Arrange the following compounds/ions in order of increasing pH, and please explain why? I am trying to understand and would love an explanation. Thanks alot.
Arrange the following compounds/ions in order of increasing pH, and please explain why? I am trying...
Arrange the group of compounds and ions/ in order of increasing pH? 1) NH4Cl, H2SO4, NaOH,Na2CO3 2)H2Se,HI,H2S,NH3 3) HCLO, HClO3,CLO^-, HBrO 4) K2SO3, Ca(OH)2, HCL,HF 5) NH3, H3O+, OH^-, HF
Arrange the following ions in order of increasing leaving group ability and nucleophilicity. Please explain your answer.
5) Arrange the following ions in order of increasing nucleophilicity and leaving group ability. Please explain your answer by discussing the influence of the resonance and inductive effects
please solve and show work! The correct order of increasing (lowest to highest) pH for the following 0.1M solution is: 1. HI 2. HF 3. NaF 4. Nal A. 2 1 3 4 B. 1 2 3 4 C.2 1 4 3 D.1 2. 4 3 E. 3 4 2 1 Reset Sel
Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO, HCl, HCN, NaOH, NH3, NaCN, KNO3, H2SO4, NH4Cl, H2SO3, NaHCO3, Na3PO4 and CH3COOH. please list each solution in order and next to it be specific next to each in terms of why each solution was placed in its respective position - please include ka and kb values in your explanation while ranking the solutions and add in any...
Why wouldnt a weak base, such as NH3, work just as well as KOH in (1)? 2.2 Is the question I have. I figured out 2.1 already. Below is relevant info. Thanks! 2. (1) Describe how adding a solution of KOH to the original sulfide precipitate results in the separa- tion of Sn4+ ion from the other Group W cations. (2) Why wouldn't a weak base, such as aque- ous NH3, work just as well as aqueous KOH in (1)?...