A chemist is titrating 0.16 mol of HCl to 1.0 L of a solution that is 1.2 M in both NH3 and NH4Br. What are the major species in the solution? (water can be ignored)
A. H+, NH4+ , CI-
B. NH3 , NH4+ ,CI-
C. H+, NH3 , Br- ,CI-
D. NH3 , NH4+ ,CI- , Br-
E. NH3 , NH4+ ,H+ , Br-
A chemist is titrating 0.16 mol of HCl to 1.0 L of a solution that is 1.2 M in both NH3 and NH4Br
A chemist is titrating 0.16 mol of HCI to 1.0 L of a solution that is 1.2 M in both NH3 and NH Br. What are the major species in the solution? (water can be ignored) A. H+, NH3, Br,cr B. NH3, NH4+.cr, Br C. NH3, NH4+, H. Br D.HT, NH4+, cr E. NH3, NH4+, cr
a chemist is titrating 0.16 mol of HCl to 1.0 L of a solution that is 1.2 M in both nh3 and nh4br. what are the major species that are present in the solution?
A chemist is titrating 0.16 mol of HCI to 1.0L of a solution that is 12 M in both NH3 and NH Br What are the major species in the solution? (water can be ignored) AH NH3. Br.cr О В NH3, NH4.cr. Br С NH3 NH4tcr D NH3, NH4+, H. Br EH, NHA.CF
Calculate the molarity of a solution made by diluting 0.041 L of 0.16 M HCl solution to a volume of 1.0 L. Enter your answer in scientific notation. Be sure to answer all parts.
A) How many milliliters of 0.15 M HCl would have to be added to 1.0 L of a buffer containing 0.25 M NH3 and 0.45 M NH4 to make the pH decrease by 0.05 pH unit? The Ka value = 5.6 x 10^-10. B) How many milliliters of the same HCl solution would, if added to 0.204 L of pure water, make the pH decrease by 0.05 pH unit?
A chemist titrates 80.0 mL of a 0.3371 M ammonia (NH3) solution with 0.5400 M HCl solution at 25 °C. Calculate the pH at equivalence. The pK, of ammonia is 4.75. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added.
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row....
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row....
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row....
the pitepara of t aus o ion ih table below. For each solution, write the chemical formulas of the major spedies present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that wll act as acids in the acids' row, the formulas of the species that will act as bases in the bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other row You will...