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Chapter 4: Problem 6

Which of the following ions will always be a spectator ion in a precipitation reaction? (a) $\mathrm{Cl}^{-},(\mathbf{b}) \mathrm{NO}_{3}^{-}$, (d) \(\mathrm{S}^{2-}\), (c) \(\mathrm{NH}_{4}^{+}\) (e) \(\mathrm{SO}_{4}^{2-} .[\) Section 4.2\(]\)

Short Answer

Expert verified
The nitrate ion (\(\mathrm{NO}_{3}^{-}\)) in option (b) will always be a spectator ion in a precipitation reaction, as it is not known to form any insoluble compounds.

Step by step solution

01

Identify common soluble ions

In general, ions from Group 1 elements (like Na+ and K+), and the ammonium ion (NH4+) are soluble in water. Additionally, the nitrate ion (NO3-) is also soluble. Knowing this, we can narrow down our choices to options (b) and (c).
02

Check for known insoluble compounds

Let's check each remaining ion to see if they form any well-known insoluble compounds: - Option (b): Nitrate ion (\(\mathrm{NO}_{3}^{-}\)): Nitrates typically produce soluble compounds when combined with other ions. - Option (c): Ammonium ion (\(\mathrm{NH}_{4}^{+}\)): Ammonium also typically produces soluble compounds when combined with other ions. As both ions under consideration tend to form soluble compounds when reacting with other ions, neither of them is likely to participate in a precipitation reaction.
03

Select the spectator ion

While both options (b) and (c) are known to have high solubility in water, the question asks which ion will *always* be a spectator ion. Based on our analysis, we can conclude that the nitrate ion (\(\mathrm{NO}_{3}^{-}\)) in option (b) is the ion that will always act as a spectator ion in a precipitation reaction, as it is not known to form any insoluble compounds.

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Most popular questions from this chapter

The U.S. standard for arsenate in drinking water requires that public water supplies must contain no greater than 10 parts per billion (ppb) arsenic. If this arsenic is present as arsenate, \(\mathrm{AsO}_{4}^{3-},\) what mass of sodium arsenate would be present in a 1.00-L sample of drinking water that just meets the standard? Parts per billion is defined on a mass basis as $$ \mathrm{Ppb}=\frac{\mathrm{g} \text { solute }}{\mathrm{g} \text { solution }} \times 10^{9} $$

State whether each of the following statements is true or false. Justify your answer in each case. (a) \(\mathrm{NH}_{3}\) contains no \(\mathrm{OH}^{-}\) ions, and yet its aqueous solutions are basic. (b) HF is a strong acid. (c) Although sulfuric acid is a strong electrolyte, an aqueous solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) contains more \(\mathrm{HSO}_{4}^{-}\) ions than \(\mathrm{SO}_{4}^{2-}\) ions.

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) $\mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (b) \(\mathrm{Br}_{2}(l)+2 \mathrm{~K}(s) \longrightarrow 2 \mathrm{KBr}(s)\) (c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)$ (d) $\mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+$

Hard water contains \(\mathrm{Ca}^{2+}, \mathrm{Mg}^{2+}\), and \(\mathrm{Fe}^{2+}\), which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with \(\mathrm{Na}^{+} .\) Keep in mind that charge balance must be maintained. (a) If \(1500 \mathrm{~L}\) of hard water contains \(0.020 \mathrm{M} \mathrm{Ca}^{2+}\) and \(0.0040 \mathrm{M} \mathrm{Mg}^{2+}\), how many moles of Nat are needed to replace these ions? (b) If the sodium is added to the water softener in the form of \(\mathrm{NaCl}\), how many grams of sodium chloride are needed?

The arsenic in a \(1.22-g\) sample of a pesticide was converted to \(\mathrm{AsO}_{4}^{3-}\) by suitable chemical treatment. It was then titrated using \(\mathrm{Ag}^{+}\) to form \(\mathrm{Ag}_{3} \mathrm{AsO}_{4}\) as a precipitate. (a) What is the oxidation state of As in $\mathrm{AsO}_{4}{ }^{3-} ?(\mathbf{b})\( Name \)\mathrm{Ag}_{3} \mathrm{AsO}_{4}$ by analogy to the corresponding compound containing phosphorus in place of arsenic. (c) If it took \(25.0 \mathrm{~mL}\) of \(0.102 \mathrm{MAg}^{+}\) to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide?
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