Isura

calculate the change in ph for 1l of buffer solution containing NH4OH and NH4Cl upon addition of 1) 0.02 moles of HCl 2) 0.02 moles of NaOH I got the initial pH as 9.2504 But now Im stuck cus I dunno what happens when we add HCl and NaOH? Please help! :)

Ksp of PbI2 at 25 degrees celcius and 15 degrees celcius is 7.5×10^-8 and 7.5×10^-9 respectively. (Pb=207 I=127) 1) write an expression for the equilibrium of PbI2 2)write an equation for the Ksp of PbI2 3)calculate the solubility of PbI2 at 25 degrees ce...

Actually I got the pH of initial solution containing NH4OH and NH4Cl. Question is to find the pH change when we add acid and a base respectively. So I know the initial one but dunno what to do after that...

And moles of NH4OH = 0.1 moles of NH4Cl = 0.1 My bad :( Thanks.

Oh that worked! Thank you so much sir! You literally saved me. Thanks again :)

.....PbI2 ==> Pb^2+ + 2I^- I...solid.....0........0 C...solid-x...x........2x E...solid-x...x........2x I put 2x considering stoichiometry. Am I wrong here? Thanks.