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Chapter 8: Problem 50

Write the net ionic equation for the neutralization of a strong acid by a strong base.

Short Answer

Expert verified
Answer: H鈦�(aq) + OH鈦�(aq) -> H2O(l)

Step by step solution

01

Write the balanced molecular equation

For the neutralization of a strong acid and a strong base, we can use hydrogen chloride (HCl) as the strong acid and sodium hydroxide (NaOH) as the strong base. The balanced molecular equation is: HCl + NaOH -> NaCl + H2O
02

Write the complete ionic equation

Since strong acids and strong bases ionize in water, the complete ionic equation involves representing each ionized species in aqueous solutions: HCl -> H^{+}(aq) + Cl^{-}(aq) NaOH -> Na^{+}(aq) + OH^{-}(aq) Replace these species in the balanced molecular equation, resulting in: H^{+}(aq) + Cl^{-}(aq) + Na^{+}(aq) + OH^{-}(aq) -> Na^{+}(aq) + Cl^{-}(aq) + H2O(l)
03

Identify and cancel spectator ions

Spectator ions are ions that appear on both sides of the equation and do not participate in the reaction. In this case, Na^{+}(aq) and Cl^{-}(aq) are spectator ions. Cancel out the spectator ions to obtain the net ionic equation: H^{+}(aq) + OH^{-}(aq) -> H2O(l)
04

Write the final net ionic equation

Our final net ionic equation for the neutralization of a strong acid by a strong base is: H^{+}(aq) + OH^{-}(aq) -> H2O(l)

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Most popular questions from this chapter

Write net ionic equations for the reactions that occur when a. a sample of acetic acid is titrated with a solution of \(\mathrm{KOH}\) b. a solution of sodium carbonate is mixed with a solution of calcium chloride. c. calcium oxide dissolves in water.

The electrolyte in an electricity-generating device called a fuel cell consists of a mixture of \(\mathrm{Li}_{2} \mathrm{CO}_{3}\) and \(\mathrm{K}_{2} \mathrm{CO}_{3}\) heated to \(650^{\circ} \mathrm{C} .\) At this temperature these ionic solids melt. Explain how the mixture of molten carbonates can conduct electricity.

Calculate the molarity of each of the following solutions: a. \(0.56 \mathrm{mol} \mathrm{BaCl}_{2}\) in \(100.0 \mathrm{mL}\) of solution b. \(0.200 \mathrm{mol} \mathrm{Na}_{2} \mathrm{CO}_{3}\) in \(200.0 \mathrm{mL}\) of solution c. \(0.325 \mathrm{mol} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) in \(250.0 \mathrm{mL}\) of solution d. \(1.48 \mathrm{mol} \mathrm{KNO}_{3}\) in \(250.0 \mathrm{mL}\) of solution

How many moles of \(\mathrm{O}_{2}\) are consumed in the conversion of one mole of \(\mathrm{FeCO}_{3}\) to each of the following compounds? Assume \(\mathrm{CO}_{2}\) is also produced. (a) \(\mathrm{Fe}_{2} \mathrm{O}_{3} ;\) (b) \(\mathrm{Fe}_{3} \mathrm{O}_{4}\)

How many milliliters of \(0.100 M\) NaOH are required to neutralize the following solutions? a. \(10.0 \mathrm{mL}\) of \(0.0500 M \mathrm{HCl}\) b. \(25.0 \mathrm{mL}\) of \(0.126 M \mathrm{HNO}_{3}\) c. \(50.0 \mathrm{mL}\) of \(0.215 M \mathrm{H}_{2} \mathrm{SO}_{4}\)
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