30 Questions
What is the term used to describe quantitative chemical analysis that involves determining the volume of a solution of accurately known concentration?
Titrimetric analysis
What is the solution of accurately known strength called in titrimetric analysis?
Standard solution
What type of reactions involve the combination of hydrogen and hydroxide ions to form water?
Neutralization reactions
What is the process of determining the amount of substance A by adding a carefully measured volume of a solution with a known concentration of B?
Titration
What type of reactions depend on the combination of ions, other than hydrogen or hydroxide ions, to form a soluble, slightly dissociated ion or compound?
Complex formation reactions
What is the term formerly used for quantitative determination, but has now been replaced by titrimetric analysis?
Volumetric analysis
What is the term for the ratio [Salt] / [Acid] in the Henderson equation?
Buffer ratio
What is the pH of a solution containing equal concentrations of acid and its salt?
pKa
What is the effect of a tenfold increase or decrease of the buffer ratio on the pH of the solution?
It raises or lowers the pH by 1 unit
What is the purpose of titrating an alkaline solution with a standard solution of an acid?
To determine the amount of base present
What is the primary function of a buffer solution?
To resist changes in pH due to the addition of small amounts of acids or bases
What is the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate, given pKa = 4.76?
4.76
What is the term for the point at which the amount of acid is exactly equivalent chemically to the amount of base present in a titration?
All of the above
What happens to the pH of a solution when a strong acid is added to an ammonium hydroxide-ammonium chloride buffer?
The pH remains almost unchanged
What is the role of the salt in a buffer solution containing a weak acid and its salt?
To reduce the ionization of the weak acid
What is the conventional manner of writing the dissociation of a weak electrolyte, such as acetic acid, in dilute aqueous solution?
HCH3COO + H2O → H3O+ + CH3COO-
What is the equation used to calculate the pH of a buffer solution from a weak acid and its salt?
pH = pKa + log [A-] / [HA]
What is the purpose of the Law of Mass Action in the context of acid-base equilibria?
To determine the dissociation constant of a weak electrolyte
What is the relationship between the primary and secondary dissociation constants of a diprotic acid?
K1 is always greater than K2
What happens to the H+ ions when a strong acid is added to an acetic acid-acetate buffer solution?
They produce an equivalent amount of the relatively weak acid
What is the importance of the relative dissociation constants in understanding the behavior of a buffer solution?
They influence the buffer action of the solution
What is the effect of increasing the dilution of a diprotic acid on the secondary dissociation?
The secondary dissociation increases
What is the significance of the magnitude of the ionization constants in the dissociation of a polyprotic acid?
They measure the extent of ionization at each stage
What is the term used to describe the equilibrium constant of the dissociation of a weak electrolyte?
Dissociation constant
What is the value of pH at the first equivalence point approximately?
4.6
Which indicator is suitable for the secondary stage of phosphoric acid?
Phenolphthalein
What is the value of pH at the second equivalence point approximately?
9.7
Why is direct titration of orthophosphoric acid as a tribasic acid impossible with any indicator?
Because K3 is very small
How can phosphoric acid be titrated indirectly?
By replacing it with an equivalent amount of HCl
What is the value of pH at the third equivalence point approximately?
12.35
Quantitative chemical analysis involves determining the volume of a standard solution required to react with a measured volume of a substance. Learn about the process of titrimetric analysis, also known as volumetric analysis, and how it's used to measure chemical concentrations.
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