Chapter 17

Pataasin ang iyong marka sa homework at exams ngayon gamit ang Quizwiz!

Select the statements that correctly describe how to calculate the pH at various points during the titration of a weak acid against a strong base.

-All the equivalence point the pH calculation is based on the reaction of the conjugate base A- with H2O -The initial [H3O+] is calculated from [HA] and Ka.

Which of the following options correctly describe how to calculate the pH at various stages during the titration of a strong acid against a strong base?

-At the equivalence point pH=7.00 -Initial pH=-log[HA]

Which of the following statements correctly describe a strong acid- weak base titration curve?

-Before the equivalence point is reached, the weak base and its conjugate acid are both present in solution. -The pH at the equivalence point its < 7.00

What factors exist the solubility of ionic compounds?

-Common ion effect - pH - Formation of complex

Which of the following quantities must be known in order to calculate the pH of an acid-base buffer solution using the Henderson-Hasselbalch equation?

-Ka of weak acid or Kb of weak base -Concentration of conjugate base - Concentration of weak base

Which of the following combinations could be used in an acid- base buffer system?

-NH3/ NH4Cl -HNO2/ KNO2 -CH3COOH/ NaCH3COO-

Why does the equivalence point for a weak base- strong acid titration occur at a pH < 7.00?

-The conjugate acid of the weak base reacts with H2O to give a solution with pH < 7.00

Which of the following statements correctly describe the titration curve for the titration of a strong acid with a strong base?

-The pH rise is very steep close to the equivalence point of the titration. -the equivalence point is at a pH of 7.00

When comparing the titration curve for a weak acid- strong base titration and a strong acid- strong base titration the following differences are found.

-the curve for the weak acid- strong base titration rises gradually before the steep rise to the equivalence point. -the pH at the equivalence point is about 7.00 for the weak acid- strong base titration.

In order for a solution of a weak acid and its conjugate base to be considered a buffer, the ratio of base concentration to acid concentration must be within the range _______________

0.1 < [base]/[acid] < 10

_____________ is the number of grams of solute in 1 L of a saturated solution (mol/L)

Molar solubility

______________ involves the principle of selective precipitation and can be used to identify the types of ions present in a solution.

Qualitative analysis

____________ is the number of grams of solute in 1 L of a saturated solution (g/L)

Solubility

For a weak acid that has dissolved in water, the ionization equilibrium will shift toward the reactants if a quantity of the conjugate base is added to the solution. this is known as the _______________________

common ion effect

The __________________ of a titration is the point at which the color of the indicator changes.

endpoint

Compared to a strong acid- strong base titration, the curve for a weak acid- strong base titration begins at a ___________ pH, and has a ____________ vertical section as the equivalence point is reached.

higher, smaller

When a strong acid or base is added to a buffer system there is a __________ change in the [HA]/[A] ratio and thus a ___________ change in pH.

smaller, smaller

An indicator is a(n) ________________ organic acid that has a different color than its ___________ base. Each indicator changes color over a specific ____ range.

weak, conjugate, pH


Kaugnay na mga set ng pag-aaral

NAQT - You Gotta Know: Geography

View Set

ABC 3.1 Electrical (408 - Switchboards and Panelboards)

View Set

MKTG473 Ch. 15: Marketing Cost and Profitability Analysis

View Set