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Which of the following Ka values represent the weakest acid?
The Ka value closest to 1 x 10^-7 represents the weakest acid, as this value corresponds to a neutral solution and indicates a weaker dissociation of the acid.
Which of the following Ka value represent the weakest acid?
ka= 1.62 x 10^-12
How to calculate the Ka of an acid?
To calculate the Ka of an acid, you can use the equation Ka H3OA- / HA, where H3O is the concentration of hydronium ions, A- is the concentration of the conjugate base, and HA is the concentration of the acid. The Ka value represents the acid's strength in donating protons in a solution.
Which is the following describes the relationship between acid strength and Ka value for weak acids?
The Ka value of a weak acid is inversely related to its acid strength. A higher Ka value indicates a stronger acid, while a lower Ka value indicates a weaker acid. Acid strength is determined by the extent of dissociation of the acid in solution, with stronger acids having higher dissociation constants (Ka values).
What is Ka for HNO2 aq H aq NO2-aq?
Ka= [H+][NO2-] [HNO2]
Which of the following Ka values represent the weakest acid?
The Ka value closest to 1 x 10^-7 represents the weakest acid, as this value corresponds to a neutral solution and indicates a weaker dissociation of the acid.
Which of the following Ka value represent the weakest acid?
ka= 1.62 x 10^-12
The abbreviation Ka represents?
acid dissociation constant
How to calculate the Ka of an acid?
To calculate the Ka of an acid, you can use the equation Ka H3OA- / HA, where H3O is the concentration of hydronium ions, A- is the concentration of the conjugate base, and HA is the concentration of the acid. The Ka value represents the acid's strength in donating protons in a solution.
What is Ka in chemistry?
Ka in chemistry is the equilibrium constant that measures the strength of a weak acid in solution. It represents the extent of ionization of the acid in water. A higher Ka value indicates a stronger acid.
Which is the following describes the relationship between acid strength and Ka value for weak acids?
The Ka value of a weak acid is inversely related to its acid strength. A higher Ka value indicates a stronger acid, while a lower Ka value indicates a weaker acid. Acid strength is determined by the extent of dissociation of the acid in solution, with stronger acids having higher dissociation constants (Ka values).
What is Ka for HNO2 aq H aq NO2-aq?
Ka= [H+][NO2-] [HNO2]
How can one determine the acid dissociation constant (Ka) from the concentration of a solution?
To determine the acid dissociation constant (Ka) from the concentration of a solution, you can measure the concentrations of the acid, its conjugate base, and the equilibrium concentrations of both in the solution. By using these values in the equilibrium expression for the acid dissociation reaction, you can calculate the Ka value.
What is the acid dissociation constant for an acid HX at equilibrium?
The acid dissociation constant (Ka) for an acid HX at equilibrium is the ratio of the concentrations of the products (H+ and X-) to the undissociated acid (HX) in the equilibrium expression for the dissociation reaction. It is a measure of the strength of the acid, with higher Ka values indicating a stronger acid.
How do Ka values of weak acid and a strong acid compare?
The Ka value of a weak acid is smaller than the Ka value of a strong acid because weak acids only partially dissociate in solution, resulting in lower concentrations of H+ ions. Strong acids like hydrochloric acid (HCl) completely dissociate in solution, leading to higher concentrations of H+ ions and therefore a larger Ka value.
What is the Ka for acetic acid CH3COOH?
The Ka for acetic acid (CH3COOH) is approximately 1.8 x 10^-5. This value represents the acid dissociation constant for acetic acid, indicating its strength as a weak acid. An acid with a higher Ka value will dissociate more readily in solution.
What is the relationship between the Ka and Kb values in a chemical reaction?
The Ka and Kb values in a chemical reaction are related by the equation Ka x Kb Kw, where Kw is the ion product constant of water. This relationship shows that as the Ka value increases, the Kb value decreases, and vice versa. This means that a stronger acid will have a weaker conjugate base, and a stronger base will have a weaker conjugate acid.
