Comparing E300 - Ascorbic acid vs E916 - Calcium iodate
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Found in 3,523 products
Found in 308 products
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Interest over time for 4 keywords in U.S. during the last 10 years.
Interest over time for 2 keywords in U.S. during the last 10 years.
Popular questions
Is ascorbic acid bad for you?
No—ascorbic acid (vitamin C) is considered safe at typical food levels and is essential for health; it’s GRAS in the U.S. and approved in the EU. Very high supplemental doses can cause gastrointestinal upset and, in susceptible people, increase kidney stone risk.
Can dogs have ascorbic acid?
Yes, small amounts in foods are safe, but dogs synthesize their own vitamin C and usually don’t need supplements. High doses may cause diarrhea, so consult a veterinarian before supplementing.
What is ascorbic acid made from?
Commercial ascorbic acid is typically made from glucose (often derived from corn, wheat, or cassava) that’s converted via microbial fermentation and chemical steps into L‑ascorbic acid.
How is ascorbic acid made?
Industrially, D‑glucose is converted to 2‑keto‑L‑gulonic acid by fermentation (or via the older Reichstein process: glucose → sorbitol → L‑sorbose → 2‑KGA) and then chemically cyclized to ascorbic acid. Modern methods use two-step fermentation to improve efficiency.
Is ascorbic acid the same as citric acid?
No—ascorbic acid (E300) is vitamin C and an antioxidant, while citric acid (E330) is a different compound mainly used as an acidulant and does not provide vitamin C.
How to calculate calcium iodate solubility in potassium iodate solution?
Use the dissolution Ca(IO3)2(s) ⇌ Ca2+ + 2 IO3− and Ksp = [Ca2+][IO3−]^2; with initial iodate C from KIO3, solve Ksp = s(C + 2s)^2 for molar solubility s (if C ≫ s, s ≈ Ksp/C^2).
How to calculate solubility of calcium iodate?
In pure water, let s be molar solubility: Ksp = s(2s)^2 = 4s^3, so s = (Ksp/4)^(1/3); convert to g/L by multiplying s by the molar mass of Ca(IO3)2.
How to calculate the concentration of iodate from calcium iodate in 0.1 kio3?
With [IO3−]0 = 0.1 M from KIO3, the iodate contributed by dissolving Ca(IO3)2 is 2s where s solves Ksp = s(0.1 + 2s)^2 (if 0.1 ≫ s, [IO3−] from Ca(IO3)2 ≈ 2Ksp/(0.1)^2).
How to calculate the concentration of iodate from calcium iodate in pure water?
For Ca(IO3)2 in water, [IO3−] = 2s with s = (Ksp/4)^(1/3), so [IO3−] = 2(Ksp/4)^(1/3) assuming activities ≈ concentrations.
How to find molar solubility of calcium iodate?
Write Ksp = [Ca2+][IO3−]^2; in pure water s = (Ksp/4)^(1/3), and in a solution with iodate C (common ion) s is given by Ksp = s(C + 2s)^2 ≈ Ksp/C^2 when C ≫ s.