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What is the pH of the solution that results from mixing the following four solutions together?

(1) 150. mL of 0.250 M NaCl
(2) 300. mL of 0.200 M HCl
(3) 100. mL of 0.050 M HNO3
(4) 450. mL of 0.200 M NaOAc

any help is greatly appreciated!

  • chemistry -

    I would determine the molarity of each component.
    moles NaCl = M x L
    moles HCl = M x L.
    moles HNO3 = M x L.
    moles NaOAc = M x L.
    Then M = moles/L.
    for NaCl that will be 0.0375/1 L = ??
    Likewise for the others.
    Finally, add the two H^+ from HCl and HNO3 to obtain total H^+.
    Then H^+ + OAc^- ==> HOAc
    You know H^+, you know OAc^-, that makes HOAc and leaves some Ac^- un-reacted. Then use Ka expression or the Henderson-Hasselbalch equation to solve for pH.

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