Predict the product(s) of the following reaction. (separate substances in a list with a comma. include states-of-matter under the given conditions in your answer.) cu(no3)2 + rb3po4 > (h2o above the arrow)

The products will be solid preciptate of copper(II) phosphate and aqueous solution of rubidium nitrate.

Explanation:

Given:

A reaction occuring between copper(II) nitrate and rubidium phosphate.

To find:

The complete chemical reaction

Solution:

The copper(II) nitrate and rubidium phosphate will undergo double displacement reaction.

The reaction will proceed in an aqueous phase.

The products will be solid preciptate of copper(II) phosphate and aqueous solution of rubidium nitrate.

(In order to initiate reaction among the two ionic solids, water was added to bring both ionic compounds in their aqueous phase)

Above reaction can also be written as:

Learn more about double displacement reaction here:

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Cu₃(PO₄)₂(s), RbNO₃(aq)

Explanation:

This reaction looks like a possible double replacement reaction, in which the metal ions have exchanged partners.

3Cu(NO₃)₂(aq) + 2Rb₃PO₄(aq) ⟶ Cu₃(PO₄)₂ + 6RbNO₃

You must recall the pertinent solubility rules:

1. Salts of Group 1 elements (e.g., Rb⁺) are soluble.

2. Salts containing nitrate ions (NO₃⁻) are soluble.

3. Most salts containing phosphate ions (PO₄³⁻) are insoluble

According to Rules 1 and 1, RbNO₃ is soluble.

According to Rule 3, Cu₃(PO₄)₂ is insoluble.

∴ 3Cu(NO₃)₂(aq) + 2Rb₃PO₄(aq) ⟶ Cu₃(PO₄)₂(s) + 6RbNO₃(aq)