Textbook Question
Write balanced complete ionic and net ionic equations for each reaction. d. HC2H3O2(aq) + K2CO3(aq) → H2O(l ) + CO2(g) + KC2H3O2(aq)
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Ch.5 - Introduction to Solutions and Aqueous Solutions
Chapter 5, Problem 59
Write balanced molecular and net ionic equations for the reaction between hydrochloric acid and rubidium hydroxide.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, hydrochloric acid (HCl) acts as an acid, donating a proton, while rubidium hydroxide (RbOH) acts as a base, accepting the proton. The result is the formation of water and a salt, which is a typical outcome of neutralization reactions.
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01:09
Acid-Base Reaction
Balanced Chemical Equations
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This ensures the law of conservation of mass is upheld. For the reaction between HCl and RbOH, the balanced molecular equation must reflect the stoichiometry of the reactants and products accurately.
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01:32Balancing Chemical Equations
Net Ionic Equations
Net ionic equations simplify chemical reactions by removing spectator ions—ions that do not participate in the reaction—from the full ionic equation. This focuses on the actual chemical species that undergo change. In the case of HCl and RbOH, the net ionic equation highlights the formation of water from H+ and OH- ions.
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00:51Net Ionic Equations
Related Practice
Textbook Question
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl- Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations for the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
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Textbook Question
Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
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Textbook Question
Complete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq) →
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Textbook Question
A 15.00-mL sample of an unknown HClO4 solution requires titration with 17.03 mL of 0.1000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO4(aq) + NaOH(aq) → H2O(l ) + NaClO4(aq)
Textbook Question
A 25.00-mL sample of an unknown H3PO4 solution is titrated with a 0.150 M NaOH solution. The equivalence point is reached when 22.97 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is H3PO4(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3PO4(aq)