Calculating the pH of Salt Solutions: Fun Questions and Answers

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carly

2/17/2023

AP Chemistry

Acid-Base Properties of Salts

Subjects

AP Chemistry

Acids and Bases

PH and POH of Strong Acids and Bases

Calculating the pH of Salt Solutions: Fun Questions and Answers

Estimating pH of salts from cation and anion dissociation is a crucial concept in chemistry. This guide explores how to determine if a salt solution is acidic, basic, or neutral based on its constituent ions.

Salts can produce acidic, basic, or neutral solutions when dissolved in water
The pH of a salt solution depends on the strength of the acid and base that formed it
Conjugate bases of weak acids tend to make solutions more basic
Conjugate acids of weak bases tend to make solutions more acidic
Group I and II metal ions generally produce neutral cations

2/17/2023

Acid-Base Properties of salts:
salts
-
Dissociation Equations:
HCI → H+ + CIT
conj.
base
a lot
Strong
acid
very little
HCN → H* + CN-
conj.

Analyzing Salt Solutions

This page delves deeper into the pH effects of salt dissociation in water, providing specific examples of salt solutions and their pH characteristics.

The page starts by examining several salt solutions:

KNO₂: K+ $neutral$ and NO₂⁻ $basic$ , resulting in a basic solution
NaNO₃: Na+ $neutral$ and NO₃⁻ $neutral$ , resulting in a neutral solution
NH₄Cl: NH₄+ $acidic$ and Cl⁻ $neutral$ , resulting in an acidic solution
NH₄CN: NH₄+ $acidic$ and CN⁻ $basic$ , resulting in a solution where the pH depends on the relative strengths of the ions

Example: CH₃NH₃ClO₄ dissociates into CH₃NH₃+ $acidic$ and ClO₄⁻ $neutral$ , resulting in an acidic solution.

The page also introduces the concept of relative strengths of conjugate acid-base pairs:

Highlight: The strength relationship between conjugate acid-base pairs is given by the equation Ka × Kb = Kw, where Kw is the ion product of water.

Examples are provided to illustrate this concept:

For NH₃: Kb = 1.8 × 10⁻⁵, so its conjugate acid $NH₄+$ has Ka = 5.6 × 10⁻¹⁰
For HCN: Ka = 6.2 × 10⁻¹⁰, so its conjugate base $CN⁻$ has Kb = 1.6 × 10⁻⁵

This information is essential for calculating the pH of a salt solution and understanding the pH of salt in water. It also helps in determining whether a salt is acid dangerous or not, depending on its pH in solution.

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Subjects

AP Chemistry

Acids and Bases

PH and POH of Strong Acids and Bases

AP Chemistry

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Feb 17, 2023

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Calculating the pH of Salt Solutions: Fun Questions and Answers

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Salts can produce acidic, basic,... Show more

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Analyzing Salt Solutions

This page delves deeper into the pH effects of salt dissociation in water, providing specific examples of salt solutions and their pH characteristics.

The page starts by examining several salt solutions:

KNO₂: K+ $neutral$ and NO₂⁻ $basic$ , resulting in a basic solution
NaNO₃: Na+ $neutral$ and NO₃⁻ $neutral$ , resulting in a neutral solution
NH₄Cl: NH₄+ $acidic$ and Cl⁻ $neutral$ , resulting in an acidic solution
NH₄CN: NH₄+ $acidic$ and CN⁻ $basic$ , resulting in a solution where the pH depends on the relative strengths of the ions

Example: CH₃NH₃ClO₄ dissociates into CH₃NH₃+ $acidic$ and ClO₄⁻ $neutral$ , resulting in an acidic solution.

The page also introduces the concept of relative strengths of conjugate acid-base pairs:

Highlight: The strength relationship between conjugate acid-base pairs is given by the equation Ka × Kb = Kw, where Kw is the ion product of water.

Examples are provided to illustrate this concept:

For NH₃: Kb = 1.8 × 10⁻⁵, so its conjugate acid $NH₄+$ has Ka = 5.6 × 10⁻¹⁰
For HCN: Ka = 6.2 × 10⁻¹⁰, so its conjugate base $CN⁻$ has Kb = 1.6 × 10⁻⁵

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Acid-Base Properties of Salts

This page introduces the fundamental concepts of salt dissociation in water and its effect on pH. It explains how to predict the acidity or basicity of salt solutions based on their constituent ions.

Definition: Salts are ionic compounds formed from the neutralization reaction between an acid and a base.

The dissociation equations of acids are presented, showing how strong and weak acids behave differently in solution. For example:

Example: HCl → H+ + Cl- $strong acid, dissociates completely$ Example: HCN → H+ + CN- $weak acid, dissociates partially$

The page emphasizes that the strength of conjugate acids and bases is inversely related to their parent compounds.

Highlight: Anions that are conjugates of weak acids tend to be basic, while cations that are conjugates of weak bases tend to be acidic.

Vocabulary: Conjugate base - the species formed when an acid loses a proton.

The acidity, basicity, or neutrality of various ions is discussed:

NO₂⁻ is basic $conjugate of a weak acid$
Na+ is neutral $Group I metal ion$
NH₄+ is acidic $conjugate of a weak base$
ClO₄⁻ is neutral $conjugate of a strong acid$

Quote: "Some conjugate bases are strong & act like a base, doesn't do a good job @ accepting H+"

This information is crucial for understanding the pH of salt solutions and predicting whether a salt is acid or base or neutral.

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Calculating the pH of Salt Solutions: Fun Questions and Answers

Analyzing Salt Solutions

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Calculating the pH of Salt Solutions: Fun Questions and Answers

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Analyzing Salt Solutions

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Acid-Base Properties of Salts

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