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13 September, 04:45

What is the pH of a solution where 250 mL of 0.50 M NaOH is completely neutralized by 175mL of HCl? What are the final concentrations of all ions?

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  1. 13 September, 08:37
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    pH = 7.0

    Final concentration = 0.29 M

    Explanation:

    1. Find the mols of each reagent:

    NaOH:

    250 mL = 0.250 L

    0.50 M

    Molarity = mol NaOH / L solution

    0.50 M = mol NaOH / 0.250 L

    mol NaOH = 0.125 mol NaOH

    2. reaction between HCl and NaOH:

    NaOH + HCl = NaCl + H2O

    3. If the reaction in completly neutralized, it means that all NaOH mol reacted with HCl:

    0.125 mol NaOH = 0.125 mol HCl

    4. concentration of HCl solution:

    Molarity = mol HCl / L solution

    M = 0.125 mol HCl / 0.175 L = 0.71 M

    5. Neutralized means all reagent reacted. and pH has to be = 7.

    6. Concentration of ions:

    Cl-:

    0.125 mol HCl = 0.125 mol Cl -

    M = 0.125 mol Cl - / (0.250 L + 0.175 L) = 0.125 mol Cl-/0.425 L = 0.29 M

    Na +:

    0.125 mol Na+

    M = 0.125 mol Na + / 0.425 L = 0.29 M
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