You are given sodium acetate, 1M HCl, NaHCO3 and Na2CO3. Determine which of these four you would need and then show calculations to make buffer pH = 4.7 by method 2. Assume making 100 mls of a 0.1 M buffer.

Neutralization of a portion of the weak base with sufficient strong acid to give the desired ratio, [A- ]/[HA]: Na+ + A- + HCl → HA + Na+ + Cl-

I've been having a lot of trouble going step by step with this one. If you could really explain the logic behind each step it would be very much appreciated!! I'm also confused about the ka value. Am I just supposed to look that up? Thank you so much for your time!

Amines are good nucleophiles, even though they are neutral molecules. how would the rate of an sn2 reaction between an amine and an alkyl halide be affected if the polarity of the solvent is increased? amines are good nucleophiles, even though they are neutral molecules. how would the rate of an reaction between an amine and an alkyl halide be affected if the polarity of the solvent is increased? because both reactants in the rate-limiting step are neutral, the reaction will be faster if the polarity of the solvent is increased. because both reactants in the rate-limiting step are neutral, the reaction will be slower if the polarity of the solvent is increased. because both reactants in the rate-limiting step are neutral, the reaction will occur at the same rate if the polarity of the solvent is increased. request answer