200mL of 0.5M aqueous and acidified solution of `KMnO_(4)` oxidises 8.8g" of a metal ion from `M^(2+)` to `M^(5+)` ion. What is the molar mass of the metal ion in `g mol ^(-1)` unit?

200 ml of water is added of 500 ml of 0.2 M solution. What is the molarity of this diluted solution?

20 ml of 0.02 M KMnO_4 was required to completely oxidise 10 ml of oxalic acid solution. What is the molarity of the oxalic acid solution ?

The amount of oxalic acid required to prepare 300 mL of 2.5 M solution is : (molar mass of oxalic acid = 90 g mol^(–1) ) :

1 mole of OH^(-) ions is obtained from 85 g of hydroxide of a metal. What is the equivalent weight of the metal ?

The diameter of a metallic ball is 4.2 cm. What is the mass of the ball, if the density of the metal is 8. 9\ g\ p e r\ c m^3 ?

In an experiment, 4g of M_(2)O_(x) oxide was reduced to 2.8g of the metal. If the atomic mass of the metal is 56g"mol"^(-1) , the number of oxygen atoms in the oxide is:

The density of 5% aqueous MgCl_(2) solution is 1.043 g mL^(-1) . What is the molarity and molaltiy of the solution? What is the molality of Cl^(ɵ) ions? (Mg = 24 "amu")

100 " mL of " x M KMnO_(4) is requried oxidise 200 " mL of " 0.2 M ferric oxalate in acidic medium what is the normality of KMnO_(4) ?

A 15mL sample of 0.20 M" " MgCl_(2) is added to 45ML of 0.40 M AlCl_(3) What is the molarity of Cl ions in the final solution

A quantity of 25.0 mL of solution containing both Fe^(2+) and Fe^(3+) ions is titrated with 25.0 mL of 0.0200 M KMnO_(4) (in dilute H_(2)SO_(4) ). As a result, all of the Fe^(2+) ions are oxidised to Fe^(3+) ions. Next 25 mL of the original solution is treated with Zn metal finally, the solution requires 40.0 mL of the same KMnO_(4) solution for oxidation to Fe^(3+) . MnO_(4)^(-)+5Fe^(2+)+8H^(+)toMn^(2+)+5Fe^(3+)+4H_(2)O Zinc aded in the second titration wil