Assertion : In a titration of weak monoprotic acid with strong base, the `pH` at the half equivalent point is `pK_(a)`. Reason : At half equivalence point, it will form acidic buffer at its maximum capacity where [acid]`=`[salt].
A
If both the statements are TRUE and STATEMENT-2 is the correct explation of STATEMENT-1
B
If both the statements are TRUE AND STATEMENT-2 is NOT the correct explanation of STATEMENT-1
During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:
A 20.0 mL sample of a 0.20 M solution of the weak diprotic acid H_(2)A is titrated with 0.250 M NaOH. The concentration of solution at the second equivalent point is:
What is the pOH of 0.1 M KB (salt of weak acid and strong base) at 25^(@)C ? (Given : pK_(b) of B^(-) =7)
A 1.025 g sample containing a weak acid HX (mol. Mass=82) is dissolved in 60 mL. water and titrated with 0.25 M NaOH. When half of the acid was neutralised the pH was found to be 5.0 and at the equivalence point the pH is 9.0. Calculate mass precentage of HX in sample :
10 mL of H_(2)A (weak diprtic acid) solutio is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following obserbation is made Ip pH of the solution at first equivalence point is pH_(1) and at secnd equibalence point is pH_(2^.) Calculate the value of (pH_(2)-pH_(1)) at 25^(@)C Given for H_(2)A,pK_(a_1) =4.6 and pK_(a_2) =8, log 25=1.4
The enthalpy of neutralization of a Weak monoprotic acid (HA) in 1 M solution with a strong base is -55.95 KJ/mol . If the unionized acid required 1.4 KJ/mol heat for it's comptate ionzatation and enthalpy of netralization of the strong monobasic acid with a strong monoacidic base is -57.3 KJ/mol . What is the % ionzation of the weak acid in molar solution ?
Calcium lactate is a salt of weak organic acid and strong base represented as Ca(LaC)_(2). A saturated solution of Ca(LaC)_(2) contains 0.13 mole in 0.5 litre solution. pOH of solution is 5.60. What is pK_(a) of lactic acid?
Is CH_3COOH strong or weak acid? Will its 0.1 M solution have pH more or less than HCl of same concentration?
Assertion : Aspirin can cause ulcer in stomach when taken empty stomach. Reason : Aspirin gets hydrolysed to salicylic acid in stomach where pH is 2.
Solution of a weak acid and its anion (that is,its conjugate base) or of a base and its common cation are buffered. When we add a small amount of acid or base to any one of the, the pH of solution change very little. pH of buffer solution can be computed as for acidic buffer : pH=pK_(a)+ log.(["Conjugate base"])/(["Acid"]) for basic buffer : pOH=pK_(b)+log.(["Conjugate acid"])/([Base]) It is generly accepted that a has useful buffer cpacity (pH change resisting power) provided that the value of [salt or conjugate base] /[acid] for acidic buffer lies within the range of 1 : 10 to 1. Buffer capacity is maximum when [conjugate base] = [acid] Useful buffer range of weak acid HA(K_(a)=10^(-5)) is :
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
