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Questions and Answers
What are the conjugate bases for the Bronsted acids H2O and HF?
What are the conjugate bases for the Bronsted acids H2O and HF?
What is the conjugated acid of the O–2 ion?
What is the conjugated acid of the O–2 ion?
In the reaction NH3 + H2O → NH4+ + OH–, what role does water play?
In the reaction NH3 + H2O → NH4+ + OH–, what role does water play?
Which of the following can act both as a Bronsted acid and a Bronsted base?
Which of the following can act both as a Bronsted acid and a Bronsted base?
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In the equilibrium NH3 + H2O ⇌ NH4+ + OH–, identify X and Y in terms of conjugate acid and base.
In the equilibrium NH3 + H2O ⇌ NH4+ + OH–, identify X and Y in terms of conjugate acid and base.
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Which of the following is least likely to behave as a Lewis base?
Which of the following is least likely to behave as a Lewis base?
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Which compound is considered the weakest acid?
Which compound is considered the weakest acid?
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For which substance is the dilution law applicable?
For which substance is the dilution law applicable?
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If [OH–] = 5.0 × 10–5 M, what is the pH of the solution?
If [OH–] = 5.0 × 10–5 M, what is the pH of the solution?
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What is the pOH of a 0.002 M HNO3 solution?
What is the pOH of a 0.002 M HNO3 solution?
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What is the calculated pH of a 0.01 M NaOH solution?
What is the calculated pH of a 0.01 M NaOH solution?
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Given a hydroxide ion concentration of 8 × 10–11 M, what is the pH of the solution?
Given a hydroxide ion concentration of 8 × 10–11 M, what is the pH of the solution?
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From a pH of 3.31, what is the approximate concentration of [H+]?
From a pH of 3.31, what is the approximate concentration of [H+]?
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What is the [H3O+] concentration in a beer with a pH of 4.30?
What is the [H3O+] concentration in a beer with a pH of 4.30?
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What is the pH of a solution if 2g of NaOH is dissolved to make 1 L?
What is the pH of a solution if 2g of NaOH is dissolved to make 1 L?
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For a 100 ml solution of 10–2 M NaOH, what is the ratio of pH to pOH?
For a 100 ml solution of 10–2 M NaOH, what is the ratio of pH to pOH?
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What is the H+ ion concentration of a 5 × 10-3 M H2CO3 solution with 10% dissociation?
What is the H+ ion concentration of a 5 × 10-3 M H2CO3 solution with 10% dissociation?
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If the pH of a 0.1 M weak acid is 3, what is its degree of dissociation?
If the pH of a 0.1 M weak acid is 3, what is its degree of dissociation?
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For 10–3 M H3PO3 with α = 10%, what is the expected pH?
For 10–3 M H3PO3 with α = 10%, what is the expected pH?
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Calculate the Ka for a 10–2 M HCN solution that has a pOH of 10.
Calculate the Ka for a 10–2 M HCN solution that has a pOH of 10.
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What would be the [H+] concentration of a 0.006 M benzoic acid (Ka = 6 × 10–5)?
What would be the [H+] concentration of a 0.006 M benzoic acid (Ka = 6 × 10–5)?
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The pKb for fluoride ion at 25°C is 10.83. What is the ionization constant for hydrofluoric acid at this temperature?
The pKb for fluoride ion at 25°C is 10.83. What is the ionization constant for hydrofluoric acid at this temperature?
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What is the concentration of OH- ions in a 0.01 M ammonia solution that is 5% ionized?
What is the concentration of OH- ions in a 0.01 M ammonia solution that is 5% ionized?
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Calculate the molarity of nitrous acid at which its pH becomes 2 (Ka = 4.5 × 10–4).
Calculate the molarity of nitrous acid at which its pH becomes 2 (Ka = 4.5 × 10–4).
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Precipitation of AgCl will occur when equal volumes of which mixture are combined, given that its Ksp is 1.8 × 10–10?
Precipitation of AgCl will occur when equal volumes of which mixture are combined, given that its Ksp is 1.8 × 10–10?
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At what pH will Mg2+ ions begin to precipitate as Mg(OH)2 from a 0.001 M solution, given its Ksp is 1.0 × 10–11?
At what pH will Mg2+ ions begin to precipitate as Mg(OH)2 from a 0.001 M solution, given its Ksp is 1.0 × 10–11?
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When 15 mL of 0.05 M AgNO3 is mixed with 45.0 mL of 0.03 M K2CrO4, will precipitation of Ag2CrO4 occur given its Ksp is 1.9 × 10–12?
When 15 mL of 0.05 M AgNO3 is mixed with 45.0 mL of 0.03 M K2CrO4, will precipitation of Ag2CrO4 occur given its Ksp is 1.9 × 10–12?
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Which option represents the correct increasing order of solubility for the given solubility products?
Which option represents the correct increasing order of solubility for the given solubility products?
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What is the concentration of CO32– ions when water reaches equilibrium with both CaCO3 and BaCO3, given their Ksp values?
What is the concentration of CO32– ions when water reaches equilibrium with both CaCO3 and BaCO3, given their Ksp values?
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What percentage of dimethylamine is ionized in a 0.02 M solution when the ionization constant is 5.4 × 10–4?
