3. There are 4 sets of solutions as given below. a. 20 mL 0.1 M acetic acid 20 mL 0.1 M HCl 20 mL 0.1 M NaOH b. 40 mL 0.1 M HCl 20 mL 0.1 M NaOH 60 mL 0.1 M sodium acetate c. 60 mL 0.1 M sodium acetate 20 mL HCl 20 mL 0.1 M acetic acid d. 40 mL 0.1 M NaOH 20 mL 0.1M acetic acid 40 mL 0.1M sodium acetate You are given 0.1M solutions of HCl, NaOH, acetic acid, sodium acetate Indicate if any of the solutions a-d given above is a buffer solutions, if not, how would you convert it into a buffer solution. You can add requisite amount of any one of the 0.1M solutions of HCl, NaOH, acetic acid or sodium acetate.

Which best describes why nh4+ can form an ionic bond with cl-?

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. the ionic radius for na+ is 102 pm and for cl– is 181 pm. in going from na to cl in period 3, why does the atomic radius decrease while the ionic radius increases? a. the inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do. b. the inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion. c. the outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. d. the outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. e. monatomic ions are bigger than the atoms from which they are formed.

Avariable that is not being directly tested during an experiment should be