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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: \(\mathrm{3HNO}_{3}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}(\mathrm{NO}_{3})_{3}(a q)\) Complete Ionic: \(3\mathrm{H}^{+}(a q) + 3\mathrm{NO}_{3}^{-}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q) + 3\mathrm{NO}_{3}^{-}(a q)\) Net Ionic: \(3\mathrm{H}^{+}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q)\) b. Balanced Formula: \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q) + \mathrm{KOH}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{KC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)\) Complete Ionic: \(\mathrm{H}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q) + \mathrm{K}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{K}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q)\) Net Ionic: \(\mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\) c. Balanced Formula: \(\mathrm{Ca}(\mathrm{OH})_{2}(a q) + 2\mathrm{HCl}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CaCl}_{2}(a q)\) Complete Ionic: \(\mathrm{Ca}^{2+}(a q) + 2\mathrm{OH}^{-}(a q) + 2\mathrm{H}^{+}(a q) + 2\mathrm{Cl}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Ca}^{2+}(a q) + 2\mathrm{Cl}^{-}(a q)\) Net Ionic: \(2\mathrm{H}^{+}(a q) + 2\mathrm{OH}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\)

Step by step solution

01

Write the balanced formula equation.

In this reaction, nitric acid \(\mathrm{HNO}_{3}\) reacts with aluminum hydroxide \(\mathrm{Al}(\mathrm{OH})_{3}\). The products of the reaction will be water and an aluminum nitrate salt. Therefore, we have: \(\mathrm{3HNO}_{3}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}(\mathrm{NO}_{3})_{3}(a q)\)
02

Write the complete ionic equation.

For the complete ionic equation, we separate the soluble ionic compounds into their respective ions. In this case, we have: \(3\mathrm{H}^{+}(a q) + 3\mathrm{NO}_{3}^{-}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q) + 3\mathrm{NO}_{3}^{-}(a q)\)
03

Write the net ionic equation.

For the net ionic equation, we cancel out ions that are present on both sides of the equation. In this case, we have: \(3\mathrm{H}^{+}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q)\) Reaction b: \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow\)
04

Write the balanced formula equation.

In this reaction, acetic acid \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}\) reacts with potassium hydroxide \(\mathrm{KOH}\). The products of the reaction will be water and a potassium acetate salt. Therefore, we have: \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q) + \mathrm{KOH}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{KC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)\)
05

Write the complete ionic equation.

For the complete ionic equation, we have: \(\mathrm{H}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q) + \mathrm{K}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{K}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q)\)
06

Write the net ionic equation.

For the net ionic equation, we have: \(\mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\) Reaction c: \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)
07

Write the balanced formula equation.

In this reaction, calcium hydroxide \(\mathrm{Ca}(\mathrm{OH})_{2}\) reacts with hydrochloric acid \(\mathrm{HCl}\). The products of the reaction will be water and a calcium chloride salt. Therefore, we have: \(\mathrm{Ca}(\mathrm{OH})_{2}(a q) + 2\mathrm{HCl}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CaCl}_{2}(a q)\)
08

Write the complete ionic equation.

For the complete ionic equation, we have: \(\mathrm{Ca}^{2+}(a q) + 2\mathrm{OH}^{-}(a q) + 2\mathrm{H}^{+}(a q) + 2\mathrm{Cl}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Ca}^{2+}(a q) + 2\mathrm{Cl}^{-}(a q)\)
09

Write the net ionic equation.

For the net ionic equation, we have: \(2\mathrm{H}^{+}(a q) + 2\mathrm{OH}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\)

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Most popular questions from this chapter

A student titrates an unknown amount of potassium hydrogen phthalate \(\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}\right.\), often abbreviated \(\mathrm{KHP}\) ) with \(20.46 \mathrm{~mL}\) of a \(0.1000 M\) NaOH solution. KHP (molar mass \(=204.22\) \(\mathrm{g} / \mathrm{mol}\) ) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

Calculate the sodium ion concentration when \(70.0 \mathrm{~mL}\) of \(3.0 \mathrm{M}\) sodium carbonate is added to \(30.0 \mathrm{~mL}\) of \(1.0 \mathrm{M}\) sodium bicarbonate.

A standard solution is prepared for the analysis of fluoxymesterone \(\left(\mathrm{C}_{20} \mathrm{H}_{29} \mathrm{FO}_{3}\right)\), an anabolic steroid. A stock solution is first prepared by dissolving \(10.0 \mathrm{mg}\) of fluoxymesterone in enough water to give a total volume of \(500.0 \mathrm{~mL}\). A \(100.0-\mu \mathrm{L}\) aliquot (portion) of this solution is diluted to a final volume of \(100.0 \mathrm{~mL}\). Calculate the concentration of the final solution in terms of molarity.

What volume of \(0.0521 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) is required to neutralize exactly \(14.20 \mathrm{~mL}\) of \(0.141 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) ? Phosphoric acid contains three acidic hydrogens.

A stream flows at a rate of \(5.00 \times 10^{4}\) liters per second \((\mathrm{L} / \mathrm{s})\) upstream of a manufacturing plant. The plant discharges \(3.50 \times\) \(10^{3} \mathrm{~L} / \mathrm{s}\) of water that contains \(65.0 \mathrm{ppm} \mathrm{HCl}\) into the stream. (See Exercise 113 for definitions.) a. Calculate the stream's total flow rate downstream from this plant. b. Calculate the concentration of \(\mathrm{HCl}\) in ppm downstream from this plant. c. Further downstream, another manufacturing plant diverts \(1.80 \times 10^{4} \mathrm{~L} / \mathrm{s}\) of water from the stream for its own use. This plant must first neutralize the acid and does so by adding lime: $$ \mathrm{CaO}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ What mass of \(\mathrm{CaO}\) is consumed in an \(8.00-\mathrm{h}\) work day by this plant? d. The original stream water contained \(10.2 \mathrm{ppm} \mathrm{Ca}^{2+}\). Although no calcium was in the waste water from the first plant, the waste water of the second plant contains \(\mathrm{Ca}^{2+}\) from the neutralization process. If \(90.0 \%\) of the water used by the second plant is returned to the stream, calculate the concentration of \(\mathrm{Ca}^{2+}\) in ppm downstream of the second plant.
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