When `2.5g` of a sample of mohr's salt reacts completely with `50mL` of `N/10 KMnO_4` solution. The % purity of the sample of Mohr's salt is :

0.80g is impure (NH_4)SO_4) was boiled with 100mL of 0.2N NaOH solution till all the NH_3 (g) evolved. The remaining solution was diluted to 250mL. 25mL of this solution was neutralized using 5mL of 0.2 NH_2 SO_4 solution. The percentage purity of the (NH_4)_2SO_4 sample is :

How many gram equivalents of H2SO4 are present in 200 ml of N/10 H2SO4 solution ?

25mL of 2N HCI, 50 mL of 4N HNO_3 and x mL of 2MH_2 SO_4 are mixed together and the total volume is made up to 1L after dilution. 50mL of this acid mixture completely reacted with 25mL of a 1NNa_2 CO_3 solution. The value of x is :

A mixture of FeO and Fe_2 O_3 is completely reacted with 100mL of 0.25M acidified KMnO_4 solution. The resulting solution was then treated with Zn dust which converted Fe^(3+) of the solution to fe^(2+) . The Fe^(2=) required 100mL of 0.10MK_2 Cr_2O_7 solution. Find out the weight % Fe_2O_3 in the mixture.

4 mole of a mixture of Mohr's salt and Fe_2(SO_4)_3 requires 500mL of 1 M K_2Cr_2O_7 for complete oxidation in acidic medium. The mole % of the Mohr's salt in the mixture is :

40 g Ba(MnO_(4))_(2) (mol.mass=375) sample containing some inert impurities in acidic medium completely reacts with 125 mL of "33.6 V" of H_(2)O_(2) . What is the percentage purity of the sample ?

To a 10mL, 1M aqueous solution of Br_(2) , excess of NaOH is added so that all Br_(2) is disproportionated to Br^(-) and BrO_(3)^(-) . The resulting solution is free from Br^(-) , by extraction and excess of OH^(-) neutralised by acidifying the solution. The resulting solution is suffcient to react with 2 g of impure CaC_(2)O_(4) (M= 128g/mol) sample. The % purity of oxalate sample is :

The concentration of an oxalic acid solution is x mol litre^-1. 40mL of this solution reacts with 16mL of 0.05M acidified KMnO_4 . What is the pH of 'x' M oxalic acid solution ? (Assume that oxalic acid dissociates completely).)

A metal M forms the sulphate M_2(SO_4)_3. A0.596 gram sample of the sulphate reacts with excess BaCI_2 to given 1.220g BaSO_4 . What is the atomic mass of M? (Atomic mass : S=32, Ba=137.3 )

A sample containing HAsO_2 (mol. mass =180 ) and weighing 3.78g is dissolved and diluted to 250mL in a volumetric flask. A 50mL sample (aliquat) is withdrawn with a pipet and titrated with 35mL of 0.05 M solution of I_2 . Calculate the percentage HAsO_2 in the sample :