Indicators and titrations

At 25 °C, 20.0 mL of 0.2 M weak monoprotic acid HX is titrated against 0.2 M NaOH. The pH of the solution (a) at the start of the titration (when NaOH has not been added) and (b) when 10 mL of NaOH is added respectively, are :
Given : $K_a=5\times10^{-4}$, $pK_a=3.3$, $\alpha\ll1$

Identify the colour of compound 'X' in the sequence of the reaction.

20 mL of a solution of acetic acid required 28.4 mL of 0.1 M NaOH for its neutralization. A solution (X) was prepared by mixing 20 mL of the above acetic acid and 14.2 mL of 0.1 M NaOH solution. What is the pH of the solution (X)?
($pK_a$ value of acetic acid is 4.75).

Given below are two statements:

Statement I: Sodium dichromate and potassium dichromate are classified as primary standards in titrimetric analysis.

Statement II: Phenolphthalein is a weak base, therefore it dissociates in acidic medium.

In the light of the above statements, choose the correct answer from the options given below

In a conductometric titration, small volume of titrant of higher concentration is added stepwise to a larger volume of titrate of much lower concentration, and the conductance is measured after each addition.

The limiting ionic conductivity ($\Lambda_0$) values (in $\mathrm{mS\,m^2\,mol^{-1}}$) for different ions in aqueous solutions are given below:

Ions	$\ce{Ag+}$	$\ce{K+}$	$\ce{Na+}$	$\ce{H+}$	$\ce{NO3-}$	$\ce{Cl-}$	$\ce{SO4^2-}$	$\ce{OH-}$	$\ce{CH3COO-}$
$\Lambda_0$	6.2	7.4	5.0	35.0	7.2	7.6	16.0	19.9	4.1

For different combinations of titrates and titrants given in List-I, the graphs of 'conductance' versus 'volume of titrant' are given in List-II.

Match each entry in List-I with the appropriate entry in List-II and choose the correct option.

To form a complete monolayer of acetic acid on 1 g of charcoal, 100 mL of 0.5 M acetic acid was used. Some of the acetic acid remained unadsorbed. To neutralize the unadsorbed acetic acid, 40 mL of 1 M NaOH solution was required. If each molecule of acetic acid occupies $\mathbf{P}\times10^{-23}\,\mathrm{m^2}$ surface area on charcoal, the value of P is _____.

[Use given data: Surface area of charcoal $= 1.5\times10^2\,\mathrm{m^2\,g^{-1}}$; Avogadro's number $(N_A) = 6.0\times10^{23}\,\mathrm{mol^{-1}}$]

The neutralization occurs when 10 mL of 0.1M acid 'A' is allowed to react with 30 mL of 0.05 M base $\mathrm{M(OH)_2}$. The basicity of the acid 'A' is ______.

[M is a metal]

50 mL of 0.1 M $\mathrm{CH_3COOH}$ is being titrated against 0.1 M NaOH. When 25 mL of NaOH has been added, the pH of the solution will be ______ $\times10^{-2}$. (Nearest integer)

(Given : $\mathrm pK_a(\mathrm{CH_3COOH})=4.76$, $\log2=0.30$, $\log3=0.48$, $\log5=0.69$, $\log7=0.84$, $\log11=1.04$)

In base vs. acid titration, at the end point methyl orange is present as

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R.

Assertion A: Phenolphthalein is a pH dependent indicator, remains colourless in acidic solution and gives pink colour in basic medium.

Reason R: Phenolphthalein is a weak acid. It doesn't dissociate in basic medium.

In the light of the above statements, choose the most appropriate answer from the options given below.

The plot of pH-metric titration of weak base $\mathrm{NH_4OH}$ vs strong acid HCl looks like :

A compound 'X' is a weak acid and it exhibits colour change at pH close to the equivalence point during neutralization of NaOH with CH$_3$COOH. Compound 'X' exists in ionized form in basic medium. The compound 'X' is

50 mL of 0.1 M CH$_3$COOH is titrated against 0.1 M NaOH solution. When 10 mL of NaOH is added, the pH of the solution becomes _______ $\times10^{-1}$. (nearest integer)

Given: pKa (CH$_3$COOH) = 4.8, log 2 = 0.3

5.00 mL of 0.10 M oxalic acid solution taken in a conical flask is titrated against NaOH from a burette using phenolphthalein indicator. The volume of NaOH required for the appearance of permanent faint pink color is tabulated below for five experiments. What is the concentration, in molarity, of the NaOH solution?

A solution of 0.1 M weak base (B) is titrated with 0.1 M of a strong acid (HA). The variation of pH of the solution with the volume of HA added is shown in the figure below. What is the p$K_b$ of the base? The neutralization reaction is given by $\ce{B + HA -> BH+ + A-}$.

An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these reactions is given in List II. Match List I with List II and select the correct answer using the code given below the lists:

2.5 mL of $\frac25$ M weak monoacidic base ($K_b=1\times10^{-12}$ at 25 °C) is titrated with $\frac2{15}$ M HCl in water at 25 °C. The concentration of H⁺ at equivalence point is ($K_w=1\times10^{-14}$ at 25 °C)