Question- A 1.00L buffer solution is 0.250M HF and 0.250M LiF. Calculate the pH of this solution after addition of 0.150 moles of solid LiOH. Ka HF=3.5x10^-4.
A solution contains 0.021M Cl- and 0.017M I-. A solution containing Cu(I) ions is added to selectively precipitate on eof the ions. At what [Cu(I)] will a precipitate begin to form, and what is its identity? Ksp CuCl=1.0x10^-6, IKsp CuI=5.1x10^-12
Can you thoroughly explain the process of your answer, like what is the conjugate base and weak acid or work out an ICE table etc etc.
Solve the above questions explain each and every step in detail