WebA) AgCN ⇋ Ag+ + CN− Ksp = 2.2 × 10−16 B) H2O + H2O ⇋ H3O+ + OH− Kw = 1 × 10−14 C) [Ag+] = [CN−] + [HCN] D) CN− + H2O ⇋ HCN + OH− Kb = 1.6 × 10−5 E) HCN + H2O ⇋ CN− + H3O+ Ka = 6.2 × 10−10 E Calculate the pH of a 0.010 M CH3CO2H solution. Ka = 1.8 × 10−5 for acetic acid. A) 9.26 B) 3.39 C) 2.02 D) 10.61 E) 4.74 B Students also viewed Quiz 11

Solved Write a balanced net ionic equation to show why the - Chegg

WebExpert Answer Transcribed image text: 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 Previous question Next question WebThe simultaneous solubility of $\mathrm{AgCN}\left(\mathrm{K}_{e p}=2.5 \times\right.$ $10^{-6}$ and $\mathrm{AgCl}\left(\mathrm{K}_{\text {ep }}=1.6 \times 10^{-10}\right)$ in … unconfirmed start of archive

Calculate simultaneous solubility of $AgCNS$ and $AgBr$ in a solution

WebThe simultaneous solubility of AgCN(K sp=2.5×10 −16) and AgCl(K sp=1.6×10 −10) in 1.0 M NH 3(aq.) are respectively: (Given K f [Ag(NH 3) 2] +=10 7) A 5.7×10 −8, 0.037 B 2.5×10 −6, 0.031 C 2.8×10 −15, 0.025 D 3.8×10 −15, 0.035 Hard Solution Verified by Toppr Correct option is A) Solve any question of Equilibrium with:- Patterns of problems > WebWrite a balanced net ionic equation to show why the solubility of AgCN (S) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Be sure to specify states such as (aq) or (S). + + + K= Submit Answer Previous question Next question WebNov 21, 2024 · The solubility of silver bromide at the new temperature must be known. Normally the solubility increases and some of the solid silver bromide will dissolve. ... AgCN. S15.2.X. 1.3 g. Q15.2.X. Calculate the minimum concentration of ammonia needed in 1.0 L of solution to dissolve 3.0 × 10 –3 mol of silver bromide. unconfirmed bitcoin hacking script