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- Is it possible, upon precipitation of the third class ions, to add H2S first, then NH4OH and NH4Cl? And whyQ2- Give scientific explanation with equations for the following: I+ Despite of precipitant agent of both of cations of groups IV and I is sulfide ion. but they are separated. 2. A mixture of ammonium hydroxide and ammonium chioride s a source of hydroxide ion of ‘group three. 3- Cations of group Il is divided into sub groups a and b.Which salt below will produce the lowest [H 3O +] in an aqueous solution? 0.1170 M N2H5Br, Kb(N2H4) = 8.900e-7 0.1170 M CH3NH3Br, Kb(CH3NH2) = 0.0003700 0.1170 M CH3CH2CH2NH3Cl, Kb(CH3CH2CH2NH2) = 0.0005100 0.1170 M C6H5NH3Br, Kb(C6H5NH2) = 4.300e-10
- Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. NiS(s)-->When all of the following are mixed together in a beaker, what is the molar concentration of the SCN- ion in the solution just after mixing but before any reaction takes place? 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 4.00 mL of 2.00 x 10-3 M KSCN 4.00 mL of 0.50 M HNO3 answer is between 0.004 and 0.005, please explain how with steps.A 0.217 g sample of HgO (molar mass = 217 g/mol) reacts with excess iodide ions according to the reaction show below. Titration of the resulting sample solution requires how many moles of 0.10 M KI to reach the equivalence point? Assume complete reaction. HgO + 4 I- + H2O HgI42- + 2 -OH
- The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.010 M solution of HClO isThe acid- dissociated constant at 25.0 degres celcius for hypochlorous acid (HCIO) is 3.0x10-8. At equilibrium, the molarity of H3O+ in a 0.066M solution of HCIO is?v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH at 25oC is 1.76 x 10-5.
- In solutions 1-4 you are adding successively larger volumes of 0.00200 M SCN- to the Fe3+ solution and diluting to 10.00 mL. Calculate the final diluted molarity of SCN- in solution #1. 3 sig figs (Calculate the same thing for the solutions 2-4 and enter the results in table 3 as [SCN-] pre-equilibrium.)Write both the charge balance equation (CBE) and mass balance equation (MBE) for the following solutions at equilibrium: 1. 0.12 M H2A 2. 0.40 M NH4ClThe reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq)---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (HNO2) when 40.5 mL of 0.674 M KOH is required to quench 101.0 mL of Nitric acid over phenolphthalein indicator.