Calcuate the `pH` value of (assume `100%` ionization)
(i) `10^(-2)` molar `HNO_(3)` solution
(ii) `0.03M HCl` solution `(log 3=0.4771)`
(iii) `0.0005 M H_(2)SO_(4)` solution

The pH of a 0.005 M H_(2)SO_(4) solution is

Find the pH of (a) 10^(-3)M HNO_(3) solution (b) 10^(-4)MH_(2)SO_(4) solution (Take log2=0.3 )

Calculate molarity of all the ions produces by following aq. Solution of electrolytes. (Assuming 100% dissociation) (i) 0.2 M NaCl solution (ii) 1.2 M Al_(2)(SO_(4)) solution (iii) 1.2 M H_(2)SO_(4) solution (vi) 2.1 M MgCl_(2) solution

Calculate pH values of (i) 0.2 M H_(2)SO_(4) solution (ii) 0.2M Ca(OH)_(2) solution.

What is the normality of 0.3 M H_(3)PO_(4) solution ?

Whenever an acid is neutralised by a base, the net reaction is : H^(+)(aq) + OH^(-)(aq) to H_(2)O(l) + 57.1 kJ Calculate the heat evolved for the following experiments : (i) 0.25 mol of HCI solution is neutralised by 0.25 mol of NaOH solution. (ii) 0.60 mol of HNO_(3) solution is mixed with 0.30 mol of KOH solution. (iii) 100 cm^(3) of 0.2 M HCl is mixed with 200 cm^(3) of 0.3M NaOH. 400 cm^(3) of 0.2 M H_(2)SO_(4) is mixed with 600 cm^(3) of 0.1 M NaOH solution.

Calculate the pH for (i) 0.001 M HCl (ii) 0.0001 M H_(2) SO_(4) (iii) 10^(-2) Ca(OH)_(2) , (iv) 10^(2) M HCl

how should a student prepare 100mL of a 1.0 M H_(2)SO_(4) solution from a 10M H_(2)SO_(4) solution?