CaCl2(aq)+ Cs3PO4(aq) --->
Complete the reaction and classify as precipitation or acid/base. Net ionic equation as well.
I believe this is a precipitation reaction since there is no H. Believe the products may be CaPO4 and Cs3Cl2? Can someone help explain this to me, having a lot of trouble with this!
Calcium phosphate is indeed a precipitate. The cesium and chloride ions stay in solution.
The formula for Calcium phosphate is Ca3(PO4)2
One of the major problems you are having with this and any other equation is that you are tying to balance the equation by making the products match the number of atoms. That isn't the way to do it.
Step 1. Write the equation. Use valences (oxidation states) to determine the formulas.
Step 2. THEN balance the equation.
For example:
CaCl2 + Cs3PO4 ==> CsCl + Ca3(PO4)2.
Note that I determined the formula for cesium chloride from the valences of Cs and Cl. The formula for calcium phosphate follows from Ca(+2) and PO4 (-3). THEN you balance the coefficients by using appropriate coefficients (not by changing the subscripts).
To determine the products and classify the reaction, let's write the molecular equation first and then proceed with the net ionic equation.
The balanced molecular equation for the reaction between CaCl₂(aq) and Cs₃PO₄(aq) is:
3CaCl₂(aq) + 2Cs₃PO₄(aq) → Ca₃(PO₄)₂(s) + 6CsCl(aq)
Based on the solubility rules, Ca₃(PO₄)₂ is insoluble (precipitate) while CsCl is soluble. Therefore, the reaction is a precipitation reaction.
Now, let's write the net ionic equation for this reaction. The net ionic equation is obtained by removing the spectator ions that are present on both sides of the equation.
The balanced net ionic equation for this reaction is:
3Ca²⁺(aq) + 2PO₄³⁻(aq) → Ca₃(PO₄)₂(s)
In the net ionic equation, the spectator ions Cs⁺ and Cl⁻ are omitted since they are present on both sides of the equation.
So, the net ionic equation is 3Ca²⁺(aq) + 2PO₄³⁻(aq) → Ca₃(PO₄)₂(s).
Therefore, the complete reaction is a precipitation reaction, and the net ionic equation represents the species involved in the formation of the insoluble precipitate Ca₃(PO₄)₂.
To determine the products and classify the reaction as precipitation or acid/base, let's analyze the given chemical equation:
CaCl2(aq) + Cs3PO4(aq) → ?
First, let's determine the ions present in the reaction. In CaCl2, Ca^2+ is the cation, and Cl^- is the anion. In Cs3PO4, Cs^+ is the cation, and PO4^3- is the anion.
To find the products, we will swap the anions and cations from the reactants:
CaCl2(aq) + Cs3PO4(aq) → CaPO4(s) + CsCl(aq)
By swapping the anions and cations, we get CaPO4 as a solid (s), indicating precipitation, and CsCl as an aqueous solution (aq).
Now let's write the net ionic equation. The net ionic equation shows only the species that undergo changes during the reaction, omitting the spectator ions that do not participate. In this case, the spectator ions are Cs^+ and Cl^-.
The ionic equation is:
Ca^2+(aq) + 2Cl^-(aq) + 3Cs^+(aq) + PO4^3-(aq) → CaPO4(s) + 3Cs^+(aq) + 2Cl^-(aq)
Simplifying further, we get the net ionic equation:
Ca^2+(aq) + PO4^3-(aq) → CaPO4(s)
In the net ionic equation, we can see that the calcium ion (Ca^2+) and the phosphate ion (PO4^3-) combine to form a solid calcium phosphate (CaPO4), indicating a precipitation reaction.
So, the complete reaction is a precipitation reaction, and the net ionic equation is Ca^2+(aq) + PO4^3-(aq) → CaPO4(s).