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Water is a toxic solvent widely used for chemical analyses.
Water is a toxic solvent widely used for chemical analyses.
False
Electrolytes form ions when dissolved in water, resulting in non-conductive solutions.
Electrolytes form ions when dissolved in water, resulting in non-conductive solutions.
False
Ethanol is an example of a non-electrolyte.
Ethanol is an example of a non-electrolyte.
True
According to Arrhenius theory, acids are sources of hydroxide ions (OH-).
According to Arrhenius theory, acids are sources of hydroxide ions (OH-).
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Acetate ion is the conjugate base of acetic acid.
Acetate ion is the conjugate base of acetic acid.
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Water can act as both an acid and a base depending on the solute present.
Water can act as both an acid and a base depending on the solute present.
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Autoprotolysis is a spontaneous reaction that involves the formation of a pair of ionic species.
Autoprotolysis is a spontaneous reaction that involves the formation of a pair of ionic species.
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Chemical equilibrium is a state where the ratio of concentrations of reactants and products can vary over time.
Chemical equilibrium is a state where the ratio of concentrations of reactants and products can vary over time.
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The concentration of water in dilute aqueous solutions is usually higher than the concentration of hydronium and hydroxide ions.
The concentration of water in dilute aqueous solutions is usually higher than the concentration of hydronium and hydroxide ions.
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The ion-product constant for water (Kw) at room temperature is typically 1.00×10^14.
The ion-product constant for water (Kw) at room temperature is typically 1.00×10^14.
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Taking the negative logarithm of the ion-product constant for water provides an unhelpful relationship.
Taking the negative logarithm of the ion-product constant for water provides an unhelpful relationship.
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The ion-product constant for water allows for easy determination of the concentrations of hydronium and hydroxide ions in solutions.
The ion-product constant for water allows for easy determination of the concentrations of hydronium and hydroxide ions in solutions.
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