Calcium chloride and Sodium carbonate Reaction | CaCl2 + Na2CO3

Calcium chloride (CaCl2) reacts with sodium carbonate (Na2CO3) and form calcium carbonate (CaCO3) and sodium chloride (NaCl). Calcium carbonate is a white precipitate and insoluble in water.

In this tutorial, we will discuss followings.

Reaction of CaCl2 and Na2CO3 and balanced equation

As mentioned earlier, calcium carbonate and sodium chloride are given as results. To give these products, an aqueous phase is required because cations and anions should be dissociated in water. In solid phase, free cations and anions are not available.

Both CaCl2 and Na2CO3 are soluble in water and dissociates completely to ions. In aqueous solution, CaCl2 dissociates to Ca2+ and Cl- ions. As well, Na2CO3 dissociates to Na+ and CO32- ions.

Balanced equation of CaCl2 and Na2CO3

CaCl2(aq) + Na2CO3(aq) → CaCO3(s) + 2NaCl(aq)

When reaction performs, all reactants and products are in aqueous state. According to the balanced equation, one mole of CaCl2 reacts with one mole of Na2CO3 and gives one mole of CaCO3 and one mole of NaCl respectively.

Reactants of the reaction: CaCl2 and Na2CO3

Calcium chloride (CaCl2)

Calcium chloride is a white solid at room temperature and soluble in water to give a colourless aqueous solution. When CaCl2 is dissolved in water, it dissociates to Ca2+ and Cl- ions.

Sodium carbonate (Na2CO3)

Sodium carbonate is a white solid and soluble in water. Aqueous sodium carbonate solution is colourless and dissociates to Na+ and CO32- ions.

Products of the reaction: CaCO3 and NaCl

Calcium carbonate (CaCO3)

Calcium carbonate is insoluble in water and deposited as a white precipitate.

Sodium chloride (NaCl)

Sodium chloride is a white solid at room temperature and highly soluble in water.

Change of oxidation numbers

Oxidation numbers of atoms are not changed during the reaction. Therefore, this reaction is not a redox reaction.

Physical and chemical observation of CaCl2 and Na2CO3 reaction

Here, we will see some physical observations and chemical properties changes during the reaction.

Colour and physical state changes

• Both CaCl2 and Na2CO3 are colourless solutions.
• One product, CaCO3 is a white precipitate while other product NaCl exist as in the aqueous phase. So, you can see a white solid at the bottom of the solution at the end of the reaction.

Safety, health hazards and environmental impacts due to NaNO2, HCl, HNO2

• CaCl2: Irritant
• Na2CO3: Irritant
• CaCO3: Corrosive and irritant
• NaCl: An eye irritant, if large amounts are ingested toxic characteristics are possible

Questions

Ask your chemistry questions and find the answers

You are given 0.01 mol dm-3 CaCl2 50 cm3 aqueous solution and 0.01 mol Na2CO3 50 cm3 aqueous solution. Both of these two solutions are mixed.

1. Write the balanced equation between CaCl2 and Na2CO3
2. Calculate how much CaCO3 is deposited in the aqueous solution.
3. Mention what assumptions are made by you during the calculations.

1. Balanced equation of CaCl2 and Na2CO3

CaCl2(aq) + Na2CO3(aq) → CaCO3(s) + 2NaCl(aq)

2. Calculate how much CaCO3 is deposited in the aqueous solution.

To decide how much CaCO3 is formed, you should calculate followings.

• How much CaCl2 and Na2CO3 are there in solutions?: Use n = CV equation.
• How much CaCl2 and Na2CO3 are reacted: Apply Stoichiometric balanced equation.

Amount of CaCl2

• Amount of CaCl2 in CaCl2 aqueous solution = 0.01 mol dm-3 * 50 * 10-3 dm3
• Amount of CaCl2 in CaCl2 aqueous solution = 0.0005 mol

Amount of Na2CO3

• Amount of Na2CO3 in Na2CO3 aqueous solution = 0.01 mol dm-3 * 50 * 10-3 dm3
• Amount of Na2CO3 in Na2CO3 aqueous solution = 0.0005 mol

Tabulated calculated values as below. According to the stoichiometric balanced equation, we can decide quantities of reacted (reactants) and quantities of generated (products).

So, all CaCl2 and Na2CO3 are consumed during the reaction. We can calculate how much CaCO3 is precipitated in the solution.

Amount of CaCO3

• Amount of CaCO3 = 0.05 mol * 100 g mol-1
• Amount of CaCO3 aqueous solution = 5 g

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