Calculate the number of moles of hcl(g) that must be added to 1.0 l of 1.0 m nac2h3o2 to produce a solution buffered at each ph.

Missing question: 
(a) pH = pKa.
(b) pH = 3.84.
(c) pH = 5.26.
a) c(sodium acetate - NaC₂H₃O₂) = 1,0 M = 1,0 mol/L.
c(NaC₂H₃O₂) = 1,0 L.
Chemical reaction: CH₃COONa + HCl ⇄ CH₃COOH + NaCl.
Ka - acid dissociation constant.
pKa = -logKa.
When pH = pKa, n(CH₃COO⁻) = n(CH₃COOH).
From chemical reaction, half of sodium acetate reacts (0,5 mol), so n(HCl) = 0,5 mol.

b) Chemical reaction: CH₃COO⁻ + H⁺ ⇄ CH₃COOH.
Henderson–Hasselbalch equation: pH = pKa + log(cs/ck).
4,20 = 4,76 + log(cs/ck).
log(cs/ck) =4,20 - 4,76 = -0,54.
cs/ck = 10∧(-0,54) = 0,288.

(1 mol - x )/x = 0,288.

x = n(HCl) = 0,776 mol.

c) Chemical reaction: CH₃COO⁻ + H⁺ ⇄ CH₃COOH.

Henderson–Hasselbalch equation: pH = pKa + log(cs/ck).
5,26 = 4,76 + log(cs/ck).
log(cs/ck) = 5,26 - 4,76 = 0,50.
cs/ck = 10∧(0,50) = 3,16.

(1 mol - x )/x = 3,16.

x = n(HCl) = 0,240 mol.

pH is a numeric scale used to specify the acidity or basicity of an aqueous solution.

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.

the answer is option a.