Please help! What is the value of K_b for the cyanide anion, CN^-? K_a (HCN) =...
What is the value of Ky for the cyanide anion, CN? Ka(HCN) = 6.2 * 10-10 Multiple Choice points _ οοοοε Ο Ο 16 και 10-5 Book Ο 3.8 10-5 References Ο 6.2 x 104 Ο 38, 104 Ο 1610-4
Calculate the concentration of cyanide (CN–) in a 0.450 M solution of hydrocyanic acid HCN and 0.10M –10 HCl. [For HCN, Ka = 6.2 × 10] a. 0.1M b. 2.8×10–9M c. 7.8×10–5M d. 1.1×10–6M e. 0.21 M with steps please
What percentage of total cyanide (CN- +HCN) is present as HCN at a pH = 7?
Consider the figure shown below. What is the pK_a of hydrogen cyanide, HCN? what is the value of TOTCN for the solution depicted in the figure? Is hypoiodous acid, H0I (pK_a = 10.70), a stronger or weaker acid than HCN? Type stronger or weaker, then briefly explain. Which is the stronger base, cyanide (CN^-) or hypoiodite (OI^-)? Type cyanide or hypoiodite, then briefly explain.
Given that Ka for HCN is 6.2 x 10-10 at 25 °C, what is the value of Kb for CN- at 25 °C? Given that Ka for (CH3)2 NH is 5.4 x 10-4 at 25°C, what is the value ofKa for (CH3)2NH2+ at 25 °C?
Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of 2.160. The Ksp for Zn(CN)2 is 3.0 × 10–16. The Ka for HCN is 6.2 × 10–10. Hint: Use the systematic treatment of equilibrium to solve this problem. 1. Write the pertinent reactions. 2. Write the charge balance equation. 3. Write the mass balance equations. 4. Write the equilibrium constant expressions for each reaction. 5. Count the equations and unknowns. 6. Solve for...
Given the following reactions, what is the Ka value for HIO? IO– + HCN ⇄ HIO + CN– K = 27 HCN + H2O ⇄ CN– + H3O+ K = 6.2 × 10–10 A. Ka(HIO) = 4.4 × 10–4 B. Ka(HIO) = 6.0 × 10–7 C. Ka(HIO) = 1.7 × 10–8 D. Ka(HIO) = 2.3 × 10–11
What is the Ka reaction of HCN? click to edit The Ka of HCN is 6.2 × 10-10. What is the Kb value for CN-at 25°C? Number
What is the Ka reaction of HCN? Ka reaction _______ The Ka of HCN is 6.2 x 10-10. What is the Kb value for CN- at 25 °C?
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Calculate the following for a 0.002 M aqueous solution of NH_3 (K_b = 1.75 times 10^-5). The[OH^-] The pH