PART A: 0.10 g of hydrogen chloride (HCl ) is dissolved in water to make 8.0 L of solution. What is the pH of the resulting hydrochloric acid solution?
PART B: 0.60 g of sodium hydroxide (NaOH ) pellets are dissolved in water to make 2.0 L of solution. What is the pH of this solution?
PART C: Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid.
PART D: A certain weak acid, HA , has a Ka value of 7.8×10−7. Calculate the percent ionization of HA in a 0.10 M solution.
PLEASE EXPLAIN YOUR STEPS and the logic behind if possible. Thank you!
Molar mass of HCl,
MM = 1*MM(H) + 1*MM(Cl)
= 1*1.008 + 1*35.5
= 36.5 g/mol
m(HCl)= 0.10 g
number of mol of HCl,
n = mass/molar mass
=(0.1 g)/(36.5 g/mol)
= 2.74*10^-3 mol
volume , V = 8.0 L
M = number of mol / volume in L
= 2.74*10^-3 mol /8 L
= 3.425*10^-4 M
[H+] = 3.425*10^-4 M
pH = -log [H+]
pH = -log (3.425*10^-4)
pH = 3.5
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