Question

Which of the following reactions will not form a precipitate?

A) K2C2O4(aq)+Ba(OH)2(aq)→

B) Pb(NO3)2(aq)+H2SO4(aq)→

C) CaCO3(s)+H2SO4(aq)→ incorrect

D) AgNO3(aq)+NaI(aq)→

E) Na2CO3(aq)+HCl(aq)→

Answer 1

E) Na₂CO₃(aq) +HCl (aq)

Step-by-step explanation:

Na₂CO₃(aq) +HCl(aq) ⟶ 2NaCl(aq) + H₂O(ℓ) + CO₂(g)

Salts of alkali metals are generally soluble

A) is wrong.

K₂C₂O₄(aq) + Ba(OH)₂(aq) ⟶ BaC₂O₄(aq) + 2KOH(aq)

Oxalates are generally insoluble.

B) and C are wrong.

Pb(NO¬₃)₂(aq)+ H₂SO₄ (aq)→ PbSO₄(s) + 2HNO₃(aq)

CaCO₃(s) + H₂SO₄(aq) ⟶ CaSO₄(s) + H₂O(ℓ) + CO₂(g)

Sulfates are generally soluble, but PbSO₄ and CaSO₄ are important exceptions.

D) is wrong.

AgNO₃(aq) + NaI(aq) ⟶ AgI(s) + NaNO₃(aq)

Iodides are generally soluble. AgI is an important exception.