Preform a calculation to determine the amount of [Co(NH3)5Cl]Cl2 required to make 100.00 mL of a 1.20 x 10-3 M Solution.
Preform a calculation to determine the amount of [Co(NH3)5Cl]Cl2 required to make 100.00 mL of a...
Calculation of percent yield of [Co(NH3)5Cl]Cl2: I'm having trouble with these steps: Calculation of limiting reagent for synthesis of [Co(NH3)5Cl]Cl2 (assume H2O2 present in excess) Calculation of theoretical yield of [Co(NH3)5Cl]Cl2 These are the reactants we used: 2.010g NH4Cl, 15mL 15M NH3, 4.067g CoCl26H2O, 3.2mL 32% H2O2, 15mL 12M HCl This is the equation used: 2CoCl2*6H2O + H2O2 + 8NH3 + 2NH4Cl --> 2[Co(NH3)5Cl]Cl2 + 14H2O
IR for [Co(NH3)5Cl]Cl2 List the major peaks that are present in the spectrum and the functional groups responsible for each one. 98 BRUKER 96 94 92 Transmittance [%] 90 88 86 84 - 3170.47 1558.64 1307.50 - 843.09 7488.13 3500 3000 1500 1000 500 2500 2000 Wavenumber cm-1 C:\Users\Jordan Chemistry\Documents\Bruker OPUS_8.2.28\DATAMEAS chloride. O Chloride Instrument type and / or accessory 3/12/2020
For [ Co(NH3)6]Cl3, [Co(NH3)5Cl1]Cl2, and [Co(NH3)4Cl2]Cl. 1) Determine the point group for each species 2) Assuming each species completely dissolves in water, determine the number of ions that would be present in solution for each. 3) Determine the total percent chlorine in each of the three compounds I need help understanding these aspects a bit more (like determining the number of ions and determining percent chlorine without an experimental mass) . I have an idea for the point groups but...
A buffer solution is prepared by dissolving 1.600 g of ammonium chloride (NH,CI) into 100.00 mL of a 0.160 M solution of ammonia (NH3). The Kb of ammonia is 1.8 x 10-5. What is the pH of the solution?
2&3 please show work Question 2) 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before the addition of any HNO3. The Kb of NH3 is 1.8x 10-5 A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55 Answer "Calculation: Question 3) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LICHO2. The Ka for HCHO2 is 1.8...
A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K = 1.34 x 10-6, 3.00 M O sodium bisulfate monohydrate, K = 1.20 x 10,3.00 M acetic acid, K, = 1.75 x 10-6, 5.00 M formic acid, K, = 1.77 x 10 , 2.00 M Determine which conjugate base is the best option to make a buffer at...
A student must make a buffer solution with a pH of 1.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K =1.34 x 10 5,3.00 M acetic acid, Ka = 1.75 x 10,5.00 M O formic acid, Kg = 1.77 x 104,2.00 M sodium bisulfate monohydrate, K = 1.20 x 102,3.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. sodium...
mges Calculations-(3 pts) Calculation used to determine the mass of Na2HPO4 needed to make 50 mL of a 0.4M buffer solution.
100.0 mL of 1.23X10-3 M Co(NO3)3 is mixed with 150.0mL of 0.22M NH3. What is the [Co+3] at equilibrium? [Kf for Co(NH3)6 +3 is 2.3 x 1033]
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.