38. (a) How many grams of NaOAc must be added to 300 ml 0.01 M HOAC to produce a buffer of pH 6.50? (b) 2.00 mM NAOH is added to the buffer above. What is the pH after the addition of the base? (c) What would happen to the buffer if 2.00 mM NAOH additional were introduced? Ans. (a) 14 g.; (b) 7; (c) pH becomes 11.53.

Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 64.2 mL of 0.368 M hypochlorous acid 3.5x10-8) by 0.368 M NaOH at the following points. (Ka (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 96.3 mL of NaOH

6. ( ) A 40 mL sample of a 0.2 M RNHz (kb = 3.7 x 10") is titrated with 0.2 M HC (eg). Calculate the pH after the addition of each of the following volume acids. a) Initial pH (b) Volume of HCI (ag): 20 mL (c) Volume of HCI (ag): 39.9 mL (d) Volume of HCI (ag): 40.0 mL (e) Volume of HCI (ag): 40.1 mL

A 50.0 mL sample of 0.150 M acetic acid, HC2H3O2, is titrated with 0.150 M NaOH solution.  Calculate the pH after the following volumes of base have been added:  (a) 0 mL;  (b) 25 mL;  (c) 49 mL;  (d) 50.0 mL;  (e) 75.0 mL.

What mass of the salt, N a A would you have to added to 0.15 M H A (weak acid) with a volume of 107 mL to make a buffer with a pH of 4.87? The K a of H A is 6.87E-5. Assume there is no change in volume. The molecular weight of Na A is 131.96 g/mol.

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A 76.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M RbOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.1 mL pH = (d) 39.9 mL pH = (b) 37.2 mL pH = (e) 69.5 mL pH = (c) 38.0 mL pH =

2. Suppose 1.44 0.150 M benzoic acid solution. Calculate the pH of the resulting buffer solution as- suming the volume of the solution does not change on addition of the solid. of sodium benzoate, Na+C,H3COO-, is added to 100.0 mL of the

1000 mL of a buffer solution contains 0.275 moles of HCN, and 0.175 moles of NaCN. Ka of HCN = 6.2 x 10^-10.a) calculate the initial pH b) calculate the pH of the buffer after the addition of 27.5 L of 1.0 M of HCl. c) what is the change in pH of the solution if the same amount of Hcl which was used in part (b) were added to 1000 mL pure water.

5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www