pr and (Ni+] in this solution. Kork for Ni (NH.), is 1 pt pr A solution...
23. A solution is prepared by adding 0.10 mole of Ni(NH3). Cl2 to 0.50 L of 3.2 M NH3. Calculate (Ni (NH3)&2+) and (Ni2+in this solution. Koveralt for Ni (NH3)22+ is 5.5 x 108. That is, 5.5 x 108 = Ni (NH3) 2+1 [Ni2+] [NH3] for the overall reaction Ni2+ (aq) + 6NH3(aq) = Ni (NH3). 2+ (aq) (Ni (NH3), 2+] = 0 [Ni2+] = C M
A solution is prepared by adding 0.075 mole of K3 [Fe(CN)6] to 0.72 L of 2.2 M NaCN. Assuming no volume change, calculate the concentrations of Fe(CN)63- and Fe3+ in this solution. The K (overall) for the formation of Fe(CN)63- is 1.0 x 1042. [Fe(CN)6*] = [Fe3+] = Submit Answer Try Another Version 2 item attempts remaining
A 0.180 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Ni?+ ions at equilibrium? Assume the formation constant of Ni(NH)2+ is 5.5 x 10
1 pt The molar solubility of silver sulfate in a 0.138 M sodium sulfate solution is M. 1 pt 1 pt Submit Answer Try Another Version 2 item attempts remaining 1 pt 1 pt
Copper(I) ions in aqueous solution react with NH3(aq) according to Cut(aq)2 NH (aq) - Cu(NH(aq) = 6.3 x 1010 Calculate the solubility (in g-L) of CuBr(s) (Ksp = 6.3 x 109) in 0.64 M NH3 (aq) solubility of CuBr(s): g/L
A 0.170 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Nia + ions at equilibrium? Assume the formation constant of Ni(NH)2+ is 5.5 x 10%.
can someone help me out!! Part A Using the Ke value of 1.2 x 109 calculate the concentration of Ni2+ (aq) and Ni(NH)that are present at equilibrium after dissolving 1.73 g NiCl2 in 100.0 mL of NH3(aq) solution such that the equilibrium concentration of NH3 is equal to 0.20 M. Express your answers in moles per liter to two significant figures separated by a comma. O AE ? Xy vx x x (X X x 10 ex [Ni2-1. [Ni(NH3)621 0.13,1.0...
о References) TUTOR Solution Concentration A solution is made by dissolving 27.7 g of nickel(II) chloride, NiCh, in enough water to make exactly 100 mL of solution. Calculate the concentration (molarity) of NiCl in mol/L (M). pt pt M NICl pr Submit Show Approach Show Tutor Steps pt Submit Answer Try Another Version 10 item attempts remaining 1 pt 1 pr 1 pt 1 pt 1 pt 1 pt 1 pf 1 pr 1 pr Pievious Naid a e to...
1 pt [cererences Use the References to access important values if needed for this question. 1 pt 1 pt The equilibrium constant, K, for the following reaction is 7.74x10-3 at 688 K. NH,I() NH3(g) + hi[g) 1 pt 1 pt 1 pt pt An equilibrium mixture in a 16.8 L container at 688 K contains 0.240 mol NHI(S), 0.115 M NHz and 6.73x10-2 MHI. What will be the concentrations of the two gases once equilibrium has been reestablished, if the...
For which of the following reactions is AS™ > 0. Choose all that apply. CH4(g) + H2O(g) + 3H2(g) + CO(g) NH,HS() + NH3(g) + H2S(g) 2H2O(g) + 2Cl2(g) + 4HCl(g) + O2(g) 2NO(g) + 2H2(g) → N2(g) + 2H2O(1) 2N2(g) + O2(g) → 2N2O(g) ООО Submit Answer Try Another Version 3 item attempts remaining ot pt pt The molar solubility of silver chromate in a 0.246 M sodium chromate solution is M Submit Answer Try Another Version 3 item...