cess bas Vaca\" M acid is necessary. The acid must be monoprotic, one acidic hyd
ID: 545889 • Letter: C
Question
cess bas Vaca" M acid is necessary. The acid must be monoprotic, one acidic hydroto Dase titration the calculation is easy usi tration and excess base after the equi V base base * Mbase that is equal to the quivalence now the equivalence number of moles of acid present. So if 46 mL of 0.1000 M base was used t trant point, then there was 4.6 x 103 moles of acid present. Therefore, every mL ot tu 10 moles of acid. Since this is a strong acid, the pH at the start of the titration i The pH at moles of acid/mL of solution). Let's assume that the acid was contained in 100 start would be 3.33. Each 1 mL addition would increase the pH by about 0.01. the pH would be 14-p(OH)-14-(-log (1 x 104 moles base/mL of solution))w would be the original 100 mL +the 47 mL of base titrant. The pH would be 1 point, you know how many moles of base was used an -3 in 100 mL 0. How is this calculation complicated by a weak acid?Explanation / Answer
Strong acids are those which are 100% completely ionized and gives complete hydration of H+ ions as H3O+ (hydronium ion), but weak acids are not 100% ionized, we use a specific term dissociation constant Ka (for weak acids) and Kb (for weak bases).
[H+] = concentration in M (in case of strong acid)
[H+] = ( concentration in M x acid dissociation constant) -------------------> if Ka is very small
Please go through Henderson-hasselbalch equation for buffers as weak acids-weak base concept is mostly used there.
Examples for weak acids: acetic acid, carbonic acid, phosphoric acid, sulfurous acid (H2SO3), oxalic acid etc.
You cannot calculate moles of weak acid as you did for strong acids.
Hope you understand the concept, otherwise please put a comment below so that i will try to resolve your queries.
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