Question
In: Chemistry
A buffer solution contains 0.350 M NaHSO3 and 0.387 M Na2SO3. Determine the pH change when...
A buffer solution contains 0.350 M NaHSO3 and 0.387 M Na2SO3. Determine the pH change when 0.104 mol HNO3 is added to 1.00 L of the buffer.
pH change =
This is all the info that was given
Solutions
Expert Solution
Calculation of initial pH of buffer solution.
We have Henderson's equation, pH = pKa + log [ Salt ]/ [ Acid]
pH = pKa + log [ Na2SO3 ] / [
NaHSO3 ]
pH = 7.172 + log 0.387 / 0.350
pH = 7.172 + 0.04364
pH = 7.2156
pH = 7.216
Calculation of pH of buffer solution after addition of HNO 3 .
Consider reaction of HNO 3 with buffer solution.
Na2SO3+ HNO 3
NaHSO3
+ NaNO 3
Let's use ICE table.
| M |
Na2SO3+ HNO 3 NaHSO3 |
||
| I | 0.387 | 0.104 | 0.350 |
| C | - 0.104 | -0.104 | +0.104 |
| E | 0.283 | 0.000 | 0.454 |
We have equation , pH = pKa + log [ Na2SO3 ] / [ NaHSO3 ]
pH = 7.172 + log ( 0.283 / 0. 454 )
pH = 7.172 - 0.2053
pH = 6.9667
pH =6.967
pH Change = pH of buffer solution after addition of nitric acid - initial pH of buffer solution.
pH change = 6.967 - 7.216
pH change = - 0.249
ANSWER : - 0.249
queen_honey_blossom answered 11 months agoRelated Solutions
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