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Chapter 4: Problem 105

Many plants are poisonous because their stems and leaves contain oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) or sodium oxalate, \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) . When ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion, $\mathrm{C}_{2} \mathrm{O}_{4}^{2-},$ 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, \(\mathrm{CaCl}_{2},\) in aqueous solution.

Short Answer

Expert verified
The net ionic equation for the reaction between sodium oxalate (Na2C2O4) and calcium chloride (CaCl2) in aqueous solution is: \(C2O4^{2-} (aq) + Ca^{2+} (aq) \rightarrow CaC2O4 (s)\)

Step by step solution

01

Write the balanced chemical equation

The balanced chemical equation for the reaction between sodium oxalate and calcium chloride is: Na2C2O4 (aq) + CaCl2 (aq) → CaC2O4 (s) + 2 NaCl (aq)
02

Identify the spectator ions

Spectator ions are ions that remain unchanged during the reaction and do not participate in it. In this case, the spectator ions are sodium (Na⁺) and chloride (Cl⁻) ions.
03

Write the net ionic equation

To write the net ionic equation, we'll remove the spectator ions from the balanced chemical equation. The net ionic equation is: C2O4²⁻ (aq) + Ca²⁺ (aq) → CaC2O4 (s) This is the net ionic equation for the reaction between sodium oxalate and calcium chloride in aqueous solution.

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Most popular questions from this chapter

A stream flows at a rate of \(5.00 \times 10^{4}\) liters per second (L/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 135 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: $$\mathrm{CaO}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(i) $$ What mass of CaO is consumed in an 8.00-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.

A 50.00 -mL sample of solution containing \(\mathrm{Fe}^{2+}\) ions is titrated with a 0.0216 \(\mathrm{M} \mathrm{KMnO}_{4}\) solution. It required 20.62 \(\mathrm{mL}\) of \(\mathrm{KMnO}_{4}\) solution to oxidize all the \(\mathrm{Fe}^{2+}\) ions to \(\mathrm{Fe}^{3+}\) ions by the reaction $$\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \stackrel{\text { Acidic }}{\longrightarrow} \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q) \text{(Unbalanced)} $$ a. What was the concentration of \(\mathrm{Fe}^{2+}\) ions in the sample solution? b. What volume of 0.0150\(M \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) solution would it take to do the same titration? The reaction is $$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{Fe}^{2+}(a q) \stackrel{\mathrm{Acidic}}{\longrightarrow} \mathrm{Cr}^{3+}(a q) +\mathrm{Fe}^{3+}(a q) \text {(Unbalanced)} $$

Specify which of the following equations represent oxidation– reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced a. $\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}(g)+3 \mathrm{H}_{2}(g)$ b. $2 \mathrm{AgNO}_{3}(a q)+\mathrm{Cu}(s) \rightarrow \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Ag}(s)$ c. $\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$ d. $2 \mathrm{H}^{+}(a q)+2 \mathrm{CrO}_{4}^{2-}(a q) \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$

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 C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?

A 30.0 -mL sample of an unknown strong base is neutralized after the addition of 12.0 \(\mathrm{mL}\) of a 0.150 \(\mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.
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