Boric acid can be titrated against sodium hydroxide using phenolphthalein as an indicator only in the presence of polyhydroxy compounds like glycol. Glycerol etc. Give reason.

Boric acid can be titrated against sodium hydroxide using methyl orange as indicator only in the presence of polyhydroxy compounds wlike catechol, manniton etc. explain.

Aqueous solution of orthoboric acid can be titrated against sodium hydroxide using phenolphthalein indicator only in presence of

Compound (A) on reaction with iodine in the solvent diglyme gives a hydride (B) and hydrogen gas. The product (B) is instantly hydrolysed by water or aqueous alkali forming compound ( C) and liberating hydrogen gas. The compound ( C) in aqueous solution behaves as a week mono basic acid. But in presence of certain organic polyhydroxy compound behaves as a strong monobasic acid. The hydride (B) in air catches fire spontaneously forming oxide which gives coloured beads with transition metal compounds. Aqueous solution of product (C) can be titrated against sodium hydroxide using phenolphthalein indicator only in presence of:

Assertion: In the titration of Na_(2)CO_(3) with HCl using methyl orange indicator, the volume of acid required is twice that of the acid required using phenolphthalein as indicaton. Reason: Two moles of HCl are required for the complete neutralisation of one mole of Na_(2)CO_(3) .

20mL of 0.1M solution of compound Na_2CO_3 .NaHCO_3. 2H_2O is titrated against 0.05 M HCI . x mL of HCI is used when phenolphthalein is used as an indicator and y mL of HCI is used when methly orange is the indicator in two separate titrations. Hence (y-x) is :

20 mL of 0.1 M solution of compound NaCO_(3).NaHCO_(3).2H_(2)O is titrated against 0.05 M HCL. X mL of HCL is used when phenolphthalein is used as an indicator and y mL of HCL is used when methly orange is the indicator in two separate titrations. Hence (y-x) is:

The table below gives the results of three titrations carried out with 0.200 M HCl to determine the molarity of a given NaOH solution using phenolphthalein as indicator. NaOH was taken in the burette and HCl was taken in a conical flask for the titrations The actual molarity of the prepared NaOH solution was "0.220 mol dm"^(-3) . Which among the following could be the reason for the wrong value obtained in titration III?

Consider the following statements and arrange in the order of true/false as given in the codes. S_1 :Ammonia on heating with concentrated solution of sodium hypochlorite gives nitrogen gas. S_2 :The phosphine gas dissolves in water in presence of sunlight and produces phosphonium hydroxide like ammonium hydroxide. S_3 :Barium azide on heating gives pure nitrogen gas. S_4 :The oxo-acids of phosphorus in which phosphorus has lower oxidation state less than +5 contain either P-P or P-H bonds but not both in addition to P=O and P-OH bonds.

40 mL 0.05 M solution of sodium sesquicarbonate dehydrate (Na_(2)CO_(3).NaHCO_(3).2H_(2)O) is titrated against 0.05 M HCl solution, x mL of acid is required to reach the phenolphthalein end point while mL of same acid were required when methyl organe indicator was used in a separate titration. Which of the following is (are) correct statements? a. y-x = 80 mL b. y+x = 160 mL c. If the titration is started with phenolphthalein indicator and methyl orange is added at the end point, 2 x mL of HCl would be required further to reach the end point d. If the same volume of same solution is titrated against 0.10 M NaOH, x//2 mL of base would be required

(a). IF both (A) and (R) are correct and (R) is the correct explanation of (A). (b). If both (A) and (R) are correct but (R) is not the correct explanation of (A). (c). If (A) is correct, but (R) is incorrect. (d). If (A) is incorrect, but (R) is correct. (e) if both (A) and (R) are incorrect. Assertion (A): In the titration of Na_(2)CO_(3) with HCl using methyl orange indicator the volume required at the equivalence point is twice that of the acid required using phenolphthalein indicator. Reason (R): 2 " mol of "HCl are required for complete neutralization of one mole of Na_(2)CO_(3) .