Chemistry pH problem help NaOH and HCl

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The discussion focuses on calculating the pH of a neutralization reaction between 0.32M HCl and 0.16M NaOH. Participants are tasked with determining the pH after adding varying volumes of HCl to 25 mL of NaOH. Key calculations involve identifying the moles of NaOH and HCl present, determining which reactant is in excess, and applying the relationship 14 = pH + pOH to find the resulting pH values for different scenarios. The correct approach requires converting volumes to moles and understanding the neutralization process.

PREREQUISITES
  • Understanding of acid-base neutralization reactions
  • Knowledge of molarity and volume conversions
  • Familiarity with pH and pOH calculations
  • Basic chemistry concepts related to moles and concentrations
NEXT STEPS
  • Learn how to calculate pH for strong acid-strong base reactions
  • Study the concept of limiting reactants in chemical reactions
  • Explore the Henderson-Hasselbalch equation for buffer solutions
  • Investigate the effects of dilution on pH in titration scenarios
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Chemistry students, educators, and anyone involved in laboratory work related to acid-base reactions and pH calculations.

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Chemistry pH problem help please NaOH and HCl

Calculate the pH after the following total volumes of .32M HCl have been added to 25 mL of 0.16M NaOH
a. 0 mL c. 12.4 mL e. 12.6 mL
b. 1 mL d. 12.5 mL f. 15.0 mL



A. i have answered correctly but i can't seem to get the right answer for any of the others i tried putting them in mmol but it never seems to work if someone could just tell me how to do b through f i would be very pleased thank you.
 
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The exercise is a neutralization reaction. Determine which moles of NaOH or HCl is in excess. That would be the one which affects the pH. A relationship which is helpful is 14 = pH + pOH
 

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