Question

Predict the relative acidic strength among the following H2O, H2S, H2Se, H2Te

Solution

Correct option is

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.  

SIMILAR QUESTIONS

Q1

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). xy, z are in the ratio of:    

Q2

Which of the following hydride is the most reducing?

Q3

Which of the following has the highest bond length? 

Q4

Which of the following has correct increasing order of hydrolysis?

Q5

Pyrophosphoric acid is a

Q6

Peroxodisulphuric acid is a

Q7

Which of the following oxides is most acidic?

Q8

Predict the relative basicity of the following ions F, Cl, Br, I

Q9

Pb(NO3)2 on heating gives

Q10

The bonds present in N2O5 are: