# Metathesis of sodium phosphate and calcium nitrate

We have 3 K atoms on the right but only 1 on the left. Reactions That Increase the Number of Ions in Solution Thus far, we have been able to write net ionic equations for our "molecular" equations because ions were removed from solution.

These two cases are at opposite ends of the spectrum, and it is important to know in which case each event occurs: Sometimes, when working on "molecular" or complete formula equations, we might complete a metathesis reaction where no reaction actually occurs.

An example is the reaction of hydrochloric acid with sodium sulfide: For example, calcium carbonate, CaCO3 is insoluble in water, but will dissolve in an aqueous hydrochloric acid solution, because the acid converts the insoluble calcium carbonate into calcium chloride, CaCl2, which is soluble.

The CaCO3 is in solid form, so its ions are in close proximity in the crystal lattace. If we merely replace each chemical name with its correct chemical formula we get the following equation.

The most commonly cited examples are acids reacting with carbonates, sulfites, and sulfides to form gases that escape from the solution. Try your hand at these for practice: The problem has already given away, the fact that sodium phosphate and potassium nitrate are soluble in water, because we are supposed to be mixing aqueous solutions of them, which we could not have if they were not soluble.

Litmus paper is red when exposed to an acidic solution and blue when exposed to a basic solution. The complete formula equation can be deceptive, leading us to see a reaction where there is none.

In this case, we should go back to the complete formula equation and write "NR" for "No Reaction" after the arrow. However, the sodium nitrate and potassium phosphate are formed in the reaction, and it is possible that one of these is not soluble in water.

A sodium nitrate solution should contain sodium ions and nitrate ions; a potassium phosphate solution should contain potassium ions and phosphate ions.

However, it really makes no difference in what order the reactants are listed -- it is still the same reaction. Notice that the mixed solutions can still be considered to contain the original sodium phosphate and potassium nitrate, because a sodium phosphate solution is characterized as containing sodium ions and phosphate ions, while a potassium nitrate solution is characterized as containing potassium ions and nitrate ions.

As soon as they shared a common aqueous medium, they immediately began assembling to form the solid. When we mix the solutions, nothing happens.

The online practice quiz would ask: Thus, there is no net ionic equation, and therefore, no reaction. The solution shown in Figure 3 b satisfies both criteria, thus the original reactants are still present.

Criteria for Success This project is evaluated by written quiz. If so, what is the balanced reaction equation? These rules are summarized in tables in most general chemistry textbooks. The solution just has sodium ions, potassium ions, chloride ions, and nitrate ions floating around separately.

Like REDOX reaction, these reactions span more than one of the four traditional reactions classes combination, decomposition, displacement, and metathesis.

Look for a chapter on nomenclature for more details on material in this project. If there is any doubt, we should attempt to work out the net ionic equation for our proposed reaction. Acids -- What Are They?

Neither of these compounds are soluble in water. We can solve this problem by putting a coefficient of 3 in front of NaNO3.a) Iron(III) chloride (aq) and cesium phosphate (aq) b) Sodium phosphate(aq) and calcium chloride(aq) This is the end of the preview.

Sign 33%(3). Experiment Six – Precipitation Reactions Objective Sodium Phosphate #9 - Silver Nitrate & Sodium Sulfate #10 - Silver Nitrate & Sodium Carbonate Sodium phosphate (aq) and calcium chloride (aq) Molecular: Spectators: Title: Experiment 2: The Use of Volumetric Glassware.

How can a chemical equation of sodium phosphate reacting with calcium nitrate to produce sodium nitrate and calcium phosphate be balanced? 2Na 3 PO 4 + 3Ca(NO 3) 2 --> 6NaNO 3 + Ca 3 (PO 4) 2.

Mar 06,  · Sodium phosphate reacts with calcium nitrate to produce sodium nitrate plus calcium phosphate?

Please help me balance, predict and classify this equation. I have an idea of what to do, but i want to clarify, thanks:)Status: Resolved.

A solution of sodium hydroxide is added to a solution of calcium hydrogen carbonate until the number of moles of sodium hydroxide added is twice the number of moles of the calcium salt.

Equal volumes of M hydrochloric acid and M sodium monohydrogen phosphate are mixed. calcium acetate + sodium carbonate Æ 5. ammonium chloride + mercury(I) acetate Æ 6.

calcium nitrate + hydrochloric acid Æ Double-Replacement Reactions In these reactions, all you do is look at the names of the reactants, and "switch partners". Just calcium nitrate + hydrochloric acid Æ calcium chloride + nitric acid Ca(NO 3) 2.

Metathesis of sodium phosphate and calcium nitrate
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