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Chapter 4: Problem 92

Many plants are poisonous because their stems and leaves contain oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) or sodium oxalate \(\left(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\); when ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}\right)\) in a sample is to precipitate this species as calcium oxalate, which is insoluble in water. Write the net ionic equation for the reaction between sodium oxalate and calcium chloride \(\left(\mathrm{CaCl}_{2}\right)\) in aqueous solution.

Short Answer

Expert verified
The net ionic equation for the reaction between sodium oxalate and calcium chloride in aqueous solution is: \(2C_2O_4^{2-}(aq) + Ca^{2+}(aq) \rightarrow CaC_2O_4(s)\)

Step by step solution

01

Write the balanced chemical equation

First, we need to write down the balanced chemical equation for the reaction between sodium oxalate and calcium chloride in aqueous solution. Sodium oxalate is a salt of sodium (Na^+) and oxalate ion (C2O4^2-), and calcium chloride is a salt of calcium (Ca^2+) and chloride ion (Cl^-). In this reaction, calcium (Ca^2+) will replace sodium (Na^+) in sodium oxalate, forming calcium oxalate (which is insoluble in water) and sodium chloride (a soluble salt). The balanced chemical equation for this reaction is: \(Na_2C_2O_4 + CaCl_2 \rightarrow CaC_2O_4 \downarrow + 2NaCl\)
02

Convert the balanced chemical equation into a net ionic equation

Now, we need to convert the balanced chemical equation into a net ionic equation by removing the spectator ions. Spectator ions are ions that do not participate in the reaction and remain unchanged in the products. In this reaction, sodium (Na^+) and chloride (Cl^-) ions are the spectator ions, as they do not participate in the formation of the solid precipitate, calcium oxalate. The net ionic equation will only show the ions that participate in the reaction: \(2C_2O_4^{2-} + Ca^{2+} \rightarrow CaC_2O_4 \downarrow\)
03

Write the net ionic equation for the reaction

Finally, having removed the spectator ions, we can now write down the net ionic equation for the reaction between sodium oxalate and calcium chloride in aqueous solution as follows: \(2C_2O_4^{2-}(aq) + Ca^{2+}(aq) \rightarrow CaC_2O_4(s)\)

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Most popular questions from this chapter

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 \(29.0-\mathrm{g}\) mixture.

Tris(pentafluorophenyl)borane, commonly known by its acronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of \(\mathrm{C}, \mathrm{F}\), and \(\mathrm{B}\); it is \(42.23 \% \mathrm{C}\) by mass and \(55.66 \% \mathrm{~F}\) by mass. a. What is the empirical formula of BARF? b. A \(2.251-g\) sample of BARF dissolved in \(347.0 \mathrm{~mL}\) of solution produces a \(0.01267 M\) solution. What is the molecular formula of BARF?

If \(10 . \mathrm{g}\) of \(\mathrm{AgNO}_{3}\) is available, what volume of \(0.25 \mathrm{M} \mathrm{AgNO}_{3}\) solution can be prepared?

On the basis of the general solubility rules given in Table 4.1, predict which of the following substances are likely to be soluble in water. a. aluminum nitrate b. magnesium chloride c. rubidium sulfate d. nickel(II) hydroxide e. lead(II) sulfide f. magnesium hydroxide g. iron(III) phosphate

What mass of solid aluminum hydroxide can be produced when \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) is added to \(200.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{KOH} ?\)
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