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Chapter 3: Problem 42

Identify the acid and base used to form these salts, and write the overall neutralization reaction in both complete and net ionic form. (a) \(\mathrm{NaNO}_{2}\) (b) \(\mathrm{CaSO}_{4}\) (c) NaI (d) \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Short Answer

Expert verified
The acids and bases are: (a) NaOH and HNO鈧�, (b) Ca(OH)鈧� and H鈧係O鈧�, (c) NaOH and HI, (d) Mg(OH)鈧� and H鈧働O鈧�. Complete and net ionics are written for each.

Step by step solution

01

Identify Salts and Their Components

For each of the given salts, identify its chemical formula and break it down into its cation and anion components. The salts are: (a) \( \mathrm{NaNO}_{2} \) with components \( \mathrm{Na}^+ \) and \( \mathrm{NO}_2^- \).(b) \( \mathrm{CaSO}_{4} \) with components \( \mathrm{Ca}^{2+} \) and \( \mathrm{SO}_4^{2-} \).(c) \( \mathrm{NaI} \) with components \( \mathrm{Na}^+ \) and \( \mathrm{I}^- \).(d) \( \mathrm{Mg}_{3}(\mathrm{PO}_{4})_{2} \) with components \( \mathrm{Mg}^{2+} \) and \( \mathrm{PO}_4^{3-} \).
02

Determine the Acid and Base

For each salt, identify the acid and base from which it is derived. (a) \( \mathrm{NaNO}_{2} \) is derived from \( \mathrm{NaOH} \) (base) and \( \mathrm{HNO}_2 \) (acid).(b) \( \mathrm{CaSO}_{4} \) is derived from \( \mathrm{Ca(OH)}_{2} \) (base) and \( \mathrm{H_{2}SO_4} \) (acid).(c) \( \mathrm{NaI} \) is derived from \( \mathrm{NaOH} \) (base) and \( \mathrm{HI} \) (acid).(d) \( \mathrm{Mg}_{3}(\mathrm{PO}_{4})_{2} \) is derived from \( \mathrm{Mg(OH)}_{2} \) (base) and \( \mathrm{H_{3}PO_4} \) (acid).
03

Write the Complete Neutralization Reaction

Write the complete reaction for each acid-base pair:(a) \( \mathrm{NaOH (aq) + HNO_2 (aq) \rightarrow NaNO_2 (aq) + H_2O (l)} \)(b) \( \mathrm{Ca(OH)_2 (aq) + H_2SO_4 (aq) \rightarrow CaSO_4 (s) + 2H_2O (l)} \)(c) \( \mathrm{NaOH (aq) + HI (aq) \rightarrow NaI (aq) + H_2O (l)} \)(d) \( \mathrm{3Mg(OH)_2 (aq) + 2H_3PO_4 (aq) \rightarrow Mg_3(PO_4)_2 (s) + 6H_2O (l)} \)
04

Write the Net Ionic Equation

Extract the net ionic form by removing the spectator ions from the complete equation:(a) \( \mathrm{OH^- (aq) + HNO_2 (aq) \rightarrow NO_2^- (aq) + H_2O (l)} \)(b) \( \mathrm{Ca^{2+} (aq) + SO_4^{2-} (aq) \rightarrow CaSO_4 (s)} \)(c) \( \mathrm{OH^- (aq) + H^+ (aq) \rightarrow H_2O (l)} \)(d) \( \mathrm{3Mg^{2+} (aq) + 2PO_4^{3-} (aq) \rightarrow Mg_3(PO_4)_2 (s)} \)
05

Confirm Reactions

Ensure each neutralization reaction accurately represents the balance of moles and charges, reflecting correct formation of water and salts.

