Question

Write balanced net ionic equations for the reactions that occur in each of the following cases:

a. Cr2(SO4)3(aq) + (NH4)2CO3(aq) →
b. Ba(NO3)2(aq) + K2SO4(aq) →
c. Fe(NO3)2(aq) + KOH(aq) →

Answer 1

The balanced net ionic equations for the reactions are:

a. Cr2(SO4)3(aq) + 3(NH4)2CO3(aq) → 2Cr(CO3)3(s) + 6NH4NO3(aq),

b. Ba(NO3)2(aq) + K2SO4(aq) → BaSO4(s) + 2KNO3(aq),

c. Fe(NO3)2(aq) + 2KOH(aq) → Fe(OH)2(s) + 2KNO3(aq)

Step-by-step explanation:

Net ionic equations represent the actual chemical change occurring in a reaction, excluding spectator ions. Examples include the exchange of ions to form water in a neutralization reaction and the formation of precipitates such as calcium phosphate or silver chloride.

Thus, the net balanced ionic equations of given reactions are:

a. Cr2(SO4)3(aq) + 3(NH4)2CO3(aq) → 2Cr(CO3)3(s) + 6NH4NO3(aq)

b. Ba(NO3)2(aq) + K2SO4(aq) → BaSO4(s) + 2KNO3(aq)

c. Fe(NO3)2(aq) + 2KOH(aq) → Fe(OH)2(s) + 2KNO3(aq)

Answer 2

a) Cr2(SO4)3(aq) + 3(NH4)2CO3(aq) → Cr2(CO3)3(s) + 3(NH4)2SO4(aq)

b) Ba(NO3)2(aq) + K2SO4(aq) → BaSO4(s) + 2KNO3(aq)

c) Fe(NO3)2(aq) + 2KOH(aq) → Fe(OH)2(s) + 2KNO3(aq)

Step-by-step explanation:

a. Cr2(SO4)3(aq) + (NH4)2CO3(aq)

Cr2(SO4)3(aq) + 3(NH4)2CO3(aq) → 2Cr^3+ + 3SO4^2- + 6NH4+ + 3CO3^2-

2Cr^3+ + 3SO4^2- + 6NH4+ + 3CO3^2- → Cr2(CO3)3 + 3(NH4)2SO4

Cr2(SO4)3(aq) + 3(NH4)2CO3(aq) → Cr2(CO3)3(s) + 3(NH4)2SO4(aq)

b. Ba(NO3)2(aq) + K2SO4(aq)

Ba(NO3)2(aq) + K2SO4(aq) → Ba2+ +2NO3- + 2K+ + SO4^2-

Ba2+ +2NO3- + 2K+ + SO4^2- → BaSO4 + 2KNO3

Ba(NO3)2(aq) + K2SO4(aq) → BaSO4(s) + 2KNO3(aq)

c. Fe(NO3)2(aq) + KOH(aq)

Fe(NO3)2(aq) + 2KOH(aq) → Fe^2+ + 2NO3- + 2K+ + 2OH-

Fe^2+ + 2NO3- + K+ + OH- → Fe(OH)2 + 2KNO3

Fe(NO3)2(aq) + 2KOH(aq) → Fe(OH)2(s) + 2KNO3(aq)