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    Calculating molar concentrations of acetic acid

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    1) Calculate the hydrogen ion concentration and the pH of the solution formed when 0.020 gram-formula weight of nitric acid is added to one liter of aqueous 0.20 M ammonia solution. Assume no significant volume change upon addition of the acid.
    2) Calculate the molar concentration of acetic acid at equilibrium in an acetic acid solution that is 1.1% ionized.
    3) Given a pure 0.50 M of HCN solution, calculate the volume that when diluted to a total volume of 70.0mL will yield a pH that is 0.65 unit higher than that of the given solution. Consider the volumes of the original solution and of the diluent to be precisely additive.
    4) Calculate the pH of 0.0013 M of NaCN.
    5) Calculate the pH of a solution which is 0.092 M in acetic acid and 0.092 M in sodium acetate.
    6) Calculate the pH of a mixture of 50mL of 0.10 M ammonium hydroxide and 51mL of 0.10 M of HCl.
    7) The solubility of ZnS is 3.5 x 10^-12 at 25 degrees Celsius. Calculate the value of K for ZnS at this temperature.
    8) Calculate the solubility of magnesium hydroxide at 25 degrees Celsius in (a) pure water and (b) a solution having a pH = 12.00. K for Mg(OH) is 8.9 x 10^-12 at this temperature. sp

    9) The value of the solubility product of lead chloride, PbCl ,is 1.6 x 10^-5 at 25 degrees Celsius.
    5.0 mL of 0.02 M Pb(NO ) is mixed with 25 mL of 0.01M of HCl. Does PbCl precipitate?

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    Solution Summary

    The expert has answered 9 chemistry questions in this solution in an attachment. Step by step solutions and explanations are provided for every question. 4 pages and 1135 words total (including questions).