pH of a equi-molar solution of Na-carbonate is much higher ( >10 mostly) than of the same Na-bicarbonate (pH roughly 8).
The first contains a (bi-ionic) double base: CO32-
while the 2nd contains one mono-acid and a mono-basic (ampholyte) ion: HCO3-
Sodium benzoate is a preservative, e.g. in beveages, salads, pickles and seafood. It prevents spoilage by yeast at lower pH values (soured products).The other three are not.And only 'sodium bi carbonate' (sodium hydrogen carbonate is a better name) is used as auxillary in baking, called 'baking powder'.
It depends on the concentrations of these substances. However, sodium hydroxide is a very strong base and therefore is capable of producing solutions with high pH values. On the other hand, sodium hydrogen carbonate is weakly acidic, and is therefore capable of producing solutions that are somewhat less than neutral. (Carbonic acid is itself a weak acid.)
In order of increasing pH: (calculated 'pH about'-values are given for 1.0 M solutions)sodium bisulfate Na+(HSO4)- is weak acidic, pKa= 1.92, (pH about 1.0)acetic acid H(OOCCH3) is weakly acidic, pKa= 4.77, (pH about 2.4)neutral: water pKa= 14, pKb= 14 so pH= 7.0sodium acetate Na+(OOCCH3)- is weakly basic, pKb= 9.23, (pH about 9.4)sodium carbonate (Na+)2(CO3)2- is weakly basic, pKb=3.75, (pH about 12.1)
The Kb of Na2CO3 is equal to 2.1 x 10^-4. Carbonate ion is the ion that results from the dissociation of Na2CO3.
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Sodium benzoate is a preservative, e.g. in beveages, salads, pickles and seafood. It prevents spoilage by yeast at lower pH values (soured products).The other three are not.And only 'sodium bi carbonate' (sodium hydrogen carbonate is a better name) is used as auxillary in baking, called 'baking powder'.
It depends on the concentrations of these substances. However, sodium hydroxide is a very strong base and therefore is capable of producing solutions with high pH values. On the other hand, sodium hydrogen carbonate is weakly acidic, and is therefore capable of producing solutions that are somewhat less than neutral. (Carbonic acid is itself a weak acid.)
sodium values will be decreased by haemolysis
In order of increasing pH: (calculated 'pH about'-values are given for 1.0 M solutions)sodium bisulfate Na+(HSO4)- is weak acidic, pKa= 1.92, (pH about 1.0)acetic acid H(OOCCH3) is weakly acidic, pKa= 4.77, (pH about 2.4)neutral: water pKa= 14, pKb= 14 so pH= 7.0sodium acetate Na+(OOCCH3)- is weakly basic, pKb= 9.23, (pH about 9.4)sodium carbonate (Na+)2(CO3)2- is weakly basic, pKb=3.75, (pH about 12.1)
An examination of ka values indicates that carboxylic acids are moderately strong acids. Thus, they undergo acid/base reactions with weak bases such as sodium bicarbonate (ka of which is 10^-7). Having said that, they would also undergo acid/base reactions with stronger bases such as sodium hydroxide. There is no ppt because the products of an acid/base reaction is an ionic salt.
The Kb of Na2CO3 is equal to 2.1 x 10^-4. Carbonate ion is the ion that results from the dissociation of Na2CO3.
The difference electronegativity values of sodium and bromine are; Sodium(Na) 0.9, Bromine(Br) 2.8 thus a difference of 1.9.
A water solution of sodium chloride is neutral.
Water solution of sodium chloride is neutral.
the difference between the electronegativity values of sodium and bromine is 1.9 , which is relatively high in general , high differences suggest ionic bonds.
A water solution of sodium chloride is neutral.
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