL of 0.1M NaOH
20 mL of 0.1M HCl + 80mL of 0.1M NaOH
75 mL of 0.2M HCl + 25mL of 0.2M NaOH
Choose the most correct answer:
Which of the Na following is a buffer solution?
CH3COONa + NaCl in water
CH3COOH + HCl in water
CH3COOH + CH3COONa in water
HCl + NH4Cl in water
Choose the most correct answer :
The solubility product of a sparingly soluble salt AX is 5.2 × 10–13. Its solubility in mol dm–3 is ______.
7.2 × 10–7
1.35 × 10–4
7.2 × 10–8
13.5 × 10–8
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
7.4
7.0
6.9
8.1
Choose the most correct answer :
The conjugate base of [Zn(H2O)4]2⊕ is __________.
[Zn(H2O)4]2-NH3
[Zn(H2O)3]2-
[Zn(H2O)3OH]⊕
[Zn(H2O)H]3⊕
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
10-7M
< 10-7M
> 10-7M
≥ 10-7M
Answer the following in one sentence :
Why cations are Lewis acids?
Answer the following in one sentence :
Why is KCl solution neutral to litmus?
Answer the following in one sentence :
How are basic buffer solutions prepared?
Answer the following in one sentence :
The dissociation constant of acetic acid is 1.8 × 10-5. Calculate percent dissociation of acetic acid in 0.01 M solution.
Answer the following in one sentence :
Write one property of a buffer solution.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H⊕ ion concentration.
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Answer the following in one sentence :
The dissociation of H2S is suppressed in the presence of HCl. Name the phenomenon.
Answer the following in one sentence:
Why is it necessary to add H2SO4 while preparing the solution of CuSO4?
Answer the following in one sentence :
Classify the following buffers into different types :
CH3COOH + CH3COONa
Acidic buffer
Basic buffer
Answer the following in one sentence :
Classify the following buffers into different types :
NH4OH + NH4Cl
Acidic buffer
Basic buffer
Answer the following in one sentence :
Classify the following buffers into different types :
Sodium benzoate + benzoic acid
Acidic buffer
Basic buffer
Answer the following in one sentence :
Classify the following buffers into different types :
Cu(OH)2 + CuCl2
Acidic buffer
Basic buffer
Answer the following in brief :
What are acids and bases according to Arrhenius theory?
Answer the following in brief :
What is meant by conjugate acid-base pair?
Label the conjugate acid-base pair in the following reaction:
\[\ce{HCl + H2O ⇌ H3O\overset{\oplus} + Cl\overset{\ominus}{}}\]
Label the conjugate acid-base pair in the following reaction:
\[\ce{CO^2-_3 + H2O ⇌ OH- + HCO^-_3}\]
Answer the following in brief :
Write a reaction in which water acts as a base.
Answer the following in brief :
Ammonia serves as a Lewis base whereas AlCl3 is Lewis acid. Explain.
Answer the following in brief :
Acetic acid is 5% ionised in its decimolar solution. Calculate the dissociation constant of acid.
Derive the relation pH + pOH = 14.
Answer the following in brief :
The aqueous solution of sodium carbonate is alkaline whereas the aqueous solution of ammonium chloride is acidic. Explain.
Answer the following in brief :
The pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation constant.
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Define the degree of dissociation.
Derive Ostwald's dilution law for the CH3COOH.
Define pH.
Define pOH.
Derive the relation pH + pOH = 14.
Answer the following :
What is meant by hydrolysis?
Answer the following :
A solution of CH3COONH4 is neutral. why?
Answer the following :
The dissociation of HCN is suppressed by the addition of HCl. Explain.
Answer the following :
Derive the relationship between the degree of dissociation and dissociation constant in weak electrolytes.
Answer the following :
Sulfides of the cation of group II are precipitated in acidic solution (H2S + HCl) whereas sulfides of cations of group IIIB are precipitated in the ammoniacal solution of H2S. Comment on the relative values of the solubility product of sulfides of these.
Answer the following :
The solubility of a sparingly soluble salt gets affected in the presence of a soluble salt having one common ion. Explain.
Answer the following :
The pH of rainwater collected in a certain region of Maharashtra on a particular day was 5.1. Calculate the H+ ion concentration of the rainwater and its percent dissociation.
Answer the following :
Explain the relation between ionic product and solubility product to predict whether a precipitate will form when two solutions are mixed?
Solutions for 3: Ionic Equilibria
Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 3 - Ionic Equilibria
Shaalaa.com has the Maharashtra State Board Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board 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. Balbharati solutions for Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board 3 (Ionic Equilibria) 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 [English] 12 Standard HSC chapter 3 Ionic Equilibria are Ionic Equilibria, Types of Electrolyte, Acids and Bases, Ionisation of Acids and Bases, Autoionization of Water, The pH Scale, Hydrolysis of Salts, Buffer Solutions, Solubility product, Common Ion Effect.
Using Balbharati Chemistry [English] 12 Standard HSC solutions Ionic Equilibria 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 Balbharati Solutions are essential questions that can be asked in the final exam. Maximum Maharashtra State Board Chemistry [English] 12 Standard HSC students prefer Balbharati Textbook Solutions to score more in exams.
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