How many grams (g) of formic acid (HCHO2) would you need to make a 555 mL solution with a pH of 2.25? Please show all steps
Let the concentration of HCO2H be c
use:
pH = -log [H+]
2.25 = -log [H+]
[H+] = 5.623*10^-3 M
HCO2H dissociates as:
HCO2H -----> H+ + HCO2-
c 0 0
c-x x x
Ka = [H+][HCO2-]/[HCO2H]
Ka = x*x/(c-x)
1.8*10^-4 = 5.623*10^-3*5.623*10^-3/(c-5.623*10^-3)
c-5.623*10^-3 = 0.1757
c=0.1813 M
volume , V = 555 mL
= 0.555 L
use:
number of mol,
n = Molarity * Volume
= 0.1813*0.555
= 0.1006 mol
Molar mass of CHO2H,
MM = 1*MM(C) + 2*MM(H) + 2*MM(O)
= 1*12.01 + 2*1.008 + 2*16.0
= 46.026 g/mol
use:
mass of CHO2H,
m = number of mol * molar mass
= 0.1006 mol * 46.03 g/mol
= 4.631 g
Answer: 4.63 g
How many grams (g) of formic acid (HCHO2) would you need to make a 555 mL...
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