Calculate the [H_3O^+] for the following conditions a. pH = 3.21 b. pOH= 13.34 C

Question

Calculate the [H_3O^+] for the following conditions a. pH = 3.21 b. pOH= 13.34 Calculate the pH of the following solutions: a. 3.7 times 10^-3 M HCl b. 8.6 times 10^-2 M HC_2H_3O_2 K_a = 1.74 times 10^-5 Calculate the pH of the following buffer a. 7.8 times 10^-2 M HC_2H_3O_2 and 8.6 times 10^-2 M NaC_2H_3O_2 A buffer is made from 3.7 times 10^-1 M HC_2H_3O_2 and 2.9 times 10^-1 M NaC_2H_3O_2 a. What is the pH? B. If you added 3.0 times 10^-3 moles of NaOH to 0.100 L of buffer what is the final pH. (assume that any change in volume is negligible.) write out the full ionization equations for the following amino acids. a. Alanine b. serine How many grams of phenylalanine are needed to make 350.00 mL of a 0.125M solution? You titrate valine as we did in class today; dissolved it, acidified the solution with an excess of HCl, then titrated with NaOH until a pH of 13.5 was reached. Use the following information to determine; a. The molecular weight of valine b. Calculate the pl

Explanation / Answer

1) a) pH = -log[H3O+]= 3.21

Thus, [H3O+] = 10-3.21 = 6.2 x 10-4 M

b) pOH = 13.34

we know that, pH +pOH = 14

Thus, pH= 14 - 13.34 = 0.66

-log[H3O+]= 0.66

Thus, [H3O+] = 10-0.66 = 0.22 M

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