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Chapter 17: Problem 84

Arrange the following \(0.10 \mathrm{M}\) solutions in order of increasing pH. (a) \(\mathrm{NaCl}\) (b) \(\mathrm{NH}_{4} \mathrm{Cl}\) (c) \(\mathrm{HCl}\) (d) \(\mathrm{NaCH}_{3} \mathrm{CO}_{2}\) (e) \(\mathrm{KOH}\)

Short Answer

Expert verified
The order is (c) HCl, (b) NH鈧凜l, (a) NaCl, (d) NaCH鈧僀O鈧�, (e) KOH.

Step by step solution

01

Understanding pH

The pH scale is a measure of how acidic or basic a solution is. A pH less than 7 indicates an acidic solution, pH equal to 7 is neutral, and a pH greater than 7 indicates a basic solution.
02

Analyze Each Compound

- **NaCl**: A neutral salt formed from a strong acid (HCl) and strong base (NaOH), resulting in a pH around 7. - **NH鈧凜l**: An acidic salt from a strong acid (HCl) and a weak base (NH鈧�), resulting in a pH less than 7. - **HCl**: A strong acid, giving a very low pH. - **NaCH鈧僀O鈧�**: A basic salt formed from a weak acid (CH鈧僀OOH) and a strong base (NaOH), resulting in a pH greater than 7. - **KOH**: A strong base with a very high pH.
03

Order by Increasing pH

Arrange the solutions from lowest to highest pH: (c) HCl, (b) NH鈧凜l, (a) NaCl, (d) NaCH鈧僀O鈧�, (e) KOH. This order is based on the strength and nature of the acids and bases each compound forms.

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Key Concepts

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

Acidic Solutions
Acidic solutions are those with a pH less than 7. These solutions arise due to the presence of compounds that release hydrogen ions \( H^+ \) into the water. For example, hydrochloric acid (HCl) is a strong acid that completely dissociates in water, thus releasing a large amount of \( H^+ \), resulting in a very low pH.

Here are some key characteristics of acidic solutions:
  • They taste sour and can turn blue litmus paper red.
  • Acidic solutions can conduct electricity because of the ions in the solution.
  • They react with metals to produce hydrogen gas.
Understanding these properties helps us recognize substances that may behave as acids in different environments.
Basic Solutions
Basic solutions have a pH greater than 7. Such solutions are formed when substances release hydroxide ions \( OH^- \) into the solution. An example is potassium hydroxide (KOH), a strong base that dissociates completely in water to provide \( OH^- \), thereby increasing the pH significantly.

Key traits of basic solutions include:
  • A bitter taste and slippery feel.
  • The ability to turn red litmus paper blue, indicating their basic nature.
  • They can neutralize acids, forming water and salt.
These properties allow bases to be used in cleaning products, soaps, and as antacids to neutralize excess stomach acid.
Neutral Solutions
Neutral solutions have a pH that equals exactly 7. This occurs when the concentration of hydrogen ions \( H^+ \) is equal to the concentration of hydroxide ions \( OH^- \). A common example is pure water, where this balance exists naturally.

Some key points about neutral solutions:
  • They do not change the color of litmus paper, as they are neither acidic nor basic.
  • In neutralization reactions, an acid and base combine to form such solutions.
  • Neutral solutions are generally non-corrosive and safe for many uses.
A vital concept in chemistry, neutrality implies a balance, making these solutions central in various chemical reactions and daily processes.
Strong Acids and Bases
Strong acids and bases dissociate completely in water, resulting in maximum production of \( H^+ \) for acids and \( OH^- \) for bases. HCl is a strong acid, contributing to an extremely low pH, while KOH is a strong base with a very high pH in solutions.

Characteristics of strong acids and bases:
  • They typically have extreme pH values, either very low or very high.
  • Strong acids and bases conduct electricity very well due to the high ion concentration.
  • They are highly reactive and must be handled with care.
These substances are pivotal in industrial processes, where high reactivity is essential, such as in cleaning, food processing, and research applications.
Weak Acids and Bases
Weak acids and bases do not fully dissociate in water, meaning only a fraction of their molecules release \( H^+ \) or \( OH^- \). Ammonium chloride (NH鈧凜l) is an example of a compound that, when dissolved, contributes to a solution being weakly acidic. Similarly, sodium acetate (NaCH鈧僀O鈧�) forms a weakly basic solution.

Some highlights about weak acids and bases include:
  • They have pH values close to 7, either slightly below or above.
  • Weak acids and bases conduct electricity poorly compared to their strong counterparts.
  • They react more gradually and are less aggressive in nature.
Due to their mild nature, weak acids and bases find use in biological systems and food products, such as maintaining the pH of blood and adding flavor to culinary dishes.

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Most popular questions from this chapter

A saturated solution of milk of magnesia, \(\mathrm{Mg}(\mathrm{OH})_{2},\) has a pH of \(10.52 .\) What is the hydronium ion concentration of the solution? What is the hydroxide ion concentration? Is the solution acidic or basic?

Carbon monoxide forms complexes with low-valent metals. For example, \(\mathrm{Ni}(\mathrm{CO})_{4}\) and \(\mathrm{Fe}(\mathrm{CO})_{5}\) are well known. CO also forms complexes with the iron(II) ion in hemoglobin, which prevents the hemoglobin from acting in its normal way. Is CO a Lewis acid or a Lewis base?

A \(2.5 \times 10^{-3} \mathrm{M}\) solution of an unknown acid has a \(\mathrm{pH}\) of 3.80 at \(25^{\circ} \mathrm{C}\). (a) What is the hydronium ion concentration of the solution? (b) Is the acid a strong acid, a moderately weak acid \((K_{\mathrm{a}}.\) of about \(10^{-5}\) ), or a very weak acid \((K_{\mathrm{a}}\) of. about \(10^{-10}) ?\)

A \(2.50-\mathrm{g}\) sample of a solid that could be \(\mathrm{Ba}(\mathrm{OH})_{2}\) or \(\mathrm{Sr}(\mathrm{OH})_{2}\) was dissolved in enough water to make \(1.00 \mathrm{L}\) of solution. If the \(\mathrm{pH}\) of the solution is \(12.61,\) what is the identity of the solid?

Several acids are listed here with their respective equilibrium constants. $$\begin{aligned} &\mathrm{HF}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq})\\\ &K_{\mathrm{a}}=7.2 \times 10^{-4} \end{aligned}$$ $$\begin{aligned} &\mathrm{HPO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{PO}_{4}^{3-}(\mathrm{aq})\\\ &K_{\mathrm{a}}=3.6 \times 10^{-13} \end{aligned}$$ $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CH}_{3} \mathrm{CO}_{2}^{-}(\mathrm{aq})\\\ &K_{\mathrm{a}}=1.8 \times 10^{-5} \end{aligned}$$ (a) Which is the strongest acid? Which is the weakest acid? (b) What is the conjugate base of the acid HF? (c) Which acid has the weakest conjugate base? (d) Which acid has the strongest conjugate base?
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