Numbers of millimoles of KOH that are needed to neutralize 35 .1 mL of 0 .101 M nitric acid has to be calculated. Concept introduction: The mole of the solution can be calculated by using following formula Molarity of the solution = Number of moles of solute Volume of solution in litre Number of moles = Molarity of the solution × Volume of solution in litre

Question

Identifying the major species in weak acid or weak base equilibria Your answer is incorrect. • Row 2: Your answer is incorrect. • Row 3: Your answer is incorrect. • Row 6: Your answer is incorrect. 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 HF is a weak acid. acids: HF 0.1 mol of NaOH is added to 1.0 L of a 0.7M HF solution. bases: 0.13 mol of HCl is added to 1.0 L of a solution that is 1.0M in both HF and KF. Exponent other: F acids: HF bases: F other: K 1 0,0,... ? 000 18 Ar

Answer 1

Question

Chapter 16, Problem 16.15QE

Interpretation Introduction

Interpretation:

Numbers of millimoles of KOH that are needed to neutralize 35.1 mL of 0.101 M nitric acid has to be calculated.

Concept introduction:

The mole of the solution can be calculated by using following formula

Molarity of the solution = Number of moles of soluteVolume of solution in litreNumber of moles = Molarity of the solution × Volume of solution in litre

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