Chemistry Lab: Sodium Bicarbonate Production (NaHCO3) from CO2 + NH3 (NH4OH) + NaCl

Reactions:
NH3(aq) + H2O(l) + CO2(g) ----------} NH4+ (aq) + HCO3-(aq)
Na+(aq) + HCO3-(aq) -------------} NaHCO3(s)
2 NaHCO3(s) + Heat (270 C) -----------} Na2CO3(s) + H2O(g) + CO2(g)
PROCEDURE:
1) IN THE HOOD, add 60 ml of concentrated ammonium hydroxide into a 125 ml Erlenmeyer flask.
2) SLOWLY add 6 g of NaCl to the 125 ml Erlenmeyer flask and swirl the flask to dissolve the sodium chloride.
3) All the NaCl should dissolve. If it does completely dissolve, pour the solution into a 250 ml beaker. (If some NaCl is left undissolved, the undissolved NaCl should be filtered out with a gravity filter).
4) Continuing in the HOOD, add approximately 50 g of CO2(s) (Dry Ice) to the 250 ml beaker using crucible tongs. As it reacts, watch for the formation of a white precipitate and note that observation in RESULTS.
5) While the reaction proceeds, set up a Buchner vacuum filter in the HOOD. Immediately after the reaction has stopped (the dry ice has reacted or sublimed - a very small amount left is OK, the solution must stay very cold - if it warms the precipitate will dissolve), squirt very little dH2O onto the filter paper in the Buchner funnel with the vacuum on just to moisten the filter paper. Swirl the beaker to suspend the white precipitate and rapidly pour it through the Buchner funnel. Continue the vacuum to remove most of the water from the precipitate for about 10 minutes.
6) Take a watch glass (which should be bigger than the top of a 250 ml beaker) and record its mass. Scrape the white precipitate from the filter paper onto the watch glass.
7) Bring the watch glass out of the hood to the bench top. (The rest of the lab may be competed at a bench top outside the hood)
8) Add about 75 ml of water to a 250 ml beaker with a single boiling chip in it and put it on a hot plate to bring it to a VERY GENTLE boil.
9) Place the watch glass (with the precipitate) on top of the beaker with the GENTLY boiling water. Continue to heat it in this fashion until the smell ammonia when wafting over the precipitate is not detected. Make sure to heat long enough to get rid of all the ammonia in the precipitate!!
10) Use a paper towel to remove any condensation from the bottom of the watch glass and then find the mass of the watch glass with the precipitate. Calculate the mass of the precipitate by subtracting the mass of the watch glass. The precipitate is the Sodium Bicarbonate (NaHCO3) product.
11) Take about 0.5 g of the product and place it in a large, Pyrex, test tube. Use a test tube holder to heat the test tube over a bunsen burner flame gently at first. Move it to a hotter part of the flame with time. Continue to heat until no signs of reaction are observed (what signs of reaction should you see? Note the reaction of heated NaHCO3). When you no longer see any signs of reaction and the sample appears visibly smaller than before heating started, set the test tube aside to cool to room temperature. This product should now be Na2CO3.
12) Take a small sample (about 0.1g) of the first product (NaHCO3) and add it to a clean, dry, small test tube and label it. Repeat this in a second test tube with the second product. Add 1.0 ml of dH2O to each of the test tubes and finger vortex each to dissolve the products in their test tubes.
13) Use a piece of pH paper to determine the pH of each product solution.
14) Calculate the theoretical yield: a) Calculate moles of NaCl used (mass NaCl)/(MM of NaCl)
b) Calculate the theoretical moles of NaHCO3 that should be produced (based on balanced equation)
c) Calculate the theoretical mass of NaHCO3 that should be produced (moles of NaHCO3 x MM of NaHCO3)
15) Calculate % yield in RESULTS. [(Actual Mass Produced)/(Theoretical Mass Calculated)]
RESULTS:
Observations of the first reaction:
Mass of empty, dry watch glass ______ g
Mass of watch glass with first product ____ g
Calculated mass of the first product (NaHCO3) ____ g
Calculation of the Theoretical Yield of NaHCO3:
Moles of NaCl used _____moles (mass NaCl)/(MM of NaCl)
Theoretical Moles of NaHCO3 that should be produced ____ moles (based on the ratio in the balanced equation)
Theoretical Mass of NaHCO3 that should be produced ____g (moles of NaHCO3)x( MM of NaHCO3)
Calculation of % Yield:
% Yield _____ %
pH of NaHCO3 solution ____ pH of Na2CO3 solution ____

[@houssameddinesiad8737]

Solvay process

[@raxxbones9642]

Music is SOOOO LOUD. Hard to focus on video cause even at low volume it's loud. Good video though

[@georgesmith9437]

Music is optional! You can mute your speakers.😊

[@ajingolk7716]

In the first reaction can we say that ammonium chloride and sodium hydroxide are formed?

[@georgesmith9437]

You could say that ammonium & bicarbonate ions are formed in the first reaction. Then bicarbonate ions react with sodium ions to form the sodium bicarbonate precipitate.

[@ajingolk7716]

@@georgesmith9437 first reaction ammonium hydroxide and sodium chloride 🤔

[@georgesmith9437]

@ajingolk7716 The double replacement reaction you are suggesting would not occur. It would require the formation of a precipitate. Ammonium chloride and sodium hydroxide are both aqueous solutions and therefore the double replacement reaction of ammonium hydroxide and sodium chloride would not occur.

[@ajingolk7716]

@@georgesmith9437 so we have ions swiming in solution, ammonium chloride dissolves in some solvent badly where sodium hydroxide dissolves well but any way thank for replaying to me i apreciate that. I have another reaction if you can help me out with 🙏 can potassium sulfate or sodium sulfate react with calcium carbonate?

[@fernandohafez6064]

Is there a problem with adding water in the NaCl + NH4O4 reaction?

[@georgesmith9437]

Yes. Sodium bicarbonate is moderately soluble in water at about 10g/100ml at room temperature. Adding water will cause a loss in product that can be collected by filtering due to its solubility in water.