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Chapter 8: Problem 118

Indicate whether a precipitate forms when these solutions are mixed, and write the formula of the precipitate if one forms: (a) Silver nitrate and potassium iodide (b) Lithium sulfate and silver acetate (c) Sodium chloride and ammonium sulfate

Short Answer

Expert verified
(a) Yes, a precipitate forms. Formula of the precipitate: AgI (b) Yes, a precipitate forms. Formula of the precipitate: Ag鈧係O鈧� (c) No precipitate forms.

Step by step solution

01

Know the solubility rules

To predict the formation of precipitates, we need to know the solubility rules. Some common solubility rules are: 1. All nitrates are soluble. 2. All acetates are soluble. 3. Most sulfates are soluble. 4. Most chlorides, bromides, and iodides are soluble, except those of silver, lead, and mercury. 5. Most carbonates, phosphates, and silicates are insoluble. Now let's apply these rules to our problems.
02

(a) Silver nitrate and potassium iodide

Write down the reactants and their ions: Silver nitrate (AgNO3): Ag鈦� and NO鈧冣伝 Potassium iodide (KI): K鈦� and I鈦� Considering possible ion combinations for the products: AgI and KNO鈧�. According to the solubility rules, iodides are generally soluble except for silver, lead, and mercury. Therefore, AgI is insoluble and will form a precipitate. KNO鈧� is soluble because all nitrates are soluble. The balanced chemical equation is: AgNO鈧�(aq) + KI(aq) 鈫� AgI(s) + KNO鈧�(aq) A precipitate forms: Yes Formula of the precipitate: AgI
03

(b) Lithium sulfate and silver acetate

Write down the reactants and their ions: Lithium sulfate (Li2SO4): 2 Li鈦� and SO鈧劼测伝 Silver acetate (AgC2H3O2): Ag鈦� and C鈧侶鈧僌鈧傗伝 Considering possible ion combinations for the products: LiC鈧侶鈧僌鈧� and Ag鈧係O鈧�. According to solubility rules, all acetates are soluble, so LiC鈧侶鈧僌鈧� is soluble. Most sulfates are soluble, but silver sulfate (Ag鈧係O鈧�) is an exception and is insoluble. Therefore, Ag鈧係O鈧� will form a precipitate. The balanced chemical equation is: Li鈧係O鈧�(aq) + 2 AgC鈧侶鈧僌鈧�(aq) 鈫� 2 LiC鈧侶鈧僌鈧�(aq) + Ag鈧係O鈧�(s) A precipitate forms: Yes Formula of the precipitate: Ag鈧係O鈧�
04

(c) Sodium chloride and ammonium sulfate

Write down the reactants and their ions: Sodium chloride (NaCl): Na鈦� and Cl鈦� Ammonium sulfate ((NH鈧�)鈧係O鈧�): 2 NH鈧勨伜 and SO鈧劼测伝 Considering possible ion combinations for the products: Na鈧係O鈧� and NH鈧凜l. Most sulfates are soluble, and sodium sulfate (Na鈧係O鈧�) is no exception. Most chlorides are soluble, and ammonium chloride (NH鈧凜l) is no exception. The balanced chemical equation is: 2 NaCl(aq) + (NH鈧�)鈧係O鈧�(aq) 鈫� Na鈧係O鈧�(aq) + 2 NH鈧凜l(aq) A precipitate forms: No Formula of the precipitate: no precipitate

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Key Concepts

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

Solubility Rules
Understanding solubility rules is crucial for determining whether a precipitation reaction will occur. These rules provide guidelines on what types of ionic compounds are soluble or insoluble when dissolved in water. Here are some simplified solubility rules to keep in mind:
  • Nitrates and Acetates: Nitrates (\(NO_3^鈭抃)) and acetates often form soluble compounds, making them good candidates to stay dissolved in solution.
  • Chlorides, Bromides, and Iodides: These halides are usually soluble, except when paired with silver, lead, or mercury, which form insoluble compounds like silver iodide (\(AgI\)).
  • Sulfates: Sulfates (\(SO_4^{2-}\)) are generally soluble, but exceptions include those of barium, lead, and silver, such as silver sulfate (\(Ag_2SO_4\)).
  • Carbonates and Phosphates: These typically form insoluble compounds unless combined with alkali metals or ammonium.
These rules help us predict whether a solid precipitate will form when solutions are mixed. For instance, in a reaction between silver nitrate and potassium iodide, silver iodide will precipitate because it is an insoluble iodide.
Chemical Equations
Chemical equations represent the rearrangement of atoms during a chemical reaction. A correctly balanced equation reflects the conservation of mass and charge, showing the same number of each type of atom on both sides of the equation. Here鈥檚 how to write a balanced chemical equation:
  • Identify the Reactants and Products: Start by listing the reactants and products. For example, when mixing silver nitrate (\(AgNO_3\)) and potassium iodide (\(KI\)), the products are silver iodide (\(AgI\)) and potassium nitrate (\(KNO_3\)).
  • Check Solubility Rules: Determine which compounds will be solid precitates or will remain in solution using solubility rules.
  • Balance the Equation: Ensure that each element is balanced. Adjust coefficients as necessary. The equation for the mentioned reaction is:\[AgNO_3(aq) + KI(aq) \rightarrow AgI(s) + KNO_3(aq)\]
Balanced chemical equations are key to understanding the stoichiometry and actual process involved in a reaction.
Ionic Compounds
Ionic compounds are formed from positive and negative ions bonding together due to their opposite charges. They typically consist of metals combining with non-metals. Here are some important features of ionic compounds:
  • Formation: Ionic compounds are made when metals lose electrons to become positively charged cations, and non-metals gain electrons to become negatively charged anions.
  • Properties: These compounds often have high melting and boiling points because of the strong forces between ions. When dissolved in water or melted, they conduct electricity due to the movement of free ions.
  • Examples: Common examples include table salt (\(NaCl\)) and silver nitrate (\(AgNO_3\)). Each compound鈥檚 specific properties depend on the ions' charges and sizes.
Understanding ionic compounds is fundamental to predicting outcomes in chemical reactions, such as precipitate formation. Each ionic compound brings specific characteristics to a reaction scenario, influencing whether a compound remains in solution or forms as a solid.

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Most popular questions from this chapter

Of the types of reactions discussed in the chapter, list three ways the reaction \(\mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{CaSO}_{4}+2 \mathrm{H}_{2} \mathrm{O}\) can be classified.

Aqueous solutions of iron(III) sulfate and barium hydroxide are combined. Does a precipitate form? If yes, write a net ionic equation for the precipitation reaction.

Balance this chemical equation, and classify it as combination, decomposition, single-replacement, or double-replacement: \(\mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}+\mathrm{H}_{2} \mathrm{O}\)

What does it mean when the label (aq) is attached to the formula for an ionic compound?

When you strike a match, trace amounts of white phosphorus \(\left(\mathrm{P}_{4}\right)\) are converted into an oxide of phosphorus, \(\mathrm{P}_{4} \mathrm{O}_{10}\). This conversion releases sufficient heat to ignite the match head. Write a balanced reaction for this conversion, and classify the reaction type(s).
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