It is given that for a common type of reaction the value of K < < 1 . The assumption made when solving the equilibrium concentrations for reactions with small K values and the procedure followed if the ‘ 5 % rule’ fails are to be stated. Concept introduction: If the error in the equilibrium concentration calculated is less than 5 % , the assumption made is stated to be correct. This is known as the ‘ 5 % rule’. If the error exceeds the 5 % value, then the quadratic formula is used for calculating the equilibrium concentrations. To determine: The assumption made when solving the equilibrium concentrations for reactions with small K values and the procedure followed if the ‘ 5 % rule’ fails.
It is given that for a common type of reaction the value of K < < 1 . The assumption made when solving the equilibrium concentrations for reactions with small K values and the procedure followed if the ‘ 5 % rule’ fails are to be stated. Concept introduction: If the error in the equilibrium concentration calculated is less than 5 % , the assumption made is stated to be correct. This is known as the ‘ 5 % rule’. If the error exceeds the 5 % value, then the quadratic formula is used for calculating the equilibrium concentrations. To determine: The assumption made when solving the equilibrium concentrations for reactions with small K values and the procedure followed if the ‘ 5 % rule’ fails.
Solution Summary: The author explains how the quadratic equation method is used for solving the equilibrium concentrations for reactions with small K values and the procedure followed if the 5% rule fails.
Interpretation: It is given that for a common type of reaction the value of
K<<1. The assumption made when solving the equilibrium concentrations for reactions with small
K values and the procedure followed if the ‘
5% rule’ fails are to be stated.
Concept introduction: If the error in the equilibrium concentration calculated is less than
5%, the assumption made is stated to be correct. This is known as the ‘
5% rule’. If the error exceeds the
5% value, then the quadratic formula is used for calculating the equilibrium concentrations.
To determine: The assumption made when solving the equilibrium concentrations for reactions with small
K values and the procedure followed if the ‘
5% rule’ fails.
What is the [OH⁻] of a 1.80 M solution of pyridine (C₅H₅N, Kb = 1.70 × 10⁻⁹)?
What is the percent ionization in a 0.260 M solution of formic acid (HCOOH) (Ka = 1.78 × 10⁻⁴)?
Determine the pH of solution of HC3H5O2 By constructing an ICE table writing the equilibrium constant expression, and using this information to determine the pH. The Ka of HC3H5O2 is 1.3 x 10-5
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