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  4. Bis2a 06.appendix a review of

0.24 Bis2a 06.appendix a review of red/ox reactions  (Page 6/31)

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Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(a) H 2 SO 4

(b) Ca(OH) 2

(c) BrOH

(d) ClNO 2

(e) TiCl 4

(f) NaH

(a) H +1, S +6, O –2; (b) Ca +2, O –2, H +1; (c) Br +1, O –2, H +1; (d) Cl +1, N +3, O –2; (e) Ti +4, Cl –1; (f) Na +1, H –1

Classify the following as acid-base reactions or oxidation-reduction reactions:

(a) Na 2 S( a q ) + 2 HCl( a q ) ⟶ 2 NaCl( a q ) + H 2 S( g )

(b) 2 Na( s ) + 2 HCl( a q ) ⟶ 2 NaCl( a q ) + H 2 ( g )

(c) Mg( s ) + Cl 2 ( g ) ⟶ MgCl 2 ( s )

(d) MgO( s ) + 2 HCl( a q ) ⟶ MgCl 2 ( a q ) + H 2 O( l )

(e) K 3 P( s ) + 2 O 2 ( g ) ⟶ K 3 PO 4 ( s )

(f) 3 KOH( a q ) + H 3 PO 4 ( a q ) ⟶ K 3 PO 4 ( a q ) + 3 H 2 O( l )

(a) acid-base; (b) oxidation-reduction: Na is oxidized, H + is reduced; (c) oxidation-reduction: Mg is oxidized, Cl 2 is reduced; (d) acid-base; (e) oxidation-reduction: P 3– is oxidized, O 2 is reduced; (f) acid-base

Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations:

(a) Mg( s ) + NiCl 2 ( a q ) ⟶ MgCl 2 ( a q ) + Ni( s )

(b) PCl 3 ( l ) + Cl 2 ( g ) ⟶ PCl 5 ( s )

(c) C 2 H 4 ( g ) + 3 O 2 ( g ) ⟶ 2 CO 2 ( g ) + 2 H 2 O( g )

(d) Zn( s ) + H 2 SO 4 ( a q ) ⟶ ZnSO 4 ( a q ) + H 2 ( g )

(e) 2 K 2 S 2 O 3 ( s ) + I 2 ( s ) ⟶ K 2 S 4 O 6 ( s ) + 2 KI( s )

(f) 3 Cu( s ) + 8 HNO 3 ( a q ) ⟶ 3 Cu ( NO 3 ) 2 ( a q ) + 2 NO( g ) + 4 H 2 O( l )

(a) Mg is oxidized from 0 to +2 and is the reducing agent, Ni is reduced from +2 to 0 and is the oxidizing agent; (b) P is oxidized from +3 to +5 and is the reducing agent, Cl is reduced from 0 to –1 and is the oxidizing agent; (c) C is oxidized from +2 to +4 and is the reducing agent, O is reduced from 0 to –2 and is the oxidizing agent; (d) Zn is oxidized from 0 to +2 and is the reducing agent, H is reduced from +1 to 0 and is the oxidizing agent; (e) S is oxidized from +2 to +2.5 and is the reducing agent, I 2 is reduced from 0 to –1 and is the oxidizing agent; (f) Cu is oxidized from O to +2, N is reduced from +5 to +2

Complete and balance the following acid-base equations:

(a) HCl gas reacts with solid Ca(OH) 2 ( s ).

(b) A solution of Sr(OH) 2 is added to a solution of HNO 3 .

(a) 2 HCl( g ) + Ca (OH) 2 ( s ) ⟶ CaCl 2 ( s ) + 2 H 2 O( l ) ; (b) Sr (OH) 2 ( a q ) + 2 HNO 3 ( a q ) ⟶ Sr ( NO 3 ) 2 ( a q ) + 2 H 2 O( l )

Complete and balance the following acid-base equations:

(a) A solution of HClO 4 is added to a solution of LiOH.

(b) Aqueous H 2 SO 4 reacts with NaOH.

(c) Ba(OH) 2 reacts with HF gas.

(a) HClO 4 ( a q ) + LiOH( a q ) ⟶ H 2 O( l ) + LiClO 4 ( a q ) ; (b) H 2 SO 4 ( a q ) + 2 NaOH( a q ) ⟶ Na 2 SO 4 ( a q ) + 2 H 2 O( l ) ; (c) Ba ( OH ) 2 ( a q ) + 2 HF( g ) ⟶ BaF 2 ( a q ) + 2 H 2 O( l )

Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.

(a) Al( s ) + F 2 ( g ) ⟶

(b) Al( s ) + CuBr 2 ( a q ) ⟶ (single displacement)

(c) P 4 ( s ) + O 2 ( g ) ⟶

(d) Ca( s ) + H 2 O( l ) ⟶ (products are a strong base and a diatomic gas)

(a) 2 Al( s ) + 3 F 2 ( g ) ⟶ 2 AlF 3 ( s ) ; (b) 2 Al( s ) + 3 CuBr 2 ( a q ) ⟶ 3 Cu( s ) + 2 AlB 3 ( a q ) ; (c) P 4 ( s ) + 5 O 2 ( g ) ⟶ P 4 O 10 ( s ) ; (d) Ca( s ) + 2 H 2 O( l ) ⟶ Ca (OH) 2 ( a q ) + H 2 ( g )

Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.

(a) K( s ) + H 2 O( l ) ⟶

(b) Ba( s ) + HBr( a q ) ⟶

(c) Sn( s ) + I 2 ( s ) ⟶

(a) 2 K( s ) + 2 H 2 O( l ) ⟶ 2 KOH( a q ) + H 2 ( g ) ; (b) Ba( s ) + 2 HBr( a q ) ⟶ BaBr 2 ( a q ) + H 2 ( g ) ; (c) Sn( s ) + 2 I 2 ( s ) ⟶ SnI 4 ( s )

Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used.

(a) Mg (OH) 2 ( s ) + HClO 4 ( a q ) ⟶

(b) SO 3 ( g ) + H 2 O( l ) ⟶ (assume an excess of water and that the product dissolves)

(c) SrO( s ) + H 2 SO 4 ( l ) ⟶

(a) Mg (OH) 2 ( s ) + 2 HClO 4 ( a q ) ⟶ Mg 2+ ( a q ) + 2 ClO 4 − ( a q ) + 2 H 2 O( l ) ; (b) SO 3 ( g ) + 2 H 2 O( l ) ⟶ H 3 O + ( a q ) + HSO 4 − ( a q ), (a solution of H 2 SO 4 ; (c) SrO( s ) + H 2 SO 4 ( l ) ⟶ SrSO 4 ( s ) + H 2 O

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Practice Key Terms 23

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Source:  OpenStax, Ucd bis2a intro to biology v1.2. OpenStax CNX. Sep 22, 2015 Download for free at https://legacy.cnx.org/content/col11890/1.1
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