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Chapter 21: Q21.6P (page 972)

How are protons removed when balancing a redox reaction in a basic solution?

Short Answer

Expert verified

By introducing an equal number of ${OH}^{-}$ on both sides of the reaction, the resultant ions are balanced.

Step by step solution

01

Definition of redox reaction

Electrons are transferred from one chemical material to another in many chemical processes. The oxidation-reduction or Redox reaction is the name given to these electron transport reactions.

02

Calculating how protons are removed when balancing a redox reaction in a basic solution

Protons are eliminated when balancing a redox reaction in a basic solution by adding an equal quantity of ${OH}^{-}$ on both sides.

The ${OH}^{-}$ ions and $H^{+}$ ions on the same side are later joined to create the water molecule.

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Most popular questions from this chapter

Balance each skeleton reaction, calculate $E °_{cell}$ , and state whether the reaction is spontaneous:

(a)role="math" localid="1663418747793" ${Cl}_{2} {(g) + Fe}^{2 +} {(aq) Cl}^{-} {(aq) + Fe}^{3 +} (aq)$

(b)role="math" localid="1663418761168" ${Mn}^{2 +} {(aq) + Co}^{3 +} {(aq) MnO}_{2} {(s) + Co}^{2 +} (aq)[acidic]$

(c) ${AgCl(s) + NO(g) Ag(s) + Cl}^{-} {(aq) + NO}_{3}^{-} (aq)[acidic]$

Electrodes used in electrocardiography are disposable, and many incorporate silvers. The metal is deposited in a thin layer on a small plastic “button,” and then some is converted to $AgCl$ :

${Ag(s) + Cl}^{-} (aq) ⇌ {AgCl(s) +e}^{-}$

(a) If the surface area of the button is ${2.0 cm}^{2}$ and the thickness of the silver layer is $7.5 \times 10^{- 6} m$ , calculate the volume (in ${cm}^{3}$ ) ofused in one electrode.

(b) The density of silver metal is ${10.5 g/cm}^{3}$ . How many grams of silver are used per electrode?

(c) Ifis plated on the button from an ${Ag}^{+}$ solution with a current of $12.0 mA$ , how many minutes does the plating take?

(d) If bulk silver costs $$ 13.00$ per troy ounce ( $31.10 g$ ), what is the cost (in cents) of the silver in one disposable electrode?

In the electrolysis of a molten mixture of $C s B r$ and $S r C l_{2}$ , identify the product that forms at the negative electrode and at the positive electrode.

A current is applied to two electrolytic cells in series. In the first, silver is deposited; in the second, a zinc electrode is consumed. How much Ag is plated out if 1.2 g of Zn dissolves?

In a concentration cell, is the more concentrated electrolyte in the cathode or the anode compartment? Explain.

See all solutions

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