What is the base ionization constant, K, for CNK (HCN) - 4.9 x 10-10 CN" +...
What is the base ionization constant, Kb, for CN−? Ka(HCN) = 4.9 × 10−10 CN- + H2O HCN + OH-
The Ka for HCN is 4.9*10-10 What is the value of Kb for CN? 2.0*10-5 4.0*10-6 4.9*104 4.9*10-24 QUESTION 12 Calculation the concentration of [H] in a solution in which [OH-] = 4*[H+)? 07 0.5*10-14 4 5*10-8
Zorcaine, C13H24N,SCI, is the salt of the base articaine and hydrochloric acid. The ionization constant for articaine is 6.4 x 10-7. (a) Is a solution of zorcaine acidic or basic? acidic O basic (b) What are the [H20+], [OH-] (in M), and pH of a 2.0% solution by mass of zorcaine, assuming that the density of the solution is 1.0 g/mL. (Assume Kw = 1.01 10-14.) [H30+1 4.9) х м [OH^] 49 M 4.0 pH
8. The ionization constant, Ka, for HCN(aq) is 6.2 x 10". What is the pH of a 0.10 molar solution of sodium cyanide, which contains the cyanide ion? a. 5.10 b. 8.90 c. 9.21 d. 11.10 e. 11.30 9. The solubility product for Ag3PO, is: Kop = 2.8 x 101 What is the solubility of Ag,PO, in water, in moles per liter? a. 1.8 x 10M b. 2.5 x 10M c. 1.9 x 10 M d. 3.1 x 10M e....
CN Finally, calculate the CN concentration. (K. (HCN) - 1.9 x 10") Calculate the Ol concentration and pll of a 1.5 x 10-M aqueous solution of sodium cyanide, N [OH- M CN- OM
please the hole steps
Review Problem 16.099 For hydrocyanic acid, HCN, k, = 4.9 10-10 x Incorrect. Did you use the Ky value and not Ky? Did you set up your equilibrium expression in the correct way? Calculate the pH of 0.20 M NaCN. 5.004 pH = the tolerance is +/-2% X Incorrect. The concentration of OH must be equal to the concentration of HCN formed. Look at your work in Part a. What is the concentration of HCN in...
9. What is the pH for 0.20 M HCIO solution? K = 2.5 x 10-7 a) 4.05 b) 3.70 c) 4.80 d) 7.00 e) 7.40 10. What is the pH of a mixture containing 0.30 M HNO, and 0.15 M NaNO, (K, for HNO2 is 4.5 x 104) a) 4.35 b) 3.05 c) 4.65 d) 5.01 e) 4.05 11. Acid strength increases in the series: HCN <HF <HSO.. Which of these species is the strongest base? a) SO42- b) F-...
Determine the pH of a 1.0 x 10-2 M solution of HCN. Kb for CN- = 1.6 X 10-5 Select one: O a. 2.5 O b. 5.6 O C. -5.6 O d. -3.6 O e. 8.4
Which of the following chemical equations corresponds to the base ionization constant, K for hydrogen sulfite ion (HSO3? HSO3 aq)H2O()= H2SO3(aq) OH (aq) H2SO3(aq)OH(aq)=HSO3(aq) H20) HSO3aq)Haq) So32(aq)+H20( HSO3 aq) H20)= so32(aq) +H30 (aq) HSO3 (aq)H30 (aq)=H2SO3(aq)+ H20()
Problem 2: Find the concentrations of Ag, CN, and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: Ksp = 2.2 x 10-16 AgCN(s) CN + H20 Ag+ + CN- HCN(aq) + OH- Kb = 1.6 x 10-5