AP Chemistry 4.2 A Represent Changes in Matter with a Balanced Chemical or Net Ionic Equation I for Physical Changes Ii for Questions

Practice AP Chemistry questions on writing balanced molecular, complete ionic, and net ionic equations while conserving atoms, charge, and relevant aqueous species.

Exam points

Explain how acid-base equilibria and conjugate pairs determine pH, buffering and reaction direction.
Apply Ka, Kb, pH and buffer relationships to calculate concentrations in aqueous systems.

[Maximum number: 1]

Answer the following questions about an experiment in which $\mathrm{CaCO}_{3}(s)$ is combined with HCl(a q), represented by the following balanced equation.

\mathrm{CaCO}_{3}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{CaCl}_{2}(a q)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)

Write the balanced net ionic equation for the reaction.

A student performs an investigation to study factors that affect the rate of the reaction. In each trial the student combines 50.0 mL of HCl(a q) at 21.2°C with 1.00 g of $\mathrm{CaCO}_{3}(s)$ and measures the time required for the reaction to go to completion. The data are given in the following table.

Table for Question AP Chemistry 4.2 A Represent Changes in Matter with a Balanced Chemical or Net Ionic Equation I for Physical Changes Ii for Questions question 1 — AP Chemistry

For the correct balanced equation (state symbols not required): 1 point
Accept one of the following:

- $\mathrm{CaCO}_{3}(s)+2 \mathrm{H}^{+}(a q) \rightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$

- $\mathrm{CaCO}_{3}(s)+2 \mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)$

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AP Chemistry 4.2 A Represent Changes in Matter with a Balanced Chemical or Net Ionic Equation I for Physical Changes Ii for Questions question 1