Kat asked in Science & MathematicsChemistry · 2 months ago

Calculate the pH of the solute in an aqueous solution of 0.663 M NH3(aq) if the Kb is 1.8 × 10−5 .?

additionally What is the percentage protonation of the

solute?

Answer in units of %

2 Answers

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  • Bobby
    Lv 7
    2 months ago

    NH3+ H2O = NH4+ + OH- 

    [OH-] = SQRT(1.8 × 10−5 * 0.663) = 3.45E-03

    pOH = 2.462 pH = 14-pOH = 11.5

    % protonation = [NH4+] / [NH3] % = 3.45 *10 ^-3 / 0.663 %  = 0.52 % 

  • Anonymous
    2 months ago

    personal finance is not the place for lazy dishonest cheaters to beg strangers to do their homework. You seem to have a problem with doing your own homework.  Even moving it to the correct category does not mean others doing your homework is right. Its not. Unless you explain to your teacher that you did not do it, some stranger from YA did it.

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