If you are titrating a base, using a weak acid as titrant would lead to the formation of a buffer as you added the weak acid. The weak acid would react with the base to form the salt of the weak acid + water, and this would buffer any changes in pH, thus making the titration meaningless.
The formic acid is a weak acid.
Citric acid is considered to be a weak acid.
In order to have an effective buffer, one needs to have a weak acid or a weak base, and the salt (conjugate) of that weak acid or weak base. Examples would be :weak acid/conjugate base: acetic acid/sodium acetateweak base/conjugate acid: ammonia/ammonium chloride
Oxalic acid is a relatively strong weak acid. It has pKa1=1.27 and pKa2=4.28.
H3PO4 is a weak acid, and a weak acid is not sufficient for a buffer.
Sodiumj carbonate is a weak alakli and propanoic acid is a weak acid so you cannot use a weak acid and a weak alkali in an experiment as they wouldn't react properly. It would be difficult to find the indicator.
It is a weak acid mainly used for TITRATION
Carbonic acid is a weak acid .This acid is used to carbonate beverages.
strong acid- hydrochloric acid - used for digestion as a secretion of stomach weak acid- citric acid - used for maintaining salts in body
Titration is the controlled neutralisation of an acid and a base. If the titration is done using a weak acid and a strong base, it can be analysed in detail and all concentrations of the aqueous species at any volume addition of the titrant can be determined.
It depends on the acid or base used. For strong acid vs. strong base, phenolphthalein can be used as indicator. For strong acid vs. weak base, methyl orange can be used as indicator. For weak acid vs. strong base, phenolphthalein can be used as indicator.
The formic acid is a weak acid.
H2CO3 Carbonic acid is a weak acid because it does not dissociate completely in solution making it a weak electrolyte.
Phosphoric acid 85% is the highest purity of this type of acid available in the market. Which is most used in food grade. Phosphoric acid is in the classification of weak acids.
There are three major differences between strong acid/strong base and weak acid/strong base titrations. For weak acid/strong base titrations: 1. The weak-acid solution has a higher initial pH. 2. The pH rises more rapidly at the start, but less rapidly near the equivalence point. 3. The pH at the equivalence point does not equal 7.00. (should be >7) In an acid-base titration, there is a 1:1 acid:base stoichiometry, so the equivalence point is the point where the moles of titrant added equals the moles of substance initially in the solution being titrated. Therefor the strength of the acid or base should not have an affect on the quantity of base required, only on the pH of the equivalence point. The number of moles of titrant and solution will have an effect on the quantity of base required.
Yes it is a weak acid
Weak.