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Chapter 15: Problem 113

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the \(\mathrm{pH}\) of the following solutions. (a) \(0.45 M \mathrm{NaCl}\) (b) \(0.18 M \mathrm{BaF}_{2}\) (c) \(0.25 \mathrm{M} \mathrm{KHSO}_{4}\) (d) \(0.33 \mathrm{M} \mathrm{NaNO}_{2}\)

Short Answer

Expert verified
(a) Neutral, (b) Weakly basic, (c) Weakly acidic, (d) Weakly basic.

Step by step solution

01

Analyze the Nature of NaCl

Sodium chloride (NaCl) is a salt formed from a strong acid (HCl) and a strong base (NaOH). Therefore, it does not affect the pH significantly, making the solution neutral.
02

Analyze the Nature of BaF2

Barium fluoride (BaF2) is a salt where barium is derived from a strong base (Ba(OH)2) and fluoride is derived from a weak acid (HF). Fluoride ions can undergo hydrolysis to form OH-, making BaF2 a weakly basic solution.
03

Analyze the Nature of KHSO4

Potassium hydrogen sulfate (KHSO4) releases HSO4- ions, which can dissociate to release H+ ions, making the solution acidic. Therefore, the solution is weakly acidic due to partial dissociation.
04

Analyze the Nature of NaNO2

Sodium nitrite (NaNO2) is a salt formed from a weak acid (HNO2) and a strong base (NaOH). The NO2- ion can undergo hydrolysis to produce OH- ions, making the solution weakly basic.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Solution Chemistry
Solution chemistry involves studying how different substances interact when dissolved in solvents, typically water. It focuses on aspects such as concentration, solubility, and how salts can dissociate into ions. Understanding solution chemistry is crucial because it influences the properties of the solutions such as conductivity, boiling point, and acidity.
  • Concentration: It's the amount of solute present in a given quantity of solvent or solution. Concentration is often expressed in terms of molarity (M), which is moles of solute per liter of solution.
  • Solubility: It refers to the maximum amount of solute that can dissolve in a solvent at a specific temperature. Solubility can affect solution formation, and it's pivotal in predicting whether a substance will form an acid, base, or neutral solution upon dissolution.
  • Dissociation: When salts dissolve, they split into their respective ions. This affects the pH, as these ions can contribute to acidity or basicity, depending on their interaction with water.
By understanding these foundational aspects, students can predict how different compounds will behave once dissolved.
Acid-Base Reactions
Acid-base reactions are chemical reactions involving the transfer of protons ( H^+ ) between reactants. These reactions are essential in solution chemistry because they influence the solution's pH.
  • Acids: Substances that donate protons in a solution. Their dissociation increases H^+ concentration, often lowering the pH.
  • Bases: Compounds that accept protons. They increase the OH^- ion concentration, raising the pH of the solution.
In the context of the exercise: - Strong acids and bases dissociate completely, whereas weak acids and bases do not fully dissociate. - NaCl is neutral because both NaOH and HCl dissociate completely and neutralize each other. - BaF_2 is weakly basic due to partial fluoride ion hydrolysis, forming OH^- ions. - KHSO_4 is weakly acidic as it releases HSO_4^- ions, which partially dissociate to release H^+ ions.
Chemical Analysis
Chemical analysis involves examining substances to understand their chemical properties and composition. For instance, by analyzing the ion composition in solutions, one can estimate pH and predict behavior in reactions.
  • Qualitative Analysis: This focuses on identifying the types of ions or molecules present in the solution. Knowing which ions are present helps determine whether the solution is acidic, basic, or neutral.
  • Quantitative Analysis: Measuring the concentration of ions to understand the extent of dissociation and consequently the effect on pH.
In the case of BaF_2 : - The analysis involves recognizing that the Ba^{2+} cation and F^- anion come from a strong base and a weak acid. This knowledge reveals the weak basic nature due to hydrolysis of fluoride ions producing OH^- ions. The meticulous examination of these ions helps predict the overall behavior and properties of solutions accurately.
Dissociation Reactions
Dissociation reactions play a critical role in understanding how compounds affect the pH when dissolved in water. Dissociation involves breaking down a compound into its ions, which can subsequently influence the acidity or basicity of the solution.
  • Complete Dissociation: Strong acids and bases dissociate fully in solution, contributing to maximum possible H^+ or OH^- ions, making them fully influence the solution's pH.
  • Partial Dissociation: Weak acids and bases do not dissociate completely. This incomplete dissociation results in a less dramatic change in the pH, contributing to the weakly acidic or basic nature of the solution.
For example: - In KHSO_4 , the partial dissociation of HSO_4^- ions hints at its weakly acidic nature. - In NaNO_2 , NO_2^- ions undergo hydrolysis forming OH^- , reflecting its weakly basic characteristic. Recognizing and understanding these dissociation processes help in estimating the pH and predicting the chemical behavior of solutions.

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Most popular questions from this chapter

Identify the Lewis acid and the Lewis base in each reaction. (a) \(\mathrm{I}_{2}(\mathrm{~s})+\mathrm{I}^{-}(\mathrm{aq}) \rightarrow \mathrm{I}_{3}^{-}(\mathrm{aq})\) (b) \(\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{BF}_{3}(\mathrm{~g}) \rightarrow \mathrm{O}_{2} \mathrm{SBF}_{3}(\mathrm{~s})\) (c) \(\mathrm{Au}^{+}(\mathrm{aq})+2 \mathrm{CN}^{-}(\mathrm{aq}) \rightarrow\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})\) (d) \(\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{CO}_{3}(\) aq \()\)

Hydroxylamine, \(\mathrm{NH}_{2} \mathrm{OH},\) is a weak base with \(K_{\mathrm{b}}=\) \(8.7 \times 10^{-9} .\) Fill in the iCe table and write the equation needed to solve for the concentration of hydroxide ion in a \(0.10 M\) solution.

Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is \(\mathrm{NaNH}_{2}\) an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the \(\mathrm{pH}\) of the following solutions. (a) \(0.30 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) (b) \(0.15 \mathrm{M} \mathrm{N}_{2} \mathrm{H}_{5} \mathrm{Cl}\) (c) \(0.50 \mathrm{M} \mathrm{KNO}_{3}\) (d) \(0.50 \mathrm{M} \mathrm{HCOONa}\)

Rank the following species in order of increasing acidity: \(\mathrm{CH}_{3} \mathrm{COOH}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HCOOH}, \mathrm{F}^{-}\)
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