Consider a buffer solution that contains 0.25 M
C6H4(CO2H)(CO2K) and
0.15 M C6H4(CO2K)2.
pKa(C6H4(CO2H)CO2-)=5.41.
1. Calculate its pH
2. Calculate...
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Chemistry
Consider a buffer solution that contains 0.25 MC6H4(CO2H)(CO2K) and0.15 M C6H4(CO2K)2.pKa(C6H4(CO2H)CO2-)=5.41.
1. Calculate its pH
2. Calculate the change in pH if 0.140 g of solid NaOH is addedto 190 mL of this solution.
3. If the acceptable buffer range of the solution is ±0.10 pHunits, calculate how many moles of H3O+ canbe neutralized by 250 mL of the initial buffer.
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4.2 Ratings (609 Votes)
1 The pH is calculated using the henderson hasselbach equation pH pKa log Salt Acid 541 log 015 025 519 2 The moles of salt acid and NaOH added are calculated n Salt M V 015 019 00285 mol n Acid 025
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