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1) A 1.00 m aqueous solution of the following compounds were produced. Which compound would you expect to produce a solution with the lowest melting point. Assume each compound fully dissolves. a) KClO3 b) MgCl2 c) NaF d) NaCl e) MgSO4
2) A 100 mL solution of 0.5 M NaOH is added to 100 mL solution of 0.5 M H2SO4. Determine the pH of the solution. (pKa1 < 0, pKa2 = 1.96). State any necessary assumptions.
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Indicate the pH at (a) the beginning of the titration (0.0 mL titrant) and after the addition of (b) 12.5 mL, (c) 24.0 mL, (d) 24.9 mL, (e) 25.0 mL, (f) 25.1 mL, and (g) 30.0 mL of the titrant. Label the half-neutralization point and the equivalen..
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carbonic acid solution with [H_2CO_3] = 0.00735 M is titrated with 0.100 M KOH. Determine the pH of the solution when 70.00mL of OH have been added.
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