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

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To find the pH when 45.0 mL of 0.250 M NaOH is added to 35.0 mL of 0.200 M HCl, start by calculating the moles of each reactant. The reaction between NaOH and HCl produces NaCl and water. After determining the limiting reagent, assess the remaining H+ or OH- ions to find the concentration of the excess ion. This excess concentration, along with the total volume of the solution, allows for the calculation of pH. If there are leftover OH- ions, pOH can be calculated first, then converted to pH.
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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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