Question

use the references to access important values if needed for this question.
write the precipitation reaction for ammonium carbonate in aqueous solution:
(use the lowest possible coefficients. be sure to specify states such as (aq) or (s). if a box is not needed, leave it blank.)

is ammonium carbonate considered soluble or not soluble?
o soluble
o not soluble

Explanation:

To determine the precipitation reaction for ammonium carbonate (\( (NH_4)_2CO_3 \)) and its solubility, we first recall solubility rules. Ammonium salts (salts with \( NH_4^+ \)) are generally soluble. For a precipitation reaction, we need to react ammonium carbonate with a salt that forms an insoluble compound with either \( NH_4^+ \) or \( CO_3^{2-} \). However, since ammonium carbonate itself is soluble, let's consider a reaction where a cation forms an insoluble carbonate. For example, reacting with calcium chloride (\( CaCl_2 \)):

Step 1: Write the reactants

\( (NH_4)_2CO_3(aq) + CaCl_2(aq) \)

Step 2: Determine products

Using double - displacement, the products are \( NH_4Cl(aq) \) and \( CaCO_3(s) \) (calcium carbonate is insoluble).

Step 3: Balance the equation

• For \( CO_3^{2-} \): 1 on left, 1 on right (in \( CaCO_3 \)).
• For \( Ca^{2+} \): 1 on left (in \( CaCl_2 \)), 1 on right (in \( CaCO_3 \)).
• For \( NH_4^+ \): 2 on left (in \( (NH_4)_2CO_3 \)), so we need 2 \( NH_4Cl \) on right.
• For \( Cl^- \): 2 on right (in \( 2NH_4Cl \)), so we need 1 \( CaCl_2 \) (2 \( Cl^- \)) on left.

The balanced equation is: \( (NH_4)_2CO_3(aq)+CaCl_2(aq)
ightarrow 2NH_4Cl(aq) + CaCO_3(s) \)

Now, for the solubility of ammonium carbonate: According to solubility rules, all ammonium salts are soluble in water. So ammonium carbonate is soluble.

Answer:

for the solubility part:
soluble