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Will calcium hydroxide react with sodium bicarbonate?
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+ Chemical reactions
+ Hydroxides
+ Sodium hydroxide
+ Sodium
+ Chemistry
+ Calcium
+ Sodium bicarbonate
Posted by
Justin Harper
Will calcium hydroxide react with sodium bicarbonate?
Sure, assuming we are talking about aqueous solutions of the two. The reaction goes like this:
CaSO4(aq) + NaOH(aq) → Ca(OH)2(s) + Na2SO4(aq)
where ‘aq’ means aqueous or in solution and ‘s’ means solid. Calcium hydroxide (Ca(OH)2) is not very water soluble (Ksp = 5.5 * 10^-6) and precipitates out of solution, driving the overall process.
Edit:
Well, after reading the other answers I believe an edit is in order. I did neglect to discuss the solubility of CaSO4 (Ksp=2.4 * 10^-5). So, neither CaSO4 nor Ca(OH)2 are particularly soluble. CaSO4 has enough solubility such that it will react with the base and, as consumed, more will dissolve…and the process will continue as long as something is driving it.
I still think that Ca(OH)2 will ppt. Remember, the expression for Ksp for Ca(OH)2 is:
Ca(OH)2 = Ca(2+) + 2 HO-
If you add NaOH, you are adding HO- and, in a very effective manner, driving the equilibrium to Ca(OH)2 (solid ppt) which will, in turn, shift the equilibrium to the right.
Sure, assuming we are talking about aqueous solutions of the two. The reaction goes like this:
CaSO4(aq) + NaOH(aq) → Ca(OH)2(s) + Na2SO4(aq)
where ‘aq’ means aqueous or in solution and ‘s’ means solid. Calcium hydroxide (Ca(OH)2) is not very water soluble (Ksp = 5.5 * 10^-6) and precipitates out of solution, driving the overall process.
Edit:
Well, after reading the other answers I believe an edit is in order. I did neglect to discuss the solubility of CaSO4 (Ksp=2.4 * 10^-5). So, neither CaSO4 nor Ca(OH)2 are particularly soluble. CaSO4 has enough solubility such that it will react with the base and, as consumed, more will dissolve…and the process will continue as long as something is driving it.
I still think that Ca(OH)2 will ppt. Remember, the expression for Ksp for Ca(OH)2 is:
Ca(OH)2 = Ca(2+) + 2 HO-
If you add NaOH, you are adding HO- and, in a very effective manner, driving the equilibrium to Ca(OH)2 (solid ppt) which will, in turn, shift the equilibrium to the right.
Sure, assuming we are talking about aqueous solutions of the two. The reaction goes like this:
CaSO4(aq) + NaOH(aq) → Ca(OH)2(s) + Na2SO4(aq)
where ‘aq’ means aqueous or in solution and ‘s’ means solid. Calcium hydroxide (Ca(OH)2) is not very water soluble (Ksp = 5.5 * 10^-6) and precipitates out of solution, driving the overall process.
Edit:
Well, after reading the other answers I believe an edit is in order. I did neglect to discuss the solubility of CaSO4 (Ksp=2.4 * 10^-5). So, neither CaSO4 nor Ca(OH)2 are particularly soluble. CaSO4 has enough solubility such that it will react with the base and, as consumed, more will dissolve…and the process will continue as long as something is driving it.
I still think that Ca(OH)2 will ppt. Remember, the expression for Ksp for Ca(OH)2 is:
Ca(OH)2 = Ca(2+) + 2 HO-
If you add NaOH, you are adding HO- and, in a very effective manner, driving the equilibrium to Ca(OH)2 (solid ppt) which will, in turn, shift the equilibrium to the right.
Sure, assuming we are talking about aqueous solutions of the two. The reaction goes like this:
CaSO4(aq) + NaOH(aq) → Ca(OH)2(s) + Na2SO4(aq)
where ‘aq’ means aqueous or in solution and ‘s’ means solid. Calcium hydroxide (Ca(OH)2) is not very water soluble (Ksp = 5.5 * 10^-6) and precipitates out of solution, driving the overall process.
Edit:
Well, after reading the other answers I believe an edit is in order. I did neglect to discuss the solubility of CaSO4 (Ksp=2.4 * 10^-5). So, neither CaSO4 nor Ca(OH)2 are particularly soluble. CaSO4 has enough solubility such that it will react with the base and, as consumed, more will dissolve…and the process will continue as long as something is driving it.
I still think that Ca(OH)2 will ppt. Remember, the expression for Ksp for Ca(OH)2 is:
Ca(OH)2 = Ca(2+) + 2 HO-
If you add NaOH, you are adding HO- and, in a very effective manner, driving the equilibrium to Ca(OH)2 (solid ppt) which will, in turn, shift the equilibrium to the right.
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Well it should….you gots weak acid and strong base…and thus…
[math]Ca(OH)_{2}(aq) + Na^{+}HCO_{3}^{-}(aq) ightarrow CaCO_{3}(s)downarrow + NaOH(aq) + H_{2}O(l)[/math]
Calcium hydroxide is fairly insoluble, but calcium carbonate is even less so … you should see a fine white precipitate deposit from solution….
Well it should….you gots weak acid and strong base…and thus…
[math]Ca(OH)_{2}(aq) + Na^{+}HCO_{3}^{-}(aq) ightarrow CaCO_{3}(s)downarrow + NaOH(aq) + H_{2}O(l)[/math]
Calcium hydroxide is fairly insoluble, but calcium carbonate is even less so … you should see a fine white precipitate deposit from solution….
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