The pH of a 0.0147M KCN solution is
A | 8.48 |
B | 3.3 |
C | 5.52 |
D |
10.7 |
HCN is a weak acid (Ka=6.20×10−10) , so the salt, KCN, acts as a weak base. What is the pH of a solution that is 0.0420M in KCN at 25 °C?
calculate the pH of each of the following solutions: a. NaCH3C02 0.63M b. NH4Cl 0.19M c. AlCl3 0.055M d. KCN 0.65M
Draw the major chemical species (excluding solvent) that exist at pH = 5.52 for a solution containing methionine
PQ-25. An aqueous buffer solution contains only HCN (PK, = 9.31) and KCN and has a pH of 8.50. What can be concluded about the relative concentrations of HCN and KCN in the buffer? (A) [HCN]> [KCN] (B) [HCN]< [KCN] (C) [HCM] = [KCN] (D) nothing can be concluded about the relative concentrations
What is the pH of a 0.4 M KCN solution? For HCN K - 4.9 * 10-10 2.54 11.46 4.85 9.71
16) The pH of an aqueous solution of 9.19×10-2 M potassium cyanide, KCN (aq), is ___ . This solution is acidicbasicneutral
Determine the pH of a 1.50 M sodium Cyanide (KCN) solution? be sure to show the 5% check!
Given that Ka for HCN is 6.2*10^-10, calculate the pH of a 0.15 M KCN solution.
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.
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?