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Chapter 17: Problem 53

For each of the following salts, indicate whether the aqueous solution will be acidic, basic, or neutral. a. \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) b. \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) c. \(\mathrm{Ca}(\mathrm{CN})_{2}\) d. \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\)

Short Answer

Expert verified
a. acidic, b. basic, c. basic, d. acidic.

Step by step solution

01

Determine the ions present in the salt

To understand the behavior of the solution, first dissociate each salt into its respective ions. For example, \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) dissociates into \(\mathrm{Fe}^{3+}\) and \(\mathrm{NO}_{3}^{-}\) ions.
02

Identify the nature of each ion

Examine each ion to determine if it will affect the pH of the solution. Cations can be acidic, neutral or basic, while anions can often be acidic or basic. For example, \(\mathrm{Fe}^{3+}\) acts as a weak acid, while \(\mathrm{NO}_{3}^{-}\) is a neutral anion because its conjugate acid, \(\mathrm{HNO}_{3}\), is a strong acid.
03

Predict solution pH for each salt

Use the nature of the ions to determine whether the solution will be acidic, basic, or neutral:- For \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\), the \(\mathrm{Fe}^{3+}\) ion will make the solution acidic.- For \(\mathrm{Na}_{2} \mathrm{CO}_{3}\), \(\mathrm{CO}_{3}^{2-}\) is a basic anion, making the solution basic.- For \(\mathrm{Ca}( ext{CN})_{2}\), \(\mathrm{CN}^{-}\) is a basic anion, making it basic as well.- For \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\), \(\mathrm{NH}_{4}^{+}\) is an acidic cation making the solution acidic.

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Key Concepts

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

Dissociation of Salts
When salts are added to water, they dissolve and break up into their constituent ions. This process is called dissociation. Dissociation is crucial to predict the behavior of salt-based solutions. Let's break it down a bit more.
  • Dissociation process: For example, when \( \text{Fe(NO}_3\text{)}_3 \) is added to water, it dissociates into \( \text{Fe}^{3+} \) and \( \text{NO}_3^- \) ions.
  • Fully dissociated ions: Each ion is now free in the solution to interact with water molecules.
These interactions are fundamental in determining the next step, which is the behavior of each ion, and its subsequent effect on the solution's pH.
Acidic and Basic Ions
The ions resulting from the dissociation of a salt can be categorized as either acidic, basic, or neutral. This categorization determines whether they will have any impact on the pH of a solution.
  • Acidic ions: These are usually metal cations that can donate protons or attract hydroxide ions. Examples include \( \text{Fe}^{3+} \), which is an acidic ion.
  • Basic ions: Typically, these are anions from weak acids that can accept protons or donate hydroxide ions. For instance, \( \text{CO}_3^{2-} \) and \( \text{CN}^- \) are basic ions.
  • Neutral ions: These ions neither donate nor accept protons in significant amounts, hence they hardly affect the pH. An example is \( \text{NO}_3^- \), which comes from the strong acid \( \text{HNO}_3 \).
Understanding whether an ion is acidic or basic is critical for predicting the pH of the solution.
Solution pH Determination
Once you've identified whether the ions are acidic, basic, or neutral, you can determine the pH of the overall solution. This is done by examining the predominant interaction at play.
  • If the solution contains predominantly acidic ions, it will result in an acidic solution. For example, in \( \text{NH}_4\text{ClO}_4 \), \( \text{NH}_4^+ \) is acidic, leading to an overall acidic solution.
  • If the solution contains predominantly basic ions, it will be a basic solution. For example, \( \text{Na}_2\text{CO}_3 \) has \( \text{CO}_3^{2-} \), making the solution basic.
  • Conversely, if the ions have balanced acidic and basic properties, the solution remains neutral.
This identification process helps in predicting whether a salt will create an acidic, basic, or neutral solution in water. Understanding solution pH is vital for tasks in both academic and real-world scenarios.

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Most popular questions from this chapter

The equilibrium equations and \(K_{a}\) values for three reaction systems are given below. \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}=\) \(\mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{HC}_{2} \mathrm{O}_{4}^{-}(a q) ; K_{a}=5.6 \times 10^{-2}\) $$ \begin{aligned} \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O} & \rightleftharpoons \\ \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q) ; K_{a}=6.9 \times 10^{-3} \\ \mathrm{HCOOH}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \\ \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{HCOO}^{-}(a q) ; K_{a}=1.7 \times 10^{-4} \end{aligned} $$ a. Which conjugate pair would be best for preparing a buffer with a pH of \(2.88\) ? b. How would you prepare \(50 \mathrm{~mL}\) of a buffer with a \(\mathrm{pH}\) of \(2.88\) assuming that you had available \(0.10 M\) solutions of each pair?

(a) Draw a pH titration curve that represents the titration of \(50.0 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{NH}_{3}\) by the addition of \(0.10 \mathrm{M}\) \(\mathrm{HCl}\) from a buret. Label the axes and put a scale on each axis. Show where the equivalence point and the buffer region are on the titration curve. You should do calculations for the \(0 \%, 30 \%\), \(50 \%\), and \(100 \%\) titration points. (b) Is the solution neutral, acidic, or basic at the equivalence point? Why?

A \(0.10 M\) aqueous solution of sodium dihydrogen phosphate, \(\mathrm{NaH}_{2} \mathrm{PO}_{4}\), has a pH of \(4.10 .\) Calculate \(K_{a 2}\) for phosphoric acid. You can ignore hydrolysis of the \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) ion.

A \(0.288-\mathrm{g}\) sample of an unknown monoprotic organic acid is dissolved in water and titrated with a \(0.115 \mathrm{M}\) sodium hydroxide solution. After the addition of \(17.54 \mathrm{~mL}\) of base, a \(\mathrm{pH}\) of \(4.92\) is recorded. The equivalence point is reached when a total of \(33.83 \mathrm{~mL}\) of \(\mathrm{NaOH}\) is added. a. What is the molar mass of the organic acid? b. What is the \(K_{a}\) value for the acid? The \(K_{a}\) value could have been determined very easily if a pH measurement had been made after the addition of \(16.92 \mathrm{~mL}\) of \(\mathrm{NaOH}\). Why?

Phthalic acid, \(\mathrm{H}_{2} \mathrm{C}_{8} \mathrm{H}_{4} \mathrm{O}_{4}\), is a diprotic acid used in the synthesis of phenolphthalein indicator. \(K_{a 1}=1.2 \times 10^{-3}\), and \(K_{a 2}=3.9 \times 10^{-6}\). (a) Calculate the hydronium-ion concentration of a \(0.015 M\) solution. (b) What is the concentration of the \(\mathrm{C}_{8} \mathrm{H}_{4} \mathrm{O}_{4}^{2-}\) ion in the solution?
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