Converting the molarities into moles but I'm having trouble with the reaction

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SUMMARY

The discussion focuses on calculating the pH resulting from the reaction between 45.0 mL of 0.250 M NaOH and 35.0 mL of 0.200 M HCl. The reaction produces sodium chloride (NaCl) and water, and participants emphasize the importance of determining the limiting reagent to find the remaining concentration of H+ ions. The final pH can be calculated directly from the leftover H+ or by first determining the pOH if OH- ions remain after the reaction.

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  • Understanding of molarity and how to convert it to moles
  • Basic knowledge of acid-base reactions and neutralization
  • Familiarity with calculating pH and pOH
  • Concept of limiting reagents in chemical reactions
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  • Learn how to calculate moles from molarity and volume
  • Study the principles of acid-base neutralization reactions
  • Explore the relationship between pH, pOH, and ion concentrations
  • Investigate how to identify limiting reagents in chemical equations
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Chemistry students, educators, and anyone involved in chemical calculations or acid-base chemistry will benefit from this discussion.

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Can anyone help me with this problem?


Find the pH when 45.0 mL of 0.250 M NaOH(aq) is added to 35.0 mL of 0.200 M HCl(aq).

I started by converting the molarities into moles but I'm having trouble with what the reaction should look like. Shouldn't it produce a salt (NaCl) and water? And if so, how would I calculate the [H+] and then ph from that?
 
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shaggyace said:
Shouldn't it produce a salt (NaCl) and water?

Yes. If you've already converted to moles and you now know that the products are salt and water, you can now determine your limiting reagent and figure out how much H+ you have left over. With that and the total volume, you can determine the pH.
 


Alternatively, you may have to calculate pOH first, if there is OH- left.
 

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