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Chapter 4: Problem 46

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium sulfide + nickel(II) sulfate (b) Lead(II) nitrate + potassium bromide

Short Answer

Expert verified
Yes, precipitates form in both reactions. NiS forms in (a) and PbBr鈧 forms in (b).

Step by step solution

01

Identify the reactants

The reactants for part (a) are sodium sulfide (Na鈧係) and nickel(II) sulfate (NiSO鈧). The reactants for part (b) are lead(II) nitrate (Pb(NO鈧)鈧) and potassium bromide (KBr).
02

Determine possible products

For part (a), mixing Na鈧係 and NiSO鈧 could yield sodium sulfate (Na鈧係O鈧) and nickel(II) sulfide (NiS). For part (b), mixing Pb(NO鈧)鈧 and KBr could yield lead(II) bromide (PbBr鈧) and potassium nitrate (KNO鈧).
03

Check solubility of products

Use the solubility rules to determine if any of the products are insoluble and will precipitate. NiS is insoluble, so a precipitate will form in part (a). PbBr鈧 is also insoluble, so a precipitate will form in part (b).
04

Write the balanced molecular equations

For part (a): Na鈧係 (aq) + NiSO鈧 (aq) 鈫 Na鈧係O鈧 (aq) + NiS (s)For part (b): Pb(NO鈧)鈧 (aq) + 2 KBr (aq) 鈫 2 KNO鈧 (aq) + PbBr鈧 (s)
05

Write the total ionic equations

For part (a): 2 Na鈦 (aq) + S虏鈦 (aq) + Ni虏鈦 (aq) + SO鈧劼测伝 (aq) 鈫 2 Na鈦 (aq) + SO鈧劼测伝 (aq) + NiS (s)For part (b): Pb虏鈦 (aq) + 2 NO鈧冣伝 (aq) + 2 K鈦 (aq) + 2 Br鈦 (aq) 鈫 2 K鈦 (aq) + 2 NO鈧冣伝 (aq) + PbBr鈧 (s)
06

Write the net ionic equations

For part (a): Ni虏鈦 (aq) + S虏鈦 (aq) 鈫 NiS (s)For part (b): Pb虏鈦 (aq) + 2 Br鈦 (aq) 鈫 PbBr鈧 (s)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Solubility Rules
Solubility rules help us determine whether a substance will dissolve in water. These rules are essential when predicting the formation of a precipitate in a chemical reaction.

Here are some general solubility rules you should remember:
  • Most nitrates (NO鈧冣伝), acetates (CH鈧僀OO鈦), and perchlorates (ClO鈧勨伝) are soluble.
  • Most alkali metal salts (like Na鈦, K鈦) and ammonium (NH鈧勨伜) are soluble.
  • Chlorides (Cl鈦), bromides (Br鈦), and iodides (I鈦) are generally soluble, except when paired with silver (Ag鈦), mercury (Hg鈧偮测伜), or lead (Pb虏鈦).
  • Sulfates (SO鈧劼测伝) are usually soluble, but barium (Ba虏鈦), calcium (Ca虏鈦), and lead (Pb虏鈦) sulfates are exceptions.
  • Most carbonates (CO鈧兟测伝), phosphates (PO鈧劼斥伝), and sulfides (S虏鈦) are insoluble, except for those of alkali metals and ammonium.
Using these rules, you can predict whether a precipitate will form when two solutions are mixed.
In our example, NiS and PbBr鈧 are precipitates because they don't dissolve in water.
Molecular Equation
A molecular equation shows the reactants and products of a reaction in their complete and neutral forms. It鈥檚 useful for providing an overall picture of the reaction.

For Example:
  • For Sodium sulfide and Nickel(II) sulfate: Na鈧係 (aq) + NiSO鈧 (aq) 鈫 Na鈧係O鈧 (aq) + NiS (s)
  • For Lead(II) nitrate and Potassium bromide: Pb(NO鈧)鈧 (aq) + 2 KBr (aq) 鈫 2 KNO鈧 (aq) + PbBr鈧 (s)
Notice that all components are shown as complete compounds. The states of matter (aqueous 'aq', solid 's') are indicated, which helps in identifying the precipitate.
Total Ionic Equation
A total ionic equation shows all the soluble ionic substances dissociated into their ions. This provides more detail about what happens during the reaction.

