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Chapter 4: Problem 57

The metal cadmium tends to form \(\mathrm{Cd}^{2+}\) ions. The following observations are made: (i) When a strip of zinc metal is placed in \(\mathrm{CdCl}_{2}(a q),\) cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q),\) nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations. (b) Which elements more closely define the position of cadmium in the activity series? (c) What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?

Short Answer

Expert verified
(a) The net ionic equations are: (i) \(Zn (s) + Cd^{2+} (aq) \rightarrow Zn^{2+} (aq) + Cd (s)\) (ii) \(Cd (s) + Ni^{2+} (aq) \rightarrow Cd^{2+} (aq) + Ni (s)\) (b) In the activity series, cadmium is located between zinc and nickel. (c) To locate the position of cadmium more precisely, perform experiments with other metals in the activity series and observe displacements. This would involve testing the reactivity of cadmium towards a variety of metallic ions, such as Cu^2+, Ag^+, Pb^2+, and Mg^2+.

Step by step solution

01

(Step 1: Identify the reactions involved in each observation)

In order to write the net ionic equations, we have to identify the reactions occurring in these observations based on given information: Observation (i): Zinc strip is placed in CdCl2 (aq) Observation (ii): Cadmium strip is placed in Ni (NO3)2 (aq)
02

(Step 2: Write the ionic equations for each reaction)

Now, we'll write the ionic equations for each reaction: For Observation (i): Zn (s) + Cd^2+ (aq) → Zn^2+ (aq) + Cd (s) For Observation (ii): Cd (s) + Ni^2+ (aq) → Cd^2+ (aq) + Ni (s)
03

(Step 3: Answer part a - Write the net ionic equations)

Based on step 2, we can write the net ionic equations for each reaction since there are no spectator ions involved. Net ionic equations are the same as the ionic equations in this case: (i) Zn (s) + Cd^2+ (aq) → Zn^2+ (aq) + Cd (s) (ii) Cd (s) + Ni^2+ (aq) → Cd^2+ (aq) + Ni (s)
04

(Step 4: Answer part b - Locate the position of cadmium in the activity series)

Activity series is a list of elements organized by their ability to undergo a redox reaction. More active metals readily lose electrons and form cations, whereas less active metals form cations with difficulty. Based on the reactions above: (i) Zn is more active than Cd, as Zn can displace Cd^2+ ions. (ii) Cd is more active than Ni, as Cd can displace Ni^2+ ions. So, in the activity series, cadmium is located between zinc and nickel.
05

(Step 5: Answer part c - Experiments to locate the position of Cd more precisely)

To locate the position of cadmium more precisely, we can perform experiments with other metals in the activity series. We could add cadmium to solutions containing ions of other metals in the series (both more active and less active than zinc and nickel) and observe any possible displacements. This would require testing the reactivity of cadmium towards a variety of metallic ions, such as Cu^2+, Ag^+, Pb^2+, and Mg^2+. By observing whether cadmium can successfully displace these ions, we can further identify its position in the activity series with better accuracy.

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Most popular questions from this chapter

Tartaric acid, \(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{6}\) , has two acidic hydrogens. The acid is often present in wines and a salt derived from the acid precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 24.65 \(\mathrm{mL}\) of 0.2500 \(\mathrm{M}\) NaOH solution to titrate both acidic protons in 50.00 \(\mathrm{mL}\) of the tartaric acid solution. Write a balanced net ionic equation for the neutralization reaction, and calculate the molarity of the tartaric acid solution.

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