Comparing E916 - Calcium iodate vs E917 - potassium iodate

Overview

E916 - Calcium iodate

Calcium iodate (E916) is an iodine-containing compound sometimes used to supply iodine or to treat flour. It is uncommon on everyday labels, but you may see it in certain baked goods or specialized products depending on local rules.

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E917 - potassium iodate

Potassium iodate (E917) is a food-grade source of iodine and a strong oxidizing agent. It is mainly used to iodize table salt and, in some places, as a dough improver in bread-making. Many manufacturers now prefer other dough conditioners, but potassium iodate remains common for salt fortification in numerous countries.

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Synonyms
E916
Calcium iodate
E917
potassium iodate
Functions
flour treatment agent
flour treatment agent
Origins
Synthetic
Mineral
Synthetic
Products

Found in 308 products

Found in 81 products

Search rank & volume
#323470 / mo🇺🇸U.S.
#2671.4K / mo🇺🇸U.S.
Awareness score

×0.24
under-aware

×2.45
over-aware

Search volume over time

Interest over time for 2 keywords in U.S. during the last 10 years.

Interest over time for 2 keywords in U.S. during the last 10 years.

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Popular questions

  1. 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).

  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.

  3. 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).

  4. 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.

  5. 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.

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  1. Is potassium iodate dangerous?

    At permitted food-use levels it’s considered safe, but it’s a strong oxidizer and excessive iodine intake can disturb thyroid function (especially in people with thyroid disease, infants, or during pregnancy). As a pure chemical it can irritate eyes/skin and should be handled with care.

  2. Why is potassium iodate banned?

    In the EU/UK it’s not authorized as a food additive (flour treatment agent) due to safety concerns about excess iodine exposure and lack of technological need; however, some countries still allow limited uses such as salt iodization. Regulations vary by country.

  3. What is potassium iodate used for?

    It’s used as an oxidizing flour improver/dough conditioner in some countries and as a stable iodine source for iodizing table salt.

  4. How does sodium bisulfite and potassium iodate react to make iodine reaction with starch equations?

    In acid, bisulfite first reduces iodate to iodide: IO3− + 3 HSO3− → I− + 3 HSO4−; once bisulfite is consumed, iodate oxidizes iodide to iodine: IO3− + 5 I− + 6 H+ → 3 I2 + 3 H2O; iodine then forms I3− with I− (I2 + I− → I3−), which gives the blue starch–iodine complex.

  5. How much of solid kio3 do you need to make 25.00ml of a 0.20m potassium iodate solution? 1.07 g?

    About 1.07 g KIO3 (0.02500 L × 0.200 mol/L = 0.00500 mol; molar mass ≈ 214 g/mol; mass ≈ 1.07 g).

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