Answer:
Strong acids are assumed 100% dissociated in water- True
As a solution becomes more basic, the pOH of the solution increases- false
The conjugate base of a weak acid is a strong base- true
The Ka equilibrium constant always refers to the reaction of an acid with water to produce the conjugate base of the acid and the hydronium ion- True
As the Kb value for a base increases, base strength increases- true
The weaker the acid, the stronger the conjugate base- true
Explanation:
An acid is regarded as a strong acid if it attains 100% or complete dissociation in water.
The pOH decreases as a solution becomes more basic (as OH^- concentration increases).
Ka refers to the dissociation of an acid HA into H3O^+ and A^-.
The greater the base dissociation constant, the greater the base strength.
The weaker an acid is, the stronger , its conjugate base will be.
Let's see the reasons behind these true or false:
1. Strong acids have a large dissociation constant, so they dissociate completely in water.
An acid is regarded as a strong acid if it attains 100% or complete dissociation in water.
2. The pOH decreases as a solution becomes more basic.
3. Ka refers to the dissociation of an acid HA into [tex]H_3O^+ and A^-[/tex]
4.The greater the base dissociation constant, the greater the base strength.
5. Kb value for a base increases, base strength increases
6.The weaker an acid is, the stronger its conjugate base will be.
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