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What best describes solutions of equal concentrations of HCL and CH3COOH?
Wiki User
∙ 10y ago
Do not have the same pH.
Wiki User
∙ 10y ago
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What are the equilibrium concentrations of hydronium ion acetate ion and acetic acid in a 0.10 m aqueous solution of acetic acid?
In a 0.10 M aqueous solution of acetic acid, the equilibrium concentrations of hydronium ion (H3O+) and acetate ion (CH3COO-) will be equal to the initial concentration of the acetic acid, which is 0.10 M. The concentration of acetic acid (CH3COOH) will decrease by an amount equal to the amount of hydronium ion produced.
The acid base indicator bromcresol green is weak acid. The yellow acid and blue base forms of the indicator are present in equal concentrations in a sloution when the pH 4.68. What is b.g. pKa?
By definition, the pKa of a weak acid is the pH at which the concentrations of the acid and its conjugate base are equal. In this case, since the solution is yellow (acid) and blue (base) at pH 4.68, it means that the concentration of the acid and base forms of the indicator are equal. Therefore, the pKa of bromcresol green is 4.68.
Why does pH scale generally range from 0 to 14 in aqueous solutions?
The pH scale ranges from 0 to 14 in aqueous solutions because it corresponds to the concentration of hydrogen ions (H+) in the solution. A pH of 7 is considered neutral, with equal concentrations of H+ and OH- ions. Values below 7 indicate an acidic solution with higher H+ concentrations, while values above 7 indicate a basic solution with lower H+ concentrations.
Is it true that solutions that have an equal concentration of H plus ions and OH- are considered acidic?
No, solutions with equal concentrations of H+ and OH- ions (pH of 7) are considered neutral. Acids have more H+ ions than OH- ions, while bases have more OH- ions than H+ ions.
What is a following characterizes a reaction at equilibrium?
At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. The concentrations of reactants and products remain constant over time. The equilibrium constant, which is the ratio of product concentrations to reactant concentrations, is constant at a given temperature.
What are solutions with equal concentrations of solutes?
isotonic
How are the concentrations of hydronium ions and hydroxide ions in aqueous solutions related?
The concentrations of hydronium (H3O+) and hydroxide (OH-) ions in aqueous solutions are inversely related. As one increases, the other decreases. This relationship is based on the autoionization of water, where water molecules can act as both acids (donating H+ ions to form hydronium ions) and bases (accepting H+ ions to form hydroxide ions).
What are the equilibrium concentrations of hydronium ion acetate ion and acetic acid in a 0.10 m aqueous solution of acetic acid?
In a 0.10 M aqueous solution of acetic acid, the equilibrium concentrations of hydronium ion (H3O+) and acetate ion (CH3COO-) will be equal to the initial concentration of the acetic acid, which is 0.10 M. The concentration of acetic acid (CH3COOH) will decrease by an amount equal to the amount of hydronium ion produced.
What are the hydrogen ion and hydrogen ion concentrations in water?
These concentrations are supposed to be equal.
The acid base indicator bromcresol green is weak acid. The yellow acid and blue base forms of the indicator are present in equal concentrations in a sloution when the pH 4.68. What is b.g. pKa?
By definition, the pKa of a weak acid is the pH at which the concentrations of the acid and its conjugate base are equal. In this case, since the solution is yellow (acid) and blue (base) at pH 4.68, it means that the concentration of the acid and base forms of the indicator are equal. Therefore, the pKa of bromcresol green is 4.68.
What is osmosis controlled by?
Osmosis is primarily controlled by the concentration gradient of solute particles across a selectively permeable membrane. Water will move from an area of low solute concentration to an area of high solute concentration in an attempt to equalize the concentrations on both sides of the membrane.
What will happen to two solutions in equilibrium?
In a dynamic equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction, causing no overall change in the concentrations of the reactants and products. This results in a stable state where both solutions coexist without any noticeable changes over time.
Why does the level of a more concentrated solution rise when two solutions of different concentrations are separated by a semipermeable membrane and when does it stop rising?
The more concentrated solution is hypertonic and osmotic pressure (a hydrostatic force whose sole purpose in life is to make concentrations equal) tends to move solvent into the more concentrated solution. It will stop rising when either a) the solution concentrations are the same on both sides of the membrane, or b) when the osmotic pressure becomes equal to the ambient air pressure.
What has greater osmotic power at equal concentrations?
electrolytes
Why does pH scale generally range from 0 to 14 in aqueous solutions?
The pH scale ranges from 0 to 14 in aqueous solutions because it corresponds to the concentration of hydrogen ions (H+) in the solution. A pH of 7 is considered neutral, with equal concentrations of H+ and OH- ions. Values below 7 indicate an acidic solution with higher H+ concentrations, while values above 7 indicate a basic solution with lower H+ concentrations.
If the discriminant is zero the equation has solutions?
It has 2 equal solutions
Is it true that solutions that have an equal concentration of H plus ions and OH- are considered acidic?
No, solutions with equal concentrations of H+ and OH- ions (pH of 7) are considered neutral. Acids have more H+ ions than OH- ions, while bases have more OH- ions than H+ ions.
