Asked by Zekariyas
How many moles of NH4Cl must be added to 1.5L of 0.2 M solution of NH3 to form a buffer whose PH is 9.(Kb=1.8x10^-5)
Answers
Answered by
DrBob222
Use the Henderson-Hasselbalch equation.
pH = pKa + log[(base/(acid)]
You know pH, you can calculate pKa (convert Kb to pKb then pKa + pKb = pKw = 14), you know (NH3), solve for (acid; i.e., NH4Cl). Then M NH4Cl = mols/L. You know M and L, solve for mols. Then mols = grams/molar mass. You know mols and molar mass, solve for grams.
Post your work if you get stuck.
pH = pKa + log[(base/(acid)]
You know pH, you can calculate pKa (convert Kb to pKb then pKa + pKb = pKw = 14), you know (NH3), solve for (acid; i.e., NH4Cl). Then M NH4Cl = mols/L. You know M and L, solve for mols. Then mols = grams/molar mass. You know mols and molar mass, solve for grams.
Post your work if you get stuck.
Answered by
Anonymous
0.5r
Answered by
Anonymous
0.54
Answered by
Koket engida
0.36
Answered by
Koket engida
0.54
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