For Example:
  • For Sodium sulfide and Nickel(II) sulfate: 2 Na鈦 (aq) + S虏鈦 (aq) + Ni虏鈦 (aq) + SO鈧劼测伝 (aq) 鈫 2 Na鈦 (aq) + SO鈧劼测伝 (aq) + NiS (s)
  • For Lead(II) nitrate and Potassium bromide: Pb虏鈦 (aq) + 2 NO鈧冣伝 (aq) + 2 K鈦 (aq) + 2 Br鈦 (aq) 鈫 2 K鈦 (aq) + 2 NO鈧冣伝 (aq) + PbBr鈧 (s)
Here, we see the ions in the solution before they react to form the precipitate. Substances that don't participate in the reaction (i.e., spectator ions) look unchanged.
Net Ionic Equation
A net ionic equation removes the spectator ions, showing only the ions that participate in forming the precipitate. This gives a clearer understanding of the actual chemical change.

For Example:
  • For Sodium sulfide and Nickel(II) sulfate: Ni虏鈦 (aq) + S虏鈦 (aq) 鈫 NiS (s)
  • For Lead(II) nitrate and Potassium bromide: Pb虏鈦 (aq) + 2 Br鈦 (aq) 鈫 PbBr鈧 (s)
By removing the spectator ions (like Na鈦 and SO鈧劼测伝 for the first reaction), we focus on the change that occurs to form the solid precipitate. Understanding these reactions is crucial in predicting and explaining chemical behavior in solutions!

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Most popular questions from this chapter

Sodium hydroxide is used extensively in acid-base titrations because it is a strong, inexpensive base. A sodium hydroxide solution was standardized by titrating \(25.00 \mathrm{~mL}\) of \(0.1528 \mathrm{M}\) standard hydrochloric acid. The initial buret reading of the sodium hydroxide was \(2.24 \mathrm{~mL},\) and the final reading was \(39.21 \mathrm{~mL}\). What was the molarity of the base solution?

Limestone (calcium carbonate) is insoluble in water but dissolves in aqueous hydrochloric acid. Write balanced total ionic and net ionic equations, showing hydrochloric acid as it actually exists in water and the reaction as a proton- transfer process.

To study a marine organism, a biologist prepares a \(1.00-\mathrm{kg}\) sample to simulate the ion concentrations in seawater. She mixes \(26.5 \mathrm{~g}\) of \(\mathrm{NaCl}, 2.40 \mathrm{~g}\) of \(\mathrm{MgCl}_{2}, 3.35 \mathrm{~g}\) of \(\mathrm{MgSO}_{4}, 1.20 \mathrm{~g}\) of \(\mathrm{CaCl}_{2}, 1.05 \mathrm{~g}\) of \(\mathrm{KCl}, 0.315 \mathrm{~g}\) of \(\mathrm{NaHCO}_{3},\) and \(0.098 \mathrm{~g}\) of \(\mathrm{NaBr}\) in distilled water. (a) If the density of the solution is \(1.025 \mathrm{~g} / \mathrm{cm}^{3}\). what is the molarity of each ion? (b) What is the total molarity of alkali metal ions? (c) What is the total molarity of alkaline earth metal ions? (d) What is the total molarity of anions?

How many moles and how many ions of each type are present in each of the following? (a) \(130 \mathrm{~mL}\) of \(0.45 \mathrm{M}\) aluminum chloride (b) \(9.80 \mathrm{~mL}\) of a solution containing \(2.59 \mathrm{~g}\) lithium sulfate \(/ \mathrm{L}\) (c) \(245 \mathrm{~mL}\) of a solution containing \(3.68 \times 10^{22}\) formula units of potassium bromide per liter

Over time, as their free fatty acid (FFA) content increases, edible fats and oils become rancid. To measure rancidity, the fat or oil is dissolved in ethanol, and any FFA present is titrated with KOH dissolved in ethanol. In a series of tests on olive oil, a stock solution of \(0.050 \mathrm{M}\) ethanolic \(\mathrm{KOH}\) was prepared at \(25^{\circ} \mathrm{C},\) stored at \(0^{\circ} \mathrm{C},\) and then placed in a \(100-\mathrm{mL}\) buret to titrate oleic acid [an FFA with formula \(\left.\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{7} \mathrm{CH}=\mathrm{CH}\left(\mathrm{CH}_{2}\right)_{7} \mathrm{COOH}\right]\) in the oil. Each of four \(10.00-\mathrm{g}\) samples of oil took several minutes to titrate: the first required \(19.60 \mathrm{~mL}\), the second \(19.80 \mathrm{~mL},\) and the third and fourth \(20.00 \mathrm{~mL}\) of the ethanolic \(\mathrm{KOH}\). (a) What is the apparent acidity of each sample, in terms of mass \(\%\) of oleic acid? (Note: As the ethanolic KOH warms in the buret, its volume increases by a factor of \(0.00104 /{ }^{\circ} \mathrm{C}\).) (b) Is the variation in acidity a random or systematic error? Explain. (c) What is the actual acidity? How would you demonstrate this?
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