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Chapter 4: Problem 45

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{FeSO}_{4}(a q)+\mathrm{KCl}(a q)\) 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
The precipitates formed for each reaction are: a. No precipitate b. \(Al(OH)_3\) c. \(CaSO_4\) d. \(NiS\)

Step by step solution

01

Identify ions present in each solution

Write the ionic forms of each compound: a. \(FeSO_4 (aq) \) = \(Fe^{2+}\) + \(SO_4^{2-}\) \\ \(KCl (aq) \) = \(K^+\) + \(Cl^-\) b. \(Al(NO_3)_3 (aq) \) = \(Al^{3+}\) + \(3NO_3^-\) \\ \(Ba (OH)_2 (aq) \) = \(Ba^{2+}\) + \(2OH^-\) c. \(CaCl_2 (aq) \) = \(Ca^{2+}\) + \(2Cl^-\) \\ \(Na_2 SO_4 (aq)\) = \(2Na^+\) + \(SO_4^{2-}\) d. \(K_2 S (aq) \) = \(2K^+\) + \(S^{2-}\) \\ \(Ni (NO_3)_2 (aq) \) = \(Ni^{2+}\) + \(2NO_3^-\)
02

Apply solubility rules

Determine which of the possible products of the combinations of solutions are insoluble. a. Possible products: \(FeCl_2\) and \(K_2SO_4\) \\ b. Possible products: \(Al(OH)_3\) and \(Ba(NO_3)_2\) \\ c. Possible products: \(CaSO_4\) and \(2NaCl\) \\ d. Possible products: \(K_2(NO_3)_2\) and \(NiS\) For each combination, check the solubility rules: a. \(FeCl_2\) is soluble and \(K_2SO_4\) is soluble. \\ b. \(Al(OH)_3\) is insoluble, and \(Ba(NO_3)_2\) is soluble. \\ c. \(CaSO_4\) is slightly insoluble, and \(2NaCl\) is soluble. \\ d. \(K_2(NO_3)_2\) is soluble, and \(NiS\) is insoluble.
03

Identify precipitates

Based on the solubility rules, identify which reactions form precipitates: a. No precipitate is formed. b. A precipitate of \(Al(OH)_3\) is formed. c. A slightly insoluble precipitate of \(CaSO_4\) is formed. d. A precipitate of \(NiS\) is formed. The precipitates formed for each reaction are: a. No precipitate \\ b. \(Al(OH)_3\) \\ c. \(CaSO_4\) \\ d. \(NiS\)

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Most popular questions from this chapter

A \(2.20-\mathrm{g}\) sample of an unknown acid (empirical formula \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{3}\) ) is dissolved in \(1.0 \mathrm{~L}\) of water. A titration required \(25.0\) \(\mathrm{mL}\) of \(0.500 \mathrm{M} \mathrm{NaOH}\) to react completely with all the acid present. Assuming the unknown acid has one acidic proton per molecule, what is the molecular formula of the unknown acid?

A \(10.00-\mathrm{mL}\) sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\), is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH}\), and \(16.58 \mathrm{~mL}\) is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{~g} / \mathrm{cm}^{3}\), what is the mass percent of acetic acid in the vinegar?

Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is \(53.66 \% \mathrm{C}\) and \(4.09 \% \mathrm{H}\) by mass. A titration required \(18.02 \mathrm{~mL}\) of \(0.0406 \mathrm{M} \mathrm{NaOH}\) to neutralize \(0.3602 \mathrm{~g}\) carminic acid. Assuming that there is only one acidic hydrogen per molecule, what is the molecular formula of carminic acid?

The drawings below represent aqueous solutions. Solution A is \(2.00 \mathrm{~L}\) of a \(2.00 \mathrm{M}\) aqueous solution of copper(II) nitrate. Solution \(\mathrm{B}\) is \(2.00 \mathrm{~L}\) of a \(3.00 \mathrm{M}\) aqueous solution of potassium hydroxide. a. Draw a picture of the solution made by mixing solutions \(\mathrm{A}\) and \(\mathrm{B}\) together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions \(\mathrm{A}\) and \(\mathrm{B}\), and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in \(M\) ) of all ions left in solution (from part a) and the mass of solid formed.

Some of the substances commonly used in stomach antacids are \(\mathrm{MgO}, \mathrm{Mg}(\mathrm{OH})_{2}\), and \(\mathrm{Al}(\mathrm{OH})_{3}\) a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of \(0.10 \mathrm{M} \mathrm{HCl}\) per gram?
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