To learn how to calculate ion concentrations in an aqueous solution of a strong

Question

To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Sulfuric acid, H2SO4 , is a strong acid. Its complete dissociation in aqueous solution is represented as H2SO4 rightarrow H+ HSO4- A HSO4- anion can dissociate further by HSO4- H+ + SO42- but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as Calculate the concentration of HSO4- ions in a 0.010 M aqueous solution of sulfuric acid. Express your answer to two significant figures and include the appropriate units. Ammonia, NH3, is a weak base with a Kb value of 1.8 times 10-5. What is the percent ionization of ammonia at this concentration? Express your answer with the appropriate units. Use the simulation to test the pH of a 0.1 M solution of methylamine, NH2(CH3), dimethylamine, NH(CH3)2, and trimethylamine, N(CH3)3. Given the trend in pH for this series, rank the bases in the set below. Rank from strongest to weakest base. To rank items as equivalent, overlap them. Use the data in the simulation to find the Ka value of HOAc, acetic acid Express your answer to two significant figures.

Explanation / Answer

4*.01^3/x=.012

x=3.33*10^-4 M HSO4-

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