Calculate the for the following conditions: a. pH = 3.21 b. pOH = 13.34 Calculat

Question

Calculate the for the following conditions: a. pH = 3.21 b. pOH = 13.34 Calculate the pH of the following solutions: Calculate the pH of the following buffer a. and A buffer is made from and a. What is the pH? b If you added moles of 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 350.0 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 pI

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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