Question

Determine the pH change when 0.050 mol HNO3 is added to 1.00 L of a buffer solution that is 0.464 M in HClO and 0.226 M in ClO-.

Answer #1

Given that volume of buffer = 1.0 L

molarity of ClO- = 0.226 M

molarity of HClO = 0.464 M

[ClO-] = molarity x volume = 0.226 M x 1.0 L = 0.226 mol

[HClO] = molarity x volume = 0.464 M x 1.0 L = 0.464 mol

[HNO3] = 0.05 mol

Original pH = pKa + log [ClO-]/ [HOCl] ----------(1)

pH after addition of HNO3:

ClO- + HNO3 ---------> HOCl + NO3-

Hence,

new pH = pKa + log {[ClO-] - [HNO3]/[HOCl] +[HNO3]} --------(2)

Since HNO3 is a strong caid, pH will be decreased compared to original pH.

To get change in pH, subtract (2) from (1).

Then,

change in pH = pKa + log [ClO-]/ [HOCl] - pKa + log {[ClO-] - [HNO3]/[HOCl]+[HNO3]}

= log [ClO-]/ [HOCl] - log {[ClO-] - [HNO3]/[HOCl]+[HNO3]}

= log [ 0.226/ 0.464] - log [ 0.226 - 0.05 ] / [ 0.464+0.05]

= 0.46

Therefore, change in pH = 0.46

Determine the pH change when 0.081 mol HI is added to 1.00 L of
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1. A buffer solution contains 0.476 M KH2PO4 and 0.202 M
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pH change = ______
2. Determine the pH change when
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pH after addition − pH before addition = pH
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buffer.
2) Determine the pH change when 0.070 mol HBR is added
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Please show work

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buffer.
pH after addition − pH before addition = pH change
=
2.)
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=

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Determine the pH change when
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Determine the pH change when 0.094 mol KOH is added to 1.00 L of
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