6) Calculate the pH of a 0.021 M NaCN solution. [K (HCN) 4.9 x 1010] 6)...
21. Which of these oxides will produce a basic solution when dissolved in water? A) CO2 B) SO C) P205 D) Rb20 Ks = 2.0 x 10-5 22. Calculate the pH of a 0.021 M NaCN solution. [K, = 4.9 x 10-10 A) 1.68 B) 3.18 C) 5.49 D) 7.00 E) 10.82 23. Which response gives the products of hydrolysis of KF? A) KOH + HF B) OH + HF C) KOH + H+F D) KH+ + OH E) No...
Calculate the pH of a 0.75M aqueous solution of NaCN, Ka for HCN = 6.2E-10 Can someone explain to me how to do this problem step by step, and also explain why the reaction equation was written the way it was?? Calculate the pH of a 0.75 M aqueous solution of NaCN, K, for HCN is 6.2 X 1010. CNag)+ H2)HCNa)+ OH (aq) A/700 8) 9,21 15 0)479 A) 7.00 B) 9.2 C) 11.54D) 4.79 E) 2.46
8) Calculate the [H30+) and the pH of a 0.021 M HNO3 solution. A) 4.8 x 10-13 M and 12.32 B) 4.8 * 10-13 M and -12.32 C) 0.021 M and -1.68 D) 0.021 M and 1.68
Find the pH of 0.130 M NaCN solution. For HCN, Ka=4.9×10^-10
a) Calculate the pH for a 1.63 M solution of HCN which also contains 1.75 M NaCN. Ka = 4.9 x 10-10 for HCN b) Calculate the pH after 65.0 mL of 1.47 M HCl is added to 850.0 mL of the solution in part a) above.
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 0.65 M NaCN. What is the concentration of HCN in the solution? PH= [HCN]= Times 10 M
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)
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.
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