91影视

On the basis of the general solubility rules given in Table \(7.1,\) write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. Underline the formula of the precipitate (solid) that forms. If no precipitation reaction is likely for the solutes given, so indicate. a. sodium carbonate, \(\mathrm{Na}_{2} \mathrm{CO}_{3},\) and copper(II) sulfate, \(\mathrm{CuSO}_{4}\) b. hydrochloric acid, \(\mathrm{HCl}\), and silver acetate, \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) c. barium chloride, \(\mathrm{BaCl}_{2},\) and calcium nitrate, \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) d. ammonium sulfide, \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{~S},\) and iron(III) chloride, \(\mathrm{FeCl}_{3}\) e. sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4},\) and lead(II) nitrate, \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) f. potassium phosphate, \(\mathrm{K}_{3} \mathrm{PO}_{4}\), and calcium chloride, \(\mathrm{CaCl}_{2}\)

Step by step solution

01

Identify the ions present in the solutions

In sodium carbonate solution, we have sodium ions (Na+) and carbonate ions (CO3虏鈦�), while in copper(II) sulfate solution, we have copper(II) ions (Cu虏鈦�) and sulfate ions (SO4虏鈦�).

02

Determine if any combination of ions might form an insoluble compound

According to the solubility rules, most sulfate salts are soluble, but copper(II) carbonate is insoluble. Therefore, a precipitation reaction will occur, and copper(II) carbonate (CuCO3) will be formed as a precipitate.

03

Write the balanced molecular equation for the precipitation reaction

The equation will be: Na2CO3(aq) + CuSO4(aq) 鈫� 2 Na鈦�(aq) + SO鈧劼测伝(aq) + \underline{CuCO鈧�(s)} b. Hydrochloric acid, HCl, and silver acetate, AgC鈧侶鈧僌鈧�

04

Identify the ions present in the solutions

In hydrochloric acid solution, we have hydrogen ions (H鈦�) and chloride ions (Cl鈦�), while in silver acetate solution, we have silver ions (Ag鈦�) and acetate ions (C鈧侶鈧僌鈧傗伝).

05

Determine if any combination of ions might form an insoluble compound

According to the solubility rules, most chloride salts are soluble, but silver chloride is insoluble. Therefore, a precipitation reaction will occur, and silver chloride (AgCl) will be formed as a precipitate.

06

Write the balanced molecular equation for the precipitation reaction

The equation will be: HCl(aq) + AgC鈧侶鈧僌鈧�(aq) 鈫� H鈦�(aq) + C鈧侶鈧僌鈧傗伝(aq) + \underline{AgCl(s)} c. Barium chloride, BaCl2, and calcium nitrate, Ca(NO鈧�)鈧�

07

Identify the ions present in the solutions

In barium chloride solution, we have barium ions (Ba虏鈦�) and chloride ions (Cl鈦�), while in calcium nitrate solution, we have calcium ions (Ca虏鈦�) and nitrate ions (NO鈧冣伝).

08

Determine if any combination of ions might form an insoluble compound

According to the solubility rules, all nitrate salts are soluble, and there is no possible combination of the ions that would form an insoluble compound. Therefore, no precipitation reaction is likely for these solutes. d. Ammonium sulfide, (NH鈧�)鈧係, and iron(III) chloride, FeCl3

09

Identify the ions present in the solutions

In ammonium sulfide solution, we have ammonium ions (NH鈧勨伜) and sulfide ions (S虏鈦�), while in iron(III) chloride solution, we have iron(III) ions (Fe鲁鈦�) and chloride ions (Cl鈦�).

10

Determine if any combination of ions might form an insoluble compound

According to the solubility rules, most sulfide salts are insoluble (except those of Group 1 elements and NH鈧勨伜). In this case, iron(III) sulfide (Fe鈧係鈧�) is insoluble and will be formed as a precipitate.

11

Write the balanced molecular equation for the precipitation reaction

The equation will be: 2 (NH鈧�)鈧係(aq) + FeCl鈧�(aq) 鈫� 6 NH鈧勨伜(aq) + 6 Cl鈦�(aq) + \underline{Fe鈧係鈧�(s)} e. Sulfuric acid, H鈧係O鈧�, and lead(II) nitrate, Pb(NO鈧�)鈧�

12

Identify the ions present in the solutions

In sulfuric acid solution, we have hydrogen ions (H鈦�) and sulfate ions (SO鈧劼测伝), while in lead(II) nitrate solution, we have lead(II) ions (Pb虏鈦�) and nitrate ions (NO鈧冣伝).

13

Determine if any combination of ions might form an insoluble compound

According to the solubility rules, most sulfate salts are soluble, but lead(II) sulfate (PbSO鈧�) is insoluble. Therefore, a precipitation reaction will occur and lead(II) sulfate will be formed as a precipitate.

