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  1. #1
    (φ⇒(ψ⇒φ)) CRyan64's Avatar
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    Chem help, will rep for any help i can get

    1. If the Kb of a weak base is 7.6x10^-6, what is the pH of a 0.25M solution of this base?

    2. The Ka of a monoprotic weak acid is 3.8x10^-3. What percent ionization of a 0.161 M solution of this acid?

    3. Enough of a monoprotic acid is dissolved in water to produce a 0.0156 M solution. The pH of the resulting solution is 6.22. Calculate the Ka for the acid.

    4. Enough of a monoprotic acid is dissolved in water to produce a 0.0134 M solution. The pH of the resulting solution is 2.63. Calculate the Ka for the acid.

    5. A certain weak base has a Kb of 8.60 × 10-7. What concentration of this base will produce a pH of 10.34?

    6. Using chemical equations, show how the triprotic acid H3PO4 ionizes in water. Phases, such as (l) or (aq), are optional.

    7. For the diprotic weak acid H2A, Ka1 = 3.0 × 10-5 and Ka2 = 5.4 × 10-7. What is the pH of a 0.0450 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
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  2. #2
    Registered User Brandon914's Avatar
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    ph= [h+][oh-] 1x10^-7+1x10^-7=1X10^-14 those formulas should answer most of those.
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  3. #3
    (φ⇒(ψ⇒φ)) CRyan64's Avatar
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    bump for halp
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  4. #4
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    Damn I used to know this stuff.
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  5. #5
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    6.
    H3PO4 is in equilibrium with H2PO4− + H+
    H2PO4− is in equilibrium with HPO42− + H+
    HPO42− is in equilibrium with PO43− + H+
    I doesn't afraid of anything...
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  6. #6
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    pH= -log Molarity
    Ka = M^-pH



    alter the equation from there to get pOH or Ka etc
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