According to Henderson-Hasselbulch equation:
pH = pKa + Log(nNaF/nHF)
i.e. 3 = -Log(7.2*10-4) + Log{(w/42)/0.3}
i.e. 3 = 3.14 + Log(w/12.6)
i.e. Log(12.6/w) = 0.14
i.e. 12.6/w = 1.38
Therefore, the mass of NaF needed = 12.6/1.38 = 9.128 g
Consider a solution initially containing 0.300 mol of hydrogen fluoride (HF). How many grams of Naf (42.0 /mo vould...
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