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Chapter 15: Problem 114

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) \(0.50 \mathrm{M} \mathrm{HCOONa}\)

Short Answer

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

Step by step solution

01

Identify the Nature of the Solution

For each compound, examine whether it can cause the solution to be acidic, neutral, or basic. This is based on the potential donation or acceptance of \( ext{H}^+ \) ions.
02

Determine the pH for NH4Cl Solution

Ammonium chloride (NH4Cl) is derived from a weak base (NH3) and a strong acid (HCl). It tends to make the solution acidic because of the hydrolysis of NH4+. Therefore, the solution is weakly acidic.
03

Determine the pH for N2H5Cl Solution

Hydrazinium chloride (N2H5Cl) acts similarly to ammonium chloride, as it is derived from a weak base (N2H4) and a strong acid (HCl). It produces a weakly acidic solution.
04

Determine the pH for KNO3 Solution

Potassium nitrate (KNO3) is derived from a strong base (KOH) and a strong acid (HNO3), neither of which hydrolyzes significantly in water. This means the solution will be neutral.
05

Determine the pH for HCOONa Solution

Sodium formate (HCOONa) is derived from a weak acid (HCOOH) and a strong base (NaOH). It produces a solution that is weakly basic due to the hydrolysis of the formate ion (HCOO-).

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Key Concepts

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

Strong Acid and Weak Base Interactions
When a strong acid such as hydrochloric acid (HCl) reacts with a weak base like ammonia (NH鈧�), they form a salt. In our example, ammonium chloride (NH鈧凜l), is produced.
  • The salt formed from these reactions typically results in a slightly acidic solution.
  • This happens because the ammonium ion ( ext{NH鈧剗^+) can donate a proton ( ext{H}^+), which increases the hydrogen ion concentration in the solution.
  • Thus, even though the base ammonia is weak, the resulting solution from its salt with a strong acid will exhibit more acidic characteristic.
The more substantial the acidic component in these interactions, the more the equilibrium of the formed salt solution favors acidic tendencies.
Acid-Base Hydrolysis
Acid-base hydrolysis is a crucial concept in determining the pH of salts. When salts are dissolved in water, they can sometimes react with water to produce ext{H}^+ or ext{OH}^- ions, depending on their components.
  • For example, when ammonium chloride (NH鈧凜l) dissolves, the ammonium ion undergoes hydrolysis to form ammonia ( ext{NH鈧儅) and ext{H}^+ ions.
  • Similarly, sodium formate (HCOONa) upon dissolution will undergo hydrolysis, where the formate ion (HCOO鈦�) reacts with ext{H}_2 ext{O} to form formic acid (HCOOH) and ext{OH}^- ions.
The hydrolysis reactions are fundamental in predicting whether the solution will tend to be acidic or basic, determining indirectly the resultant pH.
Properties of Ionic Compounds
Ionic compounds such as salts can have varying effects on pH based on their constituting ions.
  • The nature of ions derived from strong acids and bases creates neutral solutions because both kinds dissociate completely and neither reacts significantly with water.
  • Examples include salts like potassium nitrate (KNO鈧�), which is made from a strong base (KOH) and a strong acid (HNO鈧�).
  • On the other hand, salts from a weak base and a strong acid, or vice versa, do affect the pH due to extensive hydrolysis reactions, as seen with ammonium (NH鈧勨伜) or formate ions (HCOO鈦�).
These intrinsic properties of ionic compounds greatly influence their environment when dissolved, characterizing their general behavior in aqueous solutions.
Neutralization Reactions
Neutralization reactions occur when an acid and a base react to form water and a salt. However, the context around these reactions defines the pH of the resultant solution.
  • When a strong acid neutralizes a strong base, such as in the formation of KNO鈧� from HNO鈧� and KOH, the resulting solution is typically neutral.
  • In contrast, the reaction of a strong acid with a weak base or a strong base with a weak acid will not yield a neutral solution.
  • Instead, the final solution tends either towards acidity or basicity, indicative of the more dominant influence of the stronger constituent.
This balance in neutralization reactions is essential in pH estimation when dealing with various combinations of acids and bases in their reactions.

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Most popular questions from this chapter

If \(K_{\mathrm{b}}\) for ammonia is \(1.8 \times 10^{-5},\) calculate \(K_{\mathrm{a}}\) for its conjugate acid, \(\mathrm{NH}_{4}^{+}\). Note that \(\mathrm{NH}_{3}\) is the conjugate acid of the amide ion, \(\mathrm{NH}_{2}^{-}\). Can \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) for the \(\mathrm{NH}_{3} \mid \mathrm{NH}_{2}^{-}\) pair be calculated from the preceding data and the value of \(K_{\mathrm{w}} ?\)

Morphine, \(\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{O}_{3} \mathrm{~N},\) is a weak base with \(K_{\mathrm{b}}=\) \(1.6 \times 10^{-6} .\) It is a prescription drug used to deaden pain; the average dose is \(10 \mathrm{mg}\). Calculate the \(\mathrm{pH}\) of a \(0.0010 M\) solution.

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Br酶nsted-Lowry, and Lewis. (a) \(\cdot \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) (b) \(\mathrm{Zn}(\mathrm{OH})_{3}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}(\mathrm{OH})_{4}^{2-}(\mathrm{aq})\)

Lactic acid, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH},\) forms in muscles as a by-product of their contraction. If the \(\mathrm{pH}\) of a \(0.0376 \mathrm{M}\) solution is \(2.66,\) what is \(K_{\mathrm{a}}\) and \(\mathrm{p} K_{\mathrm{a}}\) for lactic acid?

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) \(0.25 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) (c) \(0.080 \mathrm{M} \mathrm{HI}\) (d) \(0.12 M \mathrm{LiI}\)
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