Chapter 17 Practice Test - Buffers, Titrations, Ksp

Sep 20, 2026

Uploaded by Mimi

Practice test focused on buffers, titration curves, acid-base calculations, and Ksp/solubility relationships. Covers the common ion effect, buffer formation and selection, changes in pH after adding strong acid or base, and interpreting equivalence points from titration data. Includes multiple-choice problems using equilibrium concepts (Ka, pKa), net ionic reactions, blood buffer system identification, and quantitative Ksp expressions to find ion concentrations, solubility, and least-soluble compounds from Ksp tables.

LanguageEnglish

CategoryExam

FormatPDF

Pages15

Reading Time38 min

AccessFree to download

Target 1: Common ion effect and buffer pH calculations

Common ion effect definition

pH change from adding acid to a conjugate system

Target 2: Buffer preparation and operation

Buffer formation constraints

Best buffer selection

Net ionic reactions with buffers

Primary buffer system in blood

Target 3: Titration curve shapes

Identifying strong/weak acid-base combinations

Using equivalence-point pH to classify titration

Target 4: pH at any point in titrations

Mixing strong acid and base

Equivalence-point pH estimation

Weak acid buffer titration calculations

Target 5: Ksp and solubility

Writing Ksp expressions

Finding ion concentration in saturated solutions

Computing Ksp from solubility

Determining least soluble compound from Ksp

Practice Test Chapter 17Buffers,Titrations,Ksp Part I:Circle the letter of the best annswer(s)No calculators are allowed on the multiplechoice portion of the practice test! Target 1:I can explain the Common lon Effect and make associatedcalculations. 1.The Common lon Effect is defined as a(n).. a.decrease in pH when an acid is added to a buffer solution whichcontains an acid with a greater Ka than the Kb of the conjugate base. b.increase in pH when an acid is added to a buffer solution whichcontains an acid with a greater Ka than the Kp of the conjugate base. c.decrease in the solubility of a strong acid when mixed with a weakbase. d.increase in the percent ionization of either a weak acid or a weak baseupon the addition of a strong electrolyte containing an ion in commonwith the acid or base. shift in equilibrium caused by the addition of a compound having an ionin common with the dissolved substance 2.What change will be caused by addition of a smail amount of HCi to a soiutioncontaining fluoride ions and hydrogen fluoride? a.The concentration of hydronium ions will increase significantly. b.The concentration of fluoride ions will increase as willthe concentrationof hydronium ions. c.The concentration of hydrogen fluoride will decrease and theconcentration of fluoride ions will increase. The concentration of fluoride ion will decrease and the concentration ofhydrogen fluoride will increase. e.The fluoride ions will precipitate out of solution as its acid salt. | Target 2:I can describe how a buffer solution of a particular pH is
made and how it operates to control pH.I can also calculate the
change in pH of a simple buffer solution caused by adding a small
amount of strong acid or base. | | --- | 3.Which one of the following pairs cannot be mixed together to form a buffer solution?Ac STRone BAe a.C5H5N,C5H5NHCI b.HC2H₃O2,NaC2H₃O2 KOH,HI STKoG Ac STRo d.NH3,NH₄CI e.NaCIO,HCIO 4.Which of the following solutions would make the best buffer? a.0.10 M HCl and 0.10 M NaCI b.0.10 M NH₄Cl and 0.10M NaCl c.0.10 M NH₄Cl and 0.10 MHC2H3O2irs CoNt. @0.10 MHF and 0.10 M NaF→WEAL AcioBASE e.None of the above would make very good buffers. 5.The net ionic equation describing the reaction of added NaOH to a buffersolution containing HCO3-and CO32-is a.OH-(aq)+CO₃2-(aq)→HCO₄3-(aq)⑥OH-(aq)+HCO3-(aq)→H₂O()+CO32-(aq) c.2 Na+(aq)+CO₃2-(aq)→Na₂CO3(aq) d.Na+(aq)+HCO3-(aq)→NaHCO3(aq) e.Na+(aq)+H₂O(I)→H+(aq)+NaOH(aq) buffer6.The primary buffer system that controls the pH of blood is the_system. a.carbon dioxide,carbonate b.carbonate,bicarbonate C.carbonic acid,oxygen d.carbonate,carbonic acide carbonic acid,bicarbonate use H² 7.The Ka of benzoic acid is 6.30×10-5.The pH of a buffer prepared bycombining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 Mbenzoic acid is① equahian. a.1.709 b.0.851 c.3.406 4.201e.2.383 componeont of the but Le fr,t=pka!baccG a共moe No we2 a caleulalw! pka(册) s ai44e fes 4an 4Qe abskuke value of Qc efpowemt(0-5. | Target 3:I can describe the shape and key features of titration
curves involving both strong and weak acids and bases. | | --- | 8.An initial pH of 4.00,an equivalence point at pH 9.35,and a moderately short,nearly vertical middle section correspond to a titration curve for a.strong acid titrated by a strong base b.strong base titrated by a strong acidweak acid titrated by a strong base d.weak base titrated by a strong acid e.weak base titrated by a weak acid BASe ADDED 9.A 25.0 mL sample of a solution of an unknown compound is titrated with aok ue lasic sat!due 书1e lwydolysis 0.115M NaOH solution.The titration curve below was obtained.The unknowncompound is.(The pH=8.10 at equivalence point.) a.a strong acid b.a strong basea weak acid d.a weak base e.neither an acid nor a base pH ofsolutionin fiaskmL of0.115 M NaOH added to fiask | T

FAQs

How is Ksp used to find solubility or ion concentrations?

Ksp is written as an expression of the dissolved ions raised to their stoichiometric powers. Using the Ksp value, the test problems compute ion concentrations in saturated solutions and calculate Ksp from given solubility.

Sep 20, 2026

Uploaded by Mimi