The fully protonated form of the amino-acid glycine (R=H) may be simply written as H2Gly+. Write the balanced acid dissociation equilibria (Ka1 and Ka2) for this acid.

How (which direction: right or left) will the equilibrium shift if PCl3 is removed as it is formed? Why will it shift in that direction? PCl5 (g) + heat ⇌ PCl3 (g) + Cl2 (g)

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. 0.04 mol of NaOH is added to 1. of a 0.2 MHF solution. 0.1 mol of HI is added to 1.0 L of a solution that is 0.7 M in both HF and KF 000000 acids: 0 Obases: 0 O other: O acids: O bases: 0 Oother: O X 0.0 S ?圖面固 C 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 HCH3CO2 is a weak acid. 1.6 mol of NaOH is added to 1.0 L of a 1.0M HCH3 CO2 solution. 0.62 mol of HBr is added to 1.0 L of a solution that is 1.5M in both HCH3CO₂ and KCH3CO2. 0 acids: bases: other: acids: bases: other: П 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 NH, is a weak base. acids: 1.0 mol of HNO, is added to 1.0 L of a 1.0 M NH, bases: O solution other: 0.2 mol of HBr is added to O acids: 1.0 L of a solution that is O. bases: 0.7 M in both NH, and NH Br. other: Check Explanation 2021 McGraw-Hi Education. All Rights Reserved. Terms of Use Privacy Accessibility

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. 0.6 mol of HI is added to 1.0 L of a 0.6M NH3 solution. 0.09 mol of KOH is added to 1.0 L of a solution that is and 0.2M in both NH3 NH₁Br. acids: n bases: other: acids: bases: other: X 0,0,... 5

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. acids: ☐ 0.2 mol of HBr is added to 1.0 L of a 0.6M NH3 solution. bases: ☑ other: ☐ 0.06 mol of HNO3 is added acids: ☐ to 1.0 L of a solution that is bases: ☐ 0.2M in both NH3 and NH,C1. 4 other: ☐ 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 HCH₂ CO₂ is a weak acid. 1.7 mol of NaOH is added to 1.0 L of a 1.0M HCH₂ CO₂ solution. 0.4 mol of HCl is added to 1.0 L of a solution that is 0.8M in both HCH₂ CO₂ and NaCH3 CO₂. acids: 0 bases: other: acids: bases: other: □ X 0,0,... Ś ? 00. 18 Ar

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. acids: 0,0,... 0.20 mol of HNO, is added to 1.0 L of a 1.2M NH, bases: U solution. other: 0.3 mol of KOH is added to acids: 1.0 L of a solution that is 0.6M in both NH, and bases: U NH,CI. other: I

3. Answer all sections (i) - (iv). 1 mole of ethanol (C2H5OH) and 1 mole of ethanoic acid (CH;COOH) were reacted at 25 °C, in a non- aqueous solvent, until equilibrium was reached. It was subsequently determined that 0.33 moles of ethanol remained at equilibrium. (i) Write an equation for the reaction. (ii) Write an expression for the equilibrium constant, Kc, for the reaction and calculate its value. Subsequently a further 3 moles of C2H5OH was added to the solution. (ii) Determine the concentrations of all the species present when equilibrium is restored.