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Chapter 4: Problem 66

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) b. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow\) c. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

Short Answer

Expert verified
a. Balanced formula: HNO3(aq) + Al(OH)3(s) -> Al(NO3)3(aq) + 3H2O(l) Complete ionic equation: H+(aq) + NO3^-(aq) + Al(OH)3(s) -> Al^3+(aq) + 3NO3^-(aq) + 3H2O(l) Net ionic equation: H+(aq) + Al(OH)3(s) -> Al^3+(aq) + 3H2O(l) b. Balanced formula: HC2H3O2(aq) + KOH(aq) -> KC2H3O2(aq) + H2O(l) Complete ionic equation: H+(aq) + C2H3O2^-(aq) + K+(aq) + OH^-(aq) -> K+(aq) + C2H3O2^-(aq) + H2O(l) Net ionic equation: H+(aq) + OH^-(aq) -> H2O(l) c. Balanced formula: Ca(OH)2(aq) + 2HCl(aq) -> CaCl2(aq) + 2H2O(l) Complete ionic equation: Ca^2+(aq) + 2OH^-(aq) + 2H+(aq) + 2Cl^-(aq) -> Ca^2+(aq) + 2Cl^-(aq) + 2H2O(l) Net ionic equation: 2OH^-(aq) + 2H+(aq) -> 2H2O(l)

Step by step solution

01

a. HNO3(aq) + Al(OH)3(s) ->

Step 1: Identify the acid and base in the reaction, and predict the products: In this reaction, HNO3 is the acid and Al(OH)3 is the base. The products would be a salt and water. Step 2: Write the balanced formula equation for the reaction: HNO3(aq) + Al(OH)3(s) -> Al(NO3)3(aq) + 3H2O(l) Step 3: Write the complete ionic and net ionic equations for the reaction: Complete ionic equation: H+(aq) + NO3^-(aq) + Al(OH)3(s) -> Al^3+(aq) + 3NO3^-(aq) + 3H2O(l) Net ionic equation: H+(aq) + Al(OH)3(s) -> Al^3+(aq) + 3H2O(l)
02

b. HC2H3O2(aq) + KOH(aq) ->

Step 1: Identify the acid and base in the reaction, and predict the products: In this reaction, HC2H3O2 is the acid and KOH is the base. The products would be a salt and water. Step 2: Write the balanced formula equation for the reaction: HC2H3O2(aq) + KOH(aq) -> KC2H3O2(aq) + H2O(l) Step 3: Write the complete ionic and net ionic equations for the reaction: Complete ionic equation: H+(aq) + C2H3O2^-(aq) + K+(aq) + OH^-(aq) -> K+(aq) + C2H3O2^-(aq)+ H2O(l) Net ionic equation: H+(aq) + OH^-(aq) -> H2O(l)
03

c. Ca(OH)2(aq) + HCl(aq) ->

Step 1: Identify the acid and base in the reaction, and predict the products: In this reaction, Ca(OH)2 is the base and HCl is the acid. The products would be a salt and water. Step 2: Write the balanced formula equation for the reaction: Ca(OH)2(aq) + 2HCl(aq) -> CaCl2(aq) + 2H2O(l) Step 3: Write the complete ionic and net ionic equations for the reaction: Complete ionic equation: Ca^2+(aq) + 2OH^-(aq) + 2H+(aq) + 2Cl^-(aq) -> Ca^2+(aq) + 2Cl^-(aq) + 2H2O(l) Net ionic equation: 2OH^-(aq) + 2H+(aq) -> 2H2O(l)

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Most popular questions from this chapter

A \(10.00-\mathrm{mL}\) sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\), is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH}\), and \(16.58 \mathrm{~mL}\) is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{~g} / \mathrm{cm}^{3}\), what is the mass percent of acetic acid in the vinegar?

What volume of each of the following bases will react completely with \(25.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HCl}\) ? a. \(0.100 \mathrm{M} \mathrm{NaOH}\) b. \(0.0500 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}\) c. \(0.250 \mathrm{M} \mathrm{KOH}\)

Consider the reaction of \(19.0 \mathrm{~g}\) of zinc with excess silver nitrite to produce silver metal and zinc nitrite. The reaction is stopped before all the zinc metal has reacted and \(29.0 \mathrm{~g}\) of solid metal is present. Calculate the mass of each metal in the 29.0-g mixture.

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. chromium(III) chloride and sodium hydroxide b. silver nitrate and ammonium carbonate c. copper(II) sulfate and mercury(1) nitrate d. strontium nitrate and potassium iodide

The unknown acid \(\mathrm{H}_{2} \mathrm{X}\) can be neutralized completely by \(\mathrm{OH}^{-}\) according to the following (unbalanced) equation: $$ \mathrm{H}_{2} \mathrm{X}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{X}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ The ion formed as a product, \(\mathrm{X}^{2-}\), was shown to have 36 total electrons. What is element \(\mathrm{X}\) ? Propose a name for \(\mathrm{H}_{2} \mathrm{X}\). To completely neutralize a sample of \(\mathrm{H}_{2} \mathrm{X}, 35.6 \mathrm{~mL}\) of \(0.175 \mathrm{M}\) \(\mathrm{OH}^{-}\) solution was required. What was the mass of the \(\mathrm{H}_{2} \mathrm{X}\) sample used?
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