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Key Concepts

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

Ionic Compounds
Ionic compounds are chemical compounds composed of ions held together by electrostatic forces termed ionic bonding. These compounds typically form between metals and non-metals. During the formation of an ionic compound, the metal loses one or more electrons to form a positive ion or cation, while the non-metal gains those electrons to form a negative ion or anion. The compound is neutral overall because the total positive charge equals the total negative charge.
  • Examples of ionic compounds include sodium chloride (NaCl) and magnesium oxide (MgO).
  • Each ion in the compound is surrounded by oppositely charged ions.
  • Ionic compounds usually have high melting and boiling points due to the strong attractions between ions.
Understanding ionic compounds is crucial in predicting the outcomes of chemical reactions, such as neutralization reactions that form salts.
Net Ionic Equations
In chemistry, a net ionic equation represents the chemical species that are directly involved in a reaction. It is derived from the complete ionic equation by eliminating the spectator ions, which do not take part in the actual chemistry of the reaction. These equations are particularly useful in emphasizing the actual chemical changes occurring in a solution.
  • Net ionic equations focus on the ions and molecules that undergo a change.
  • Spectator ions, which remain unchanged, are omitted.
  • The process involves breaking down soluble ionic compounds into their respective ions.
For example, in the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), the net ionic equation focuses on H+ combining with OH- to form water (H2O). Understanding how to derive net ionic equations helps in visualizing the core chemical interactions in solution.
Cation and Anion Identification
Identifying cations and anions is essential for understanding how salts and ionic compounds form. Cations are positively charged ions that typically result from an atom losing electrons, while anions are negatively charged ions formed by atoms gaining electrons. Every ionic compound consists of at least one cation and one anion.
  • Cations are usually metal ions such as Na+ or Ca2+.
  • Anions are commonly non-metal ions like Cl- or SO42-.
  • Knowing the charge of ions helps in predicting the formula of the compound they form, ensuring the charges balance.
Accurate identification and pairing of these ions enable chemists to write correct formulas for compounds and describe reactions like neutralization, which forms a salt from an acid and a base.

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Most popular questions from this chapter

An unknown solution contains either lead ions or barium ions, but not both. Which one of these solutions could you use to tell whether the ions present are \(\mathrm{Pb}^{2+}\) or \(\mathrm{Ba}^{2+}\) ? Explain the reasoning behind your choice. $$\mathrm{HCl}(\mathrm{aq}), \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}), \mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})$$

You need to make a \(0.300-\mathrm{M}\) solution of \(\mathrm{NiSO}_{4}(\mathrm{aq}) . \mathrm{Cal}-\) culate the mass of \(\mathrm{NiSO}_{4} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) you should put into a 0.500-L volumetric flask.

When these pairs of reactants are combined in a beaker, (a) describe in words what the contents of the beaker would look like before and after any reaction occurs; (b) use different circles for atoms, molecules, and ions to draw a nanoscale (particulate-level) diagram of what the contents would look like; and (c) write a chemical equation to represent symbolically what the contents would look like. \(\mathrm{LiCl}(\mathrm{aq})\) and \(\mathrm{AgNO}_{3}(\mathrm{aq})\) \(\mathrm{NaOH}(\mathrm{aq})\) and \(\mathrm{HCl}(\mathrm{aq})\)

In a reaction, \(1.2 \mathrm{~g}\) element A reacts with exactly \(3.2 \mathrm{~g}\) oxygen to form an oxide, \(\mathrm{AO}_{x} ; 2.4 \mathrm{~g}\) element A reacts with exactly \(3.2 \mathrm{~g}\) oxygen to form a second oxide, \(\mathrm{AO}_{y}\) (a) Determine the ratio \(x: y\). (b) If \(x=2\), determine what the identity of element A might be.

Aluminum chloride, \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\), is an inexpensive reagent used in many industrial processes. It is made by treating scrap aluminum with chlorine according to the balanced equation $$2 \mathrm{Al}(\mathrm{s})+3 \mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow \mathrm{Al}_{2} \mathrm{Cl}_{6}(\mathrm{~s})$$ (a) Determine which reactant is limiting if \(2.70 \mathrm{~g} \mathrm{Al}\) and \(4.05 \mathrm{~g} \mathrm{Cl}_{2}\) are mixed. (b) Calculate what mass of \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\) can be produced. (c) Calculate what mass of the excess reactant remains when the reaction is complete.
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