What is the pOH of a 0.23-M HCN solution? Ka = 4.9 x 10-10
Calculate the pH of a 1.2 M HCN solution. Ka = 4.9 x 10 ^-10 for HCN (would appreciate if you wrote it down on a piece of paper so I don't get confused by the math)
The pH of a solution of 0.100 M HCN, given Ka= 4.9 X 10^-10 is Answer is supposed to be 5.5, but I'm not sure why
Calculate the pH of 3.083 M HCN (aq) acid solution, Ka = 4.9 x 10−10
Calculate the volumes of 0.200 M hydrocyanic acid, HCN (Ka = 4.9 x 10–10) solution, and 0.200 M of sodium cyanide, NaCN, solution needed to prepare 100.0 mL buffer solution with pH = 9.5
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 solution of 0.10 M hydrogen cyanide HCN? (Ka = 4.9 x 10-10) The answer is 5.15 please explain.
Find the pH of 0.130 M NaCN solution. For HCN, Ka=4.9×10^-10
Hydrocyanic acid, HCN is a weak acid with a Ka of 4.9 x 10^-10. What pH would a 0.50M solution of HCN have? Calculate the Kb value for NaCN using information from the previous question.
!!!!!!!!!!!!!!! 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.
There is a solution that is 3.2×10−2 M in HCN (Ka=4.9×10−10) and 1.7×10−2 M in NaCN. Calculate the concentrations of all species present in this solution. Express your answers in the given order using two significant figures separated by commas.