What percentage of dimethylamine is ionized in a 0.02 M solution when the ionization constant is 5.4 × 10–4?
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What is the pH of a buffer solution containing 0.250 M benzoic acid and 0.150 M sodium benzoate with a Ka of 6.5 × 10–5?
What is the pH of a buffer solution containing 0.250 M benzoic acid and 0.150 M sodium benzoate with a Ka of 6.5 × 10–5?
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What is the concentration of phenolate ion in a 0.05 M solution of phenol given its ionization constant is 1.0 × 10–10?
What is the concentration of phenolate ion in a 0.05 M solution of phenol given its ionization constant is 1.0 × 10–10?
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What is a characteristic of a buffer solution?
What is a characteristic of a buffer solution?
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Which buffer system maintains the pH of blood at around 7.4?
Which buffer system maintains the pH of blood at around 7.4?
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Calculate [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.1 M in CH3COOH, given that Ka for CH3COOH is 1.8 × 10–5.
Calculate [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.1 M in CH3COOH, given that Ka for CH3COOH is 1.8 × 10–5.
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For a desired pH of 6 using sodium acetate and acetic acid, what is the proper ratio of salt to acid (where Ka = 10–5)?
For a desired pH of 6 using sodium acetate and acetic acid, what is the proper ratio of salt to acid (where Ka = 10–5)?
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What is the pH of a buffer solution containing 0.1M HCN (pKa = 9.30) and 0.2 M NaCN?
What is the pH of a buffer solution containing 0.1M HCN (pKa = 9.30) and 0.2 M NaCN?
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What is the approximate pH of a solution made from 10 ml of 1N sodium acetate and 50 ml of 2N acetic acid (Ka = 1.8 × 10–5)?
What is the approximate pH of a solution made from 10 ml of 1N sodium acetate and 50 ml of 2N acetic acid (Ka = 1.8 × 10–5)?
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What is the pOh of a solution composed of 0.1 M NH4OH and 0.1 M NH4Cl which has a pH of 9.25?
What is the pOh of a solution composed of 0.1 M NH4OH and 0.1 M NH4Cl which has a pH of 9.25?
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If the concentration ratio of a weak acid and its salt increases ten-fold, how does the pH of the solution change?
If the concentration ratio of a weak acid and its salt increases ten-fold, how does the pH of the solution change?
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What is the pH of pure H2O?
What is the pH of pure H2O?
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Which of the following is classified as an acid salt?
Which of the following is classified as an acid salt?
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What will be the pH of a 1.0 M ammonium formate solution if Ka = 1 × 10–4 and Kb = 1 × 10–5?
What will be the pH of a 1.0 M ammonium formate solution if Ka = 1 × 10–4 and Kb = 1 × 10–5?
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Which salt listed will not undergo hydrolysis?
Which salt listed will not undergo hydrolysis?
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What is the correct formula for calculating pH in anionic hydrolysis?
What is the correct formula for calculating pH in anionic hydrolysis?
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If pKb for CN at 25°C is 4.7, what is the expected pH of a 0.5M aqueous NaCN solution?
If pKb for CN at 25°C is 4.7, what is the expected pH of a 0.5M aqueous NaCN solution?
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What is the relationship between the Ksp values of salts M2X, QY2, and PZ2 when their solubilities are equal?
What is the relationship between the Ksp values of salts M2X, QY2, and PZ2 when their solubilities are equal?
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If the pH of a solution increases from 3 to 6, how will the H+ ion concentration change?
If the pH of a solution increases from 3 to 6, how will the H+ ion concentration change?
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Study Notes
Ionic Equilibrium Questions for NEET 2025
- This material contains questions on ionic equilibrium, a topic in physical chemistry relevant to the NEET 2025 exam.
- The questions cover various concepts, including conjugate base/acid identification, Bronsted acid/base behavior, Lewis acid/base definitions, and calculations of pH/pOH values.
- Key concepts include the identification of conjugate bases associated with water and hydrofluoric acid, the definition of conjugated acid of an ion, identification of conjugate base for a reactant in a certain reaction and identifying a Bronsted acid/base. Additional questions cover how water can act both as an acid and a base, how to solve for pH or pOH given certain concentrations.
- Solutions to these questions are available in the accompanying class notes PDF. Students are advised not to seek answers directly.
Additional Notes
- Note that different types of acid/base problems require different methodologies: Bronsted and Lewis acids/bases require identification of proton donation and electron pair acceptance, and questions regarding ion concentration or hydrolysis are tackled using appropriate formulas. These may include the use of the dissociation constant or other related constants.
- The study material includes various problem types, requiring diverse approaches and formulas. The use of logarithm based calculations are also important.
- Solutions to the questions are in separate PDF notes.
- The study material is designed to help students practice and prepare for problem-solving in ionic equilibrium. A multitude of problems are presented, spanning multiple problem types, and requiring an understanding of formulas and methodologies related to different types of acid/base problems.
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Description
Test your knowledge on Bronsted acids, bases, and their conjugates. This quiz covers essential concepts such as acid-base reactions, pH calculations, and the properties of various substances. Hone your understanding of acidity and basicity in aqueous solutions.
