Molar mass of sodium formate
HCOONa = 1.0079 + 12.01 + ( 2 16.00 ) + 22.99 = 68.01 g/mol
We know that, No. of moles = Mass / Molar mass
No. of moles of HCOONa = 25.0 g / 68.01 g/ mol = 0.3676 mol
Volume of solution = 400.0 ml = 0.4000 L
[HCOONa] = No. of moles of HCOONa / volume of solution in L
= 0.3676 mol / 0.4000 L
= 0.919 M
pH of buffer solution is calculated by using Henderson's equation.
pH = pKa + log [Salt] / [Acid]
pH = 3.744 + log [HCOONa] / [HCOOH]
pH = 3.744 + log 0.919 / 0.64
pH = 3.744 + 0.157
pH = 3.901
PART 2
pH of pure water.
Consider auto ionization of water, 2 H2O H3O + + OH -
For above reaction, equilibrium constant is K w = [ H3O +] [OH - ]
At 25 0 C , value of K w = 1 10 -14
K w = [ H3O +] [OH - ] = 1 10 -14
At equilibrium , [ H3O +] = [OH - ]
[ H3O +] [ H3O +] = 1 10 -14
[ H3O +] 2 = 1 10 -14
[ H3O +] = 1 10 -07 M
We have, pH = -log [ H3O +] = - log 1 10 -07 = 7.0
PART 3
When HCl is added to water , solution becomes dilute. pH will depend on concentration of diluted HCl solution.
We can use dilution formula to find out concentration of diluted solution.
We have formula, M Stock V stock = M dilute V dilute
M dilute = M Stock V stock / V dilute
Here volume of dilute solution = 100.0 + 22.2 = 122.2 ml
Molarity of stock HCl solution = 0.0020 M
Volume of stock HCl solution = 22.2 ml
M dilute = 0.0020 M 22.2 ml / 122.2 ml = 0.000363 M
We have, pH = - log [ H3O +] = - log 0.000363 = 3.44
ANSWER : pH = 3.44
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