Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.550 g...
Calculate the pH of the following buffer solutions:
(a) a solution made by dissolving 4.550 g KH2PO4 and 1.871 g K2HPO4 in water to give 350. mL of solution.
(b) a solution made by mixing 35.00 mL 0.35 M N2H4 with 15.00 mL 0.21 M N2H5Cl.
The base dissociation constant Kb is 8.50 x 10-7 for N2H4 . Assume that the final volume is the sum of the volunes of the two solutions that are mixed.
Homework Answers
First calculate molarity of both KH2PO4 and
K2HPO4 and then molarity equation M1V1+M2V2=M(V1+V2) and calculate
pH.
From formula M(V1+V2)=M1V1+M2V2, calculate
M, then pH.
Add Answer to:
Calculate the pH of the following buffer solutions:
(a) a solution made by dissolving 4.550 g...
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what is the pH of a buffet solution that is made by dissolving
16.6 g of KClO in 495 mL of .355 M HClO? (total volune is 495
mL)
1. What is the pH of a buffer solution that is made by dissolving 16.6 g of KCIO in 495 mL of 0.355 M HCIO? (You can assume the total volume is 495 mL).
4) A buffer solution is prepared by dissolving 5.40 g of ammonium chloride in 20.0 mL of water a mixing it with 35.0 mL of 10.0 Mammonia. Ky for ammonia is 1.8x10° a) What is the pH of this buffer solution b) This buffer solution is diluted with water to volume of 100.0 mL and 5.00 mL of 0.500 M HCl are added to the 100.0 mL of buffer. What is the expected pH of the buffer solution after the...
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