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.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: