Question

Determine whether a solid forms when solutions containing the following salts are mixed. If so, write the ionic equation and the net ionic equation. Part A Na3PO4(aq) and AgNO3(aq). If a solid forms when solutions containing these salts are mixed, write the ionic equation. Part B Na3PO4(aq) and AgNO3(aq). If a solid forms when solutions containing these salts are mixed, write the net ionic equation. Part C MnSO4(aq) and Na2CO3(aq).If a solid forms when solutions containing these salts are mixed, write the ionic equation. Part D MnSO4(aq) and Na2CO3(aq).If a solid forms when solutions containing these salts are mixed, write the net ionic equation. Part G BaCl2(aq) and KOH(aq). If a solid forms when solutions containing these salts are mixed, write the ionic equation. Part H BaCl2(aq) and KOH(aq). If a solid forms when solutions containing these salts are mixed, write the net ionic equation.

Answer 1

A)

the molecular equation is

Na3P04 + 3AgN03 ---> Ag3P04 (S) + 3NaN03

here

Ag3P04 is the solid precipitate

now

ionic equation is

3 Na+ + P043- + 3 Ag+ + 3 N03- --> Ag3P04 (s) + 3 Na+ + 3 N03-

B)

cancel out the common ions

we get

net ionic equation

3 Ag+ (aq) + P043- (aq) ---> Ag3P04 (s)

C)

the molecular equation is

MnS04 + Na2C03 ---> MnC03 (s) + Na2S04

ionic equation :

Mn+2 + S042- + 2 Na+ + C032- --> MnC03 (s) + 2 Na+ + S042-

D)

net ionic equation is

Mn+2 (aq) + C032- (aq) ----> MnC03 (s)

G)

the molecular equation is

Bacl2 + 2KOH --> Ba(OH)2 + 2 KCl

no solid precipitate is formed in this case

both Ba(OH)2 and KCl are soluble