The reduction of cinnamic acid by sodium borohydride?
111102
cinnamic acid is reduced to the aldehyde and can be further reduced to the alcohol.\nsodium borohydride is caustic b/c the hydride ion(H-1) reacts with water to produce hydrogen gas and the hydroxide ion.  it acts as a strong base.
128824
NaBH4 functions as BH4-, which donates a hydride (a hydrogen with a negative charge) to the aldehyde or ketone that you're working with. The product is a sodium salt/alkoxide. Water or HCl (acid) will protonate the alkoxide to generate the alcohol that you need. \n\nThe gas formed was probably hydrogen, from when the HCl reacted with the Sodium borohydride.
125676
a fairly lengthy description can be found at\n\nhttp://apps3.fao.org/jecfa/additive_specs/docs/0/additive-0465.htm
971081
Formula: you more or less answered your question yourself. It is any combination of glycerine esters with any combination of these acids.\n\nReaction with NaOH is saponification, resulting in glycerine and the free acids (or more specifically, acid rests as dissolved salts).\n\nReaction with hydrogen in the presence of Pt or Raney-Ni as catalysts will ultimately produce the triglycerides of the corresponding saturated acids. This is known as "hardening" of fats since saturated fatty acids tend to produce solid fats whereas unsaturated fatty acid triglycerides of comparable mass remain liquid at the same temperatures.\n\nReaction with bromine will result in electrophile addition of Bromine on the double bonds of the unsaturated acids.
570827
It's called a reducing agent.
952998
The reductive dissolution of goethite ( -FeOOH) and hematite ( -Fe 2 O 3 ) by phenolic reductants has been examined in order to improve the understanding of iron transformations in soils, sediments and aquifers. Rates of goethite reductive dissolution by hydroquinone increased as the pH was increased from pH 1.8 to 4.65, arid the following reaction stoichiometry was obeyed: 2 - FeOOH + QH 2 = 2 Fe 2+ + Q + 4 OH - . As the pH was increased from pH 4.5 to 6.0, the reductive dissolution rate decreased to below the detection limit. At pH 3.4, the reductive dissolution of hematite was two orders of magnitude slower than goethite. The relationship between structure and reactivity was examined for a series of mono-, di-, and tri-hydroxybenzene reductants. Rates of reductive dissolution decreased in the following order: catechol ~- hydroquinone 〉 3,4-dihydroxybenzoic acid 〉 resorcinol-phenol-4-hydroxybenzoic acid.
43485
Well, I'm not gonna try to explain this or anything, but check this website out:\n\nhttp://www.usm.maine.edu/~newton/Chy251_253/Lectures/Esterification/Esterification.html\n\nScroll down to "Scheme 2: Saponification of an Ester," and that explains the reaction process fairly well.  I don't know if this is what you're looking for, but I hope it helps!
606155
NaOH + HCl ---> NaCl + H20
851560
solution...Bicarbonate and sodium. :)
182435
Well, there are a lot.\n\nSubstiution:\n\nR-OH + SOCl2 ---> R-Cl\n\nElimination\n        \nR-R'-OH ---->  R=R' + H20 (with an acid catalyst and heat)\n\nReduction:\n\nR-OH ---> R-CH3 (Barton Reduction)\n\nOxidation:\n\nR-OH ---> R-COOH\nR-OH ---> R=O\n\nThen alcohols can act as nucleophiles, so there is a another set of reactions. But I've listened enough, imho.
789348
This is a strange question because acid-base reactions are never redox, so there is never any such thing as an acid base reduction. The reaction between acids and bases is called neutralisation.
1072536
The liquid you want is a solution of boracic (or boric) acid.
795833
LHS:\nPb4+\nSn2+\nCl-\n\nRHS:\nPb2+\nSn4+\nCl-\n\nOxidation number of Pb in PbCl4 decreases = it is reduced = it oxidizes the other = it is the oxidizing agent
269689
Hope this helps:\n\nhttp://jchemed.chem.wisc.edu/Journal/Issues/1997/Feb/abs210.html
152537
Citric acid is a weak acid, while sodium hydroxide is a strong base. The sodium would fall off the hydroxide (because it's strong), so the reaction would be:\n\nHC6H7O7 + OH- --> H2O + C6H7O7
777907
Ninhydrin(Triketohydrindane hydrate)----C9H6O4\nLugol(Iodine Potassium-Iodide)-------  KI3 \nBiuret(Allophanamide)-----NH2CONHCONH2\n\nI cant find a chemical formula for benedict. But i found a equation.\n\nBenedict's reagent (also called Benedict's solution or Benedict's test) is a reagent used as a test for the presence of monosaccharides (such as glucose and fructose); it is also used for some disaccharides like maltose, or more generally for the presence of aldehydes, in a solution.\n\nBenedict's reagent contains blue copper(II) sulphate (CuSO4)· 5H2O which is reduced to red copper(I) oxide by aldehydes, thus oxidizing the aldehydes to carboxylic acids. The copper oxide is insoluble in water and so precipitates. The color of the final solution ranges from green to brick red depending on how many of the copper(II) ions are present. Benedict's test cannot be used to detect the presence of aromatic aldehydes.
794274
B, though its even more common as K2Cr2O7\n\nby coincidence, C, Na and H2 happen to be quite good reducing agents.