14

Write the balanced molecular equation for the precipitation reaction

The equation will be: H鈧係O鈧�(aq) + Pb(NO鈧�)鈧�(aq) 鈫� 2 H鈦�(aq) + 2 NO鈧冣伝(aq) + \underline{PbSO鈧�(s)} f. Potassium phosphate, K鈧働O鈧�, and calcium chloride, CaCl鈧�

15

Identify the ions present in the solutions

In potassium phosphate solution, we have potassium ions (K鈦�) and phosphate ions (PO鈧劼斥伝), while in calcium chloride solution, we have calcium ions (Ca虏鈦�) and chloride ions (Cl鈦�).

16

Determine if any combination of ions might form an insoluble compound

According to the solubility rules, most phosphate salts are insoluble (except those of Group 1 elements and NH鈧勨伜). Calcium phosphate (Ca鈧�(PO鈧�)鈧�) is insoluble and will be formed as a precipitate.

17

Write the balanced molecular equation for the precipitation reaction

The equation will be: 2 K鈧働O鈧�(aq) + 3 CaCl鈧�(aq) 鈫� 6 K鈦�(aq) + 6 Cl鈦�(aq) + \underline{Ca鈧�(PO鈧�)鈧�(s)}

Unlock Step-by-Step Solutions & Ace Your Exams!

• Full Textbook Solutions

  Get detailed explanations and key concepts

• Unlimited Al creation

  Al flashcards, explanations, exams and more...

• Ads-free access

  To over 500 millions flashcards

• Money-back guarantee

  We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Solubility Rules

Understanding solubility rules is essential when predicting whether a precipitation reaction will occur. Solubility rules provide guidelines about which compounds dissolve in water and which do not. For example, most nitrate ( NO鈧冣伝 ) salts are soluble in water, meaning they tend to dissolve. However, certain compounds, such as silver chloride ( AgCl ), are known to be insoluble and do not dissolve, leading to a precipitate when mixed with compatible ions. Solubility rules typically state that:

• Salts containing alkali metal ions (like Na鈦� or K鈦� ) and the ammonium ion ( NH鈧勨伜 ) are generally soluble.
• Nitrates ( NO鈧冣伝 ), acetates ( C鈧侶鈧僌鈧傗伝 ), and most chlorides ( Cl鈦� ) are soluble.
• Exceptions exist, such as chlorides of Ag鈦� and Pb虏鈦� , which form insoluble salts.

These rules help predict the chemical behavior of different aqueous solutions when they are mixed together, determining if a solid, or a precipitate, will form.

Balanced Molecular Equation

Writing a balanced molecular equation is a key step in predicting the outcome of a chemical reaction, especially precipitation reactions. This involves accounting for the number and type of each atom, ensuring that they are the same on both sides of the equation. For instance, if mixtures of sodium carbonate (Na鈧侰O鈧�) and copper(II) sulfate (CuSO鈧�) are involved, the balanced equation would be:\[ \text{Na}_2\text{CO}_3 (aq) + \text{CuSO}_4 (aq) \rightarrow 2 \text{Na}^+ (aq) + \text{SO}_4^{2-} (aq) + \underline{\text{CuCO}_3 (s)} \]The equation shows the reactants forming ions and subsequently a precipitate, ensuring mass balance (same number of each type of atom) and charge balance (equal charge on both sides). Using coefficients to adjust the number of molecules or ions helps achieve this balance, resembling a diligent checking of ingredients in a chemical 'recipe.'

Insoluble Compounds

Insoluble compounds are those that do not dissolve (or only sparingly dissolve) in water. When two aqueous solutions are combined, and an insoluble compound is formed, it appears as a solid that settles out of the liquid, known as a precipitate. This process is central to precipitation reactions. Typically, compounds like CaCO鈧� , BaSO鈧� , and AgCl are known for their low solubility in water. When their component ions meet in solution, they reach a low-solubility limit, resulting in a solid precipitate. Recognizing which combinations of ions form insoluble compounds can predict if a precipitation will occur or if the ions will remain in their aqueous forms.

Aqueous Solutions

An aqueous solution is a solution in which water is the solvent. Many reactions, particularly precipitation reactions, occur in aqueous environments because water efficiently dissolves a wide range of substances. In chemistry, we denote aqueous solutions with the symbol (aq) as part of a compound's state. For example, in a household product like table salt, sodium chloride dissolves in water to become NaCl(aq) . In the context of chemistry exercises, when we mix different aqueous solutions, their dissolved ions can react with one another. If the resulting compounds are insoluble according to the solubility rules, a solid precipitate will form. Aqueous solutions are essential in laboratory practices, mimicking environments similar to biological systems where many reactions naturally occur.