1.) What is the pH of a buffer solution that is 0.10 NH3 and 0.10 NH4+? What is the pH if 12mL of 0.20 M hydrochloric acid is added to 125 mL of buffer? For the first part, i figured that NH3 is the base and NH4+ is the conjugate acid. Therefore, the equil. reaction is NH3 + water --> NH4+ OH-. Using the given concentrations, i found Kb, pOH, and then Ph. For the second part, i'm unsure. I figured out the moles of NH3 and NH4+ by multiplying each molarity by 0.125 L. Then i did the same for H3O+ ion (formed by HCl) using 12mL as the volume. However, the problem appears as I'm unsure whether the addition of HCl will depleat the amount of NH4+ or NH3. Should i subtract the moles of the hydronium ion from the moles of NH3 and add it to NH4+? Or the other way around? 2.) A chloride salt (rantidinium chloride) is presnet in Zantac. Should a solution of rantidinium chloride be acidic, basic, or neutral? This is my logic: Since chloride ion forms an acidic solution with Hyrdogen (that is, its a conjugate base of a strong acid), then the solution should be acidic. But i need to consider rantidinium as well, and see whether that is an anion of a strong base, in which case the solution would be neutral. But how do i do that? 3.) I have to determine whether hydrolysis would occur with the following: a.) NO3- b.) OCl- c.) NH2NH3+ d.) Br- a.) Since NO3- is a conjugate base of a strong acid, no hydrolysis would occur. b.) Since OCl- is a conjugate base of a weak acid (HClO), hydrolysis does happen. c.) I have no idea! d.) Since HBr is a strong acid, no hydrolysis happens. My questions are: i.) Why does hydrolysis not happen when an ion is a conjugate acid/base of a strong acid/base? and ii.) Part C. Thank you.