Question

Calculate the pH of a solution made by adding 25.0 g of sodium formate, NaHCOO, to 400 ml of 0.64 M formic acid, нсоон. Answe
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Answer #1

Molar mass of sodium formate

HCOONa = 1.0079 + 12.01 + ( 2 \times 16.00 ) + 22.99 = 68.01 g/mol

We know that, No. of moles = Mass / Molar mass

\therefore 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 \rightleftharpoons H3O + + OH -

For above reaction, equilibrium constant is K w = [ H3O +] [OH - ]

At 25 0 C , value of K w = 1 \times 10 -14

\therefore K w = [ H3O +] [OH - ] = 1 \times 10 -14

At equilibrium , [ H3O +] = [OH - ]

\therefore [ H3O +] [ H3O +] = 1 \times 10 -14

[ H3O +] 2 = 1 \times 10 -14

[ H3O +] = 1 \times 10 -07 M

We have, pH = -log [ H3O +] = - log  1 \times 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 \times V stock = M dilute \times V dilute

M dilute = M Stock \times 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

\therefore M dilute = 0.0020 M \times 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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