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. You will find it useful to keep in mind that NH3 is a weak base. 1 mol of HBr is added to 1.0 L of a 0.9M NH3 solution. 0.1 mol of HNO3 is added to 1.0 L of a solution that is 0.3 M in both NH3 and NH₂Br. acids: bases: other: acids: bases: Oother: ooo ロロ X 00 0.0....

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. You will find it useful to keep in mind that HCN is a weak acid. acids: 0,0,.. 0.7 mol of KOH is added to 1.0 L of a 0.7M HCN bases: ? solution. other: U 0.1 mol of HNO, is added to acids: 1.0 L of a solution that is bases: 0.4M in both HCN and NaCN. other: U

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. You will find it useful to keep in mind that NH, is a weak base. 0.7 mol of HNO, is O acids: O On added to 1.0 L of a bases: O 0.7 M NH, solution. ? O other: D 0.07 mol of HCl is added to 1.0 L of a solution that is 0.3 M in both NH, and acids: 0 bases: O O other: O NH,CI.

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. You will find it useful to keep in mind that HCH3CO₂ is a weak acid. 1 mol of NaOH is added to 1.0 L of a 0.6M HCH3 CO2 solution. 0.59 mol of HI is added to 1.0 L of a solution that is 1.2M in both HCH3CO₂ and KCH3CO2. acids: bases: other: 0 acids: bases: other: X 0,0,... Ś

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. You will find it useful to keep in mind that HCH3CO₂ is a weak acid. 0.4 mol of NaOH is added to 1.0 L of a 0.4MHCH, CO₂ solution. 0.1 mol of NaOH is added to 1.0 L of a solution that is 0.5M in both HCH, CO₂ and KCH, CO₂- □ acids: bases: other: acids: 0 bases: 17 other: X Ś

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. You will find it useful to keep in mind that HF is a weak acid. 1 mol of KOH is added to 1.0 L of a 0.6M HF solution. fn 0.3 mol of NaOH is added to 1.0 L of a solution that is 0.9M in both HF and KF. Explanation tab shift caps lock Check esc O acids: Obases: Oother: O 0 0 0 0 0 0 O acids: Obases: O Oother: O ! 1 A Q A Z 1 control option @ 2 A W S ►► # 3 X command E X D 00 $ 4 0.0.... 3 R F % 5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility MacBook Pro 80 T 6 G Y B & 7 H U * 8 N J ( 9 4 7 K M ) O O A…

The undissociated base (B) is present in the greatest concentration, with the products being present in relatively smaller amounts in this equilibrium mixture. How would this affect the magnitude of Kb? Do you expect it to be small or large? Which is the strongest base? Name of base Ammonia (NH3) Methylamine (CH3NH2) Ethylamine (C2H5NH2) Diethylamine (C2H5)2NH Pyridine (CSH5N) Kb value 1.76 x 10-5 Why? 4.4 x 10-4 5.6 x 10-4 Which is the weakest base? 1.3 x 10-3 1.7 x 10-9 Why? The larger the Kb the (stronger/weaker) the base. Since a weak base dissociates incompletely setting up an equilibrium, what method could you think of that you could use to determine the concentration of [OH"] ions given the initial concentration of the acid and its Kb?

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. You will find it useful to keep in mind that HF is a weak acid. 1 mol of KOH is added to 1.0 L of a 0.9M HF solution. 0.46 mol of KOH is added to 1.0 L of a solution that is 1.0M in both HF and NaF. U acids: bases: other: acids: bases: other: X 0,0,... Ś

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. You will find it useful to keep in mind that NH, is a weak base. 0.26 mol of HCl is added to 1.0 L of a 1.2MNH₂ solution. 0.06 mol of HBr is added to 1.0 L of a solution that is 0.2M in both NH3 and NHẠC.. acids: bases: other: acids: bases: other: 1 09 X 8 0.0... S

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. You will find it useful to keep in mind that NH, is a weak base. 1 mol of HNO3 is added to 1.0 L of a 0.6M NH3 solution.. 0.55 mol of NaOH is added to 1.0 L of a solution that is 1.5M in both NH3 and NH.CI. ☐ acids: ☐ ☐ bases: ☐ O other: O acids: ☐ bases: O other: 0° 0 0,0.... X 5