Comparing E200 - Sorbic acid vs E237 - Sodium formiate
Overview
Synonyms
Products
Found in 6,918 products
Found in 5 products
Search rank & volume
Awareness score
Search volume over time
Interest over time for 2 keywords in U.S. during the last 10 years.
Interest over time for 3 keywords in U.S. during the last 10 years.
Popular questions
Is sorbic acid bad for you?
Not for most people—it's a widely approved food preservative with low toxicity at permitted levels; rare individuals may experience mild irritation or digestive upset with high exposure.
Is sorbic acid safe for dogs?
Yes, when used at regulated amounts as a preservative in dog foods it’s considered safe; excessive intake may cause stomach upset in sensitive dogs.
Is sorbic acid safe?
Yes—it's approved in the EU (E200) and generally recognized as safe (GRAS) in the U.S. at typical food-use levels, with adverse effects uncommon at those amounts.
What is sorbic acid made from?
Commercially it’s synthesized from crotonaldehyde and ketene; it also occurs naturally in small amounts in rowan (mountain ash) berries.
Is sorbic acid natural?
It occurs naturally in some fruits, but the sorbic acid used in foods is almost always synthetically produced and is chemically identical to the natural compound.
Is sodium formate an acid or base?
It’s the sodium salt of formic acid; in water the formate ion acts as a weak base, so its solutions are mildly basic.
Is sodium formate a strong base?
No—it's a weak base; the formate ion only hydrolyzes slightly in water (formic acid pKa ≈ 3.75).
. what is the effect on equilibrium when sodium formate is added to a solution of formic acid?
It adds the common ion (formate), shifting HA ⇌ H+ + A− to the left, suppressing dissociation and creating a buffer; the solution becomes less acidic than pure formic acid.
1l solution of .05m sodium formate. what is final ph if 12ml of 1.0m hcl is added?
About pH 4.25. Reaction converts 12 mmol formate to formic acid, leaving ~38 mmol A− and 12 mmol HA; with pKa ≈ 3.75, pH ≈ 3.75 + log(38/12) ≈ 4.25.
Determind how much formic acid and sodium formate to make buffer?
Specify the target pH and total buffer concentration, then use Henderson–Hasselbalch: [A−]/[HA] = 10^(pH − pKa). For example, at pH 4.25 with 0.10 M total buffer in 1 L, you’d need ~0.076 mol sodium formate and ~0.024 mol formic acid.