Find the pH of 0.130 M NaCN solution. For HCN, Ka=4.9×10^-10
What is the pH of a 0.84 M solution of NaCN (Ka of HCN = 6.2x10^-10)
What is the pH of a 0.670 M solution of NaCN (Ka of HCN is 4.9x10^-10?
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.
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 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)
Solve for the pH of a 0.0986 M solution of NaCN. Given Ka (HCN)= 6.2 * 10-10 Please have two decimal places for your answer.
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
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.
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.