Chemistry (acid-base): please help, thanks so much. pKa of NH3 =4.75, Kb of NH3

Question

Chemistry (acid-base): please help, thanks so much.

pKa of NH3 =4.75, Kb of NH3 = 1.78x10^-5, Ka of NH3 = 5.62x10^-10

Ka of HF = 6.6x10^-4, Kb of HF=1.52x10^-11

what is the final pH of a solution that has a 0.123 M of NH4F?(hint: what happens to H+ and OH- when mixed?)

will NaCN increase or decrease in solubility with a lowering pH?

You are in a lab doing experiments with an acid H2A. you titrate the acid with a strong base until first stoichiometric/ equivalence point. Determine if the substance is acting like a base of acid and determine the pH.

In an ideal buffer, the relationship between the weak acid (HA) and its conjugate base (A-) is

HA = A- b) HA < A- c)none of these

You make a 0.0123 M solution of an unknown base. You get a pH of 10.75. What is the pKa of the substance? And Why?

Hydrochloric acid at 0.1 M has a pH of 1. Acetic acid has a pH of 2.88 at the same molarity. Explain why? (saying one is strong and the other weak is not an answer)

You have a 1L solution of 0.123 M benzoic acid, a weak monoprotic acid. You also have NaOH and HCl available. How many moles of which chemical do you have to add to the benzoic acid if you want to make a buffer with a pH of 4.2? (assume no volume changes)

Explanation / Answer

Hydrochloric acid is a strong acid so low PH value, acetic acid is a weak acid so it has more PH value compare to HCl.strong acids have less PH value, weak acids have more PH value.

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