-ldentifying the major species in weak acid or weak base equilibria The preparat

Question

-ldentifying the major species in weak acid or weak base equilibria 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 l 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 NH2 is a weak base 2 mol of HNO, is added to 1.0L of a 0.9 MNH solution. acids: D bases: I other: 0.15 mol of HC is added to acids: 1.0 L of a solution that is 1.1 Min both NH2 and NH ,C1 bases other: Check Terms of U

Explanation / Answer

1)

HNO3 is an acid whereas NH3 is a weak base

Reaction between acid and base will be

HNO3 + NH3 ----- NH4NO3

Number of moles of HNO3 = 2 moles

Number of moles of NH3 = Volume of solution (in L) * Molarity of NH3 = 1.0L * 0.9 = 0.9 moles

Hence after reaction number of moles of HNO3 left = 2 - 0.9 = 1.1

Number of moles of NH4NO3 formed = 0.9

Hence major species will be HNO3 and NH4NO3

2)

HCl is an acid, NH3 is a base and NH4Cl is a salt of strong acid and weak base (hence category will be other)

Number of moles of NH3 = Number of moles of NH4Cl = Volume in L * Molarity = 1L * 1.1M = 1.1 moles

HCl + NH3 ------- NH4Cl

Number of moles of HCl = 0.15

Number of moles of NH3 left = 1.1 - 0.15 = 0.95

Number of moles of NH4Cl formed = 1.1 + 0.15 = 1.25

Hence major species are NH4Cl and NH3 in this reaction

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