Concentrated nitric acid used in the laboratory work is 68% nitric acid by mass in aqueous solution. What should be molarity of such sample of the acid if the density of solution is 1.504 g `mL^-1` ?

A monotropic acid in 1.00 M solution is 0.01% ionised. What is the dissociation constant of the acid ?

What is the action of concentrated nitric acid on copper? Give equation.

Formic acid is 4.6% dissociated in a 0.1 N solution at 20^@C . The ionisation constant of formic acid is :

A solution of protein (extracted from crabs) was prepared by dissolving 0.75 g in 125 cm^3 of an aqueous solution. At 4^@C an osmotic pressure rise of 2.6 mm of the solution was observed. Then molecular weight of protein is (Assume density of solution is 1.00 g/cm^3 ):

0.1 M acetic acid solution is titrated against 0.1M NaOH solution. What would be the difference in Ph between 1/4 and 3/4 stages of neutralisation of acid :

A 0.2 molal aqueous solution of a weak acid (HX) is 20 percent ionised. The freezing point of this solution is: ( K_f = 1.86 K/m for water)