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A buffer solution is 0.392 M in HCN and 0.206 M in KCN. If K, for HCN is 4.0x1010, what is the pH of this buffer solution?
Calculate the pH of a buffer solution that is 0.250 M in HCN and 0.170 in KCN. For HCN, Ka= 4.9 x 10^-10 (pKa = 9.31). Use both the equilibrium approach and the Henderson-Hasselbalch approach.
Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.168 M in KCN. For HCN, Ka = 4.9 times 10^-10 (pKa = 9.31). PH =
Part A. Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.171 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.230 M in HC2H3O2 and 0.170 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid NaOH.
5. If a buffer solution contains 0.0100 mol of KCN and 0.0100 mol HCN at pH = 8.50, what is the new pH after the addition of 5.00 x 10 mol HCI? The K for HCN is 6.2 x 10-10.
Given that Ka for HCN is 6.2*10^-10, calculate the pH of a 0.15 M KCN solution.
6) Calculate the pH of a 0.021 M NaCN solution. [K (HCN) 4.9 x 1010] 6) a A) 5.49 B) 1.68 C) 3.18 D) 7.00 E) 10.82
!!!!!!!!!!!!!!! Ka HCN: 4.9 x 10^-10 !!!!!!!!!!!!!!!!!! 8. (10 points) Determine the pH of a 1.50 M Sodium Cyanide (KCN) solution. Be sure to show the 5% check.
What is the pH of a 0.500 M solution of HCN. The dissociation constant for HCN is K4 = 4.9 × 10-10. 4.81 9.31 4.65 0.301 O 1.57 10-5
Find the pH of 0.130 M NaCN solution. For HCN, Ka=4.9×10^-10