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Chapter 6: Problem 47

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\operatorname{FeSO}_{4}(a q)+\operatorname{KCl}(a q)\) b. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q)\) c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) d. \(\mathrm{K}_{2} \mathrm{S}(a q)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

Short Answer

Expert verified
a. No precipitate will form. b. Al(OH)₃ will form as a precipitate. c. CaSO₄ will form a precipitate. d. NiS will form a precipitate.

Step by step solution

01

Identify the ions in each solution

In the first solution, we have Fe²⁺ and SO₄²⁻ ions present. In the second solution, we have K⁺ and Cl⁻ ions present.
02

Determine the possible products and their solubility

When these solutions are mixed, the possible products are FeCl₂ and K₂SO₄. According to solubility rules, all potassium (K⁺) and all chlorides (Cl⁻) salts are soluble. Therefore, no precipitate will form. #b. Mixing Al(NO3)3(aq) and Ba(OH)2(aq)#
03

Identify the ions in each solution

In the first solution, we have Al³⁺ and NO₃⁻ ions present. In the second solution, we have Ba²⁺ and OH⁻ ions present.
04

Determine the possible products and their solubility

When these solutions are mixed, the possible products are Al(OH)₃ and Ba(NO₃)₂. Al(OH)₃ is insoluble while Ba(NO₃)₂ is soluble (since all nitrates (NO₃⁻) are soluble). Therefore, Al(OH)₃ will form as a precipitate. #c. Mixing CaCl2(aq) and Na2SO4(aq)#
05

Identify the ions in each solution

In the first solution, we have Ca²⁺ and Cl⁻ ions present. In the second solution, we have Na⁺ and SO₄²⁻ ions present.
06

Determine the possible products and their solubility

When these solutions are mixed, the possible products are CaSO₄ and NaCl. According to solubility rules, CaSO₄ is slightly soluble, while all sodium (Na⁺) and all chlorides (Cl⁻) salts are soluble. Thus, CaSO₄ will form a precipitate. #d. Mixing K2S(aq) and Ni(NO3)2(aq)#
07

Identify the ions in each solution

In the first solution, we have K⁺ and S²⁻ ions present. In the second solution, we have Ni²⁺ and NO₃⁻ ions present.
08

Determine the possible products and their solubility

When these solutions are mixed, the possible products are KNO₃ and NiS. KNO₃ is soluble (since all nitrates (NO₃⁻) and all potassium (K⁺) salts are soluble), whereas NiS is insoluble. Thus, NiS will form a precipitate.

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Most popular questions from this chapter

Consider the reaction between oxygen \(\left(\mathrm{O}_{2}\right)\) gas and magnesium metal to form magnesium oxide. Using oxidation states, how many electrons would each oxygen atom gain, and how many electrons would each magnesium atom lose? How many magnesium atoms are needed to react with one oxygen molecule? Write a balanced equation for this reaction.

You made \(100.0 \mathrm{mL}\) of a lead(II) nitrate solution for lab but forgot to cap it. The next lab session you noticed that there was only 80.0 mL left (the rest had evaporated). In addition, you forgot the initial concentration of the solution. You decide to take \(2.00 \mathrm{mL}\) of the solution and add an excess of a concentrated sodium chloride solution. You obtain a solid with a mass of 3.407 g. What was the concentration of the original lead(II)

How would you prepare 1.00 L of a \(0.50-M\) solution of each of the following? a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from "concentrated" \((18 \mathrm{M})\) sulfuric acid b. HCl from "concentrated" (12 M) reagent c. \(\mathrm{NiCl}_{2}\) from the salt \(\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. HNO_ from "concentrated" (16 M) reagent e. Sodium carbonate from the pure solid

What volume of each of the following acids will react completely with \(50.00 \mathrm{mL}\) of \(0.200 \mathrm{M} \mathrm{NaOH} ?\) a. \(0.100 M\) HCl b. \(0.150 M\) HNO \(_{3}\) c. \(0.200 \mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (1 acidic hydrogen)

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide
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