Yesterday’s Homework Page 611 # 19 Page 612 # 20.

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Presentation transcript:

Yesterday’s Homework Page 611 # 19 Page 612 # 20

Calculate the pH of solutions having the following ion concentrations at 298 o K. [H + ] = 1.0 x log [H + ] = -2 pH = 2

Calculate the pH of solutions having the following ion concentrations at 298 o K. [H + ] = 3.0 x log [H + ] = – 6 = pH = 5.523

Calculate the pH of solutions having the following ion concentrations at 298 o K. [OH - ] = 8.2 x log [OH - ] = – 6 = pOH = 5.087

Calculate the pH of solutions having the following ion concentrations at 298 o K. pOH = pH + pOH = 14 pH = 14 – pOH = 14 – = 8.913

Calculate the pH of solutions having the following ion concentrations at 298 o K. [OH - ] = 1.0 x log [OH - ] = -6 pOH = 6 pH = 14 – 6 = 8

Calculate the pH of solutions having the following ion concentrations at 298 o K. [OH - ] = 6.5 x log [OH - ] = pOH = pH = 14 – =

Calculate the pH of solutions having the following ion concentrations at 298 o K. [H + ] = 3.6 x log [H + ] = pH = pOH = 14 – = 5.556

[H + ] =.025 Calculate the pH of solutions having the following ion concentrations at 298 o K.

[H + ] = 2.5 x log [H + ] = – 2 pH = pOH = 14 – = Calculate the pH of solutions having the following ion concentrations at 298 o K.

Now let’s try it the other way around…

Given the pH, calculate the [H + ] and [OH - ] for the following solution. pH = log [H + ] = 7.40 log [H + ] = =.60 – 8 [H + ] = 4.0 x 10 -8

Given the pH, calculate the [H + ] and [OH - ] for the following solution. pOH = 14 – 7.40 = 6.60 log [OH - ] = =.40 – 7 [OH - ] = 2.5 x 10 -7

One last thing… If you have a solution of 1.0 M HCl, what is the [H + ]?

One last thing… HCl is a strong acid. That means it dissociates completely. If [HCl] = 1.0, then [H+] = 1.0

One last thing… Same with strong bases. If [NaOH] = 1.0, then [OH - ] = 1.0

Homework Page 614 Problems 21 & 22