Predict the relative acidic strength among the following H2O, H2S, H2Se, H2Te
H2O < H2S < H2Se < H2Te
Assume that each has lost a proton. So we get: HO–, HS–, HSe–, HTe–
It can be easily seen that the volume available for the negative charge is increasing from HO– to HTe–, therefore
(i) Volume available for the negative charge is increasing from left to right
(ii) Charge density is decreasing from left to right
(iii) Basicity is decreasing from left to right
(iv) Acidity of conjugate acids is increasing from left to right
H2O < H2S < H2Se < H2Te.
1 mol each of H3PO2, H3PO3 and H3PO4 will neutralise x mol of NaOH, ymol of Ca(OH)2 and z mol of Al(OH)3 (assuming all as strong electrolytes). x, y, z are in the ratio of:
Which of the following hydride is the most reducing?
Which of the following has the highest bond length?
Which of the following has correct increasing order of hydrolysis?
Pyrophosphoric acid is a
Peroxodisulphuric acid is a
Which of the following oxides is most acidic?
Predict the relative basicity of the following ions F–, Cl–, Br–, I–
Pb(NO3)2 on heating gives
The bonds present in N2O5 are: