How Many Moles of HCl and HC3H5O3 to Achieve pH 3.77?

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SUMMARY

The discussion centers on calculating the moles of hydrochloric acid (HCl) and sodium hydrogen phosphate (HC3H5O3) required to achieve a pH of 3.77 in a 1L solution containing 0.1M sodium acetate (NaC3H5O3). The problem is identified as a buffer solution scenario, where the Henderson-Hasselbalch equation is applicable for determining the necessary concentrations of the acid and its conjugate base. Participants emphasize the importance of understanding buffer systems and the specific calculations involved in achieving the desired pH level.

PREREQUISITES
  • Understanding of buffer solutions and their components
  • Familiarity with the Henderson-Hasselbalch equation
  • Basic knowledge of molarity and pH calculations
  • Experience with acid-base titration concepts
NEXT STEPS
  • Study the Henderson-Hasselbalch equation in detail
  • Practice calculations involving buffer solutions and pH adjustments
  • Explore the properties and applications of common buffer systems
  • Learn about titration curves and their significance in acid-base chemistry
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Chemistry students, laboratory technicians, and anyone involved in acid-base chemistry or buffer solution preparation will benefit from this discussion.

dragonlady90
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Hi again,
I have another question. A 1L sol'n of a compound, NaC3H5O3 has an initial con'c of 0.1M. An unknown number of moles of Hcl is then added to bring a final solution to a Ph of 3.77. How many moles of HCl were added and what is the common name of this type of problem?

Can anyone pls help me and reply soon plssssss.

I have one more question...

1.8g of NaOH(s) was dissolved in one litre of H2O. A compound, HC3H5O3 was added. The final pH of the solution was 3.77. How many moles of HC3H5O3 are needed?

Plsssssssssss help me.
 
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