Home
Class 12
CHEMISTRY
The average concentration of SO(2) in th...

The average concentration of `SO_(2)` in the atmosphere over a city on a certain day is `10 ppm`, when the average temperature is `298 K`. Given that the solubility of `SO_(2)` in water at `298k`. Given that the solubility of `SO_(2)` in water at `298K` is `1.3653mol L^(-1)` and `pK_(a)` of `H_(2)SO_(3)` is `1.92`. Estimate the `pH` of rain on that day.

Text Solution

Verified by Experts

The correct Answer is:
4.86
Promotional Banner

Similar Questions

Explore conceptually related problems

The average concentration of SO_(2) in the atmosphere over a city on a cetrain day is 10 ppm, when the average temperature is 298 K. Given that the solubility of SO_(2) in water at 298 K is 1.3653 mol litre^(-1) and the pK_(a) of H_(2)SO_(3) is 1.92 , estimate the pH of rain on that day.

The solubility product of PbCl_(2) at 298K is 1.7 xx 10^(-5) . Calculate the solubility of PbCl_(2) in g L^(-1) at 298K

Which of the following graphs is correct for solubility of O_2 and N_2 in water at 298K.

The solubility product of PbCl_2 at 298 K is 7.1 xx 10 ^(-5) Calculate the solubility of PbCl_2 " in " g L^(-1) at 298 K.

Solubility of CdSO_(4) is 1 xx 10^(-4) mol per litre. What is the solubility of CdSO_(4) in decinormal H_(2)SO_(4) solution?

The solubility of Sb_(2)S_(3) in water is 1.0 xx 10^(-5) mol/letre at 298K. What will be its solubility product ?

The solubility of CaF_2 in water at 298 K is 1.7 xx 10 ^(-3) grams per 100 cm ^(3) .Calculate the solubility product of CaF_2 at 298 K.

The Henry's law constant for CO_(2) in water at 298 K is 1.67 kbar. Calculate the solubility of CO_(2) at 298 K when the pressure of CO_(2) is one bar.

Determine the solubility of silver chromate at 298 K given its K_(sp) value is 1.1xx10^(-12) ?

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be