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2 RCOOH + CaH2 ----> 2 RCOH + Ca(OH)2 Would this work? Might it be cheaper than sodium borohydride?
Sodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.
Wrong, it will reduce them at high temperatures with no solvent. Once again look up Rohm and Haas The Sodium borohydride digest.
Quote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.
Practical or not, You stated NaBH4 it's self will not reduce carboxylic acids. However, it can.Quote from: discodermolide on May 17, 2011, 08:08:46 AMQuote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.
Quote from: BenFrank1 on May 12, 2011, 09:31:51 PM 2 RCOOH + CaH2 ----> 2 RCOH + Ca(OH)2 Would this work? Might it be cheaper than sodium borohydride?CaH2 is not a reducing agent for carboxylic acids you will get H2 and the calcium salt of the acid, nor is sodium borohydride. Look up the Rosenmund reduction
Quote from: BenFrank1 on May 17, 2011, 11:17:45 AMPractical or not, You stated NaBH4 it's self will not reduce carboxylic acids. However, it can.Quote from: discodermolide on May 17, 2011, 08:08:46 AMQuote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.NaBH4 decomposes at 300°C and above. I would suggest that it is the H2 produced under these conditions that causes the reduction with the boron coordinating to the carbonyl oxygen and the acid oxygen assisting hydrogenation.
Possibly. But tell me this, how could CaH2 react with acetic acid to produce H2. My point being you stated you will get H2 and the calcium salt of the acid.Quote from: discodermolide on May 13, 2011, 12:56:59 AMQuote from: BenFrank1 on May 12, 2011, 09:31:51 PM 2 RCOOH + CaH2 ----> 2 RCOH + Ca(OH)2 Would this work? Might it be cheaper than sodium borohydride?In the same way that any acid or water will react with a hydride of a group I orIi metal to give H2 and the metal saltCaH2 is not a reducing agent for carboxylic acids you will get H2 and the calcium salt of the acid, nor is sodium borohydride. Look up the Rosenmund reduction
Quote from: BenFrank1 on May 12, 2011, 09:31:51 PM 2 RCOOH + CaH2 ----> 2 RCOH + Ca(OH)2 Would this work? Might it be cheaper than sodium borohydride?In the same way that any acid or water will react with a hydride of a group I orIi metal to give H2 and the metal saltCaH2 is not a reducing agent for carboxylic acids you will get H2 and the calcium salt of the acid, nor is sodium borohydride. Look up the Rosenmund reduction
The melting point of NaBH4 is 400 C.Quote from: discodermolide on May 17, 2011, 11:46:31 AMQuote from: BenFrank1 on May 17, 2011, 11:17:45 AMPractical or not, You stated NaBH4 it's self will not reduce carboxylic acids. However, it can.Quote from: discodermolide on May 17, 2011, 08:08:46 AMQuote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.The MPt is not an indicator for stability, thermal decomposition can begin well before the MPt.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.NaBH4 decomposes at 300°C and above. I would suggest that it is the H2 produced under these conditions that causes the reduction with the boron coordinating to the carbonyl oxygen and the acid oxygen assisting hydrogenation.
Quote from: BenFrank1 on May 17, 2011, 11:17:45 AMPractical or not, You stated NaBH4 it's self will not reduce carboxylic acids. However, it can.Quote from: discodermolide on May 17, 2011, 08:08:46 AMQuote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.The MPt is not an indicator for stability, thermal decomposition can begin well before the MPt.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.NaBH4 decomposes at 300°C and above. I would suggest that it is the H2 produced under these conditions that causes the reduction with the boron coordinating to the carbonyl oxygen and the acid oxygen assisting hydrogenation.
Practical or not, You stated NaBH4 it's self will not reduce carboxylic acids. However, it can.Quote from: discodermolide on May 17, 2011, 08:08:46 AMQuote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.The MPt is not an indicator for stability, thermal decomposition can begin well before the MPt.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.
Quote from: BenFrank1 on May 17, 2011, 07:32:46 AMSodium borohydride can reduce carboxylic acids, look up; Rohm and Haas The sodium Borohydride Digest!, I do think that Cah2 can reduce %100 percent acetic acid to acetaldehyde in the absence of solvents.The MPt is not an indicator for stability, thermal decomposition can begin well before the MPt.NaBH4 itself will not reduce carboxylic acids. You need to generate some BH3, which does reduce them.