Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Selective Precipitation

See all sections
Sections
Buffer
Acid and Base Titration Curves
Weak Acid Strong Base Titrations
Weak Base Strong Acid Titrations
Strong Acid Strong Base Titrations
Titrations of Diprotic and Polyprotic Acids
Ksp
Additional Practice
Equivalence Point
Acid Base Indicators
Selective Precipitation
Formation Constant
Additional Guides
Henderson Hasselbalch Equation
Additional Practice

Solution: A solution contains 0.20 M CrO 4 2- , 0.10 M CO 3 2- , and 0.010 M Cl - . If solid AgNO3 is added slowly to the solution without changing the total volume of the solution, in what order will the preci

Problem

A solution contains 0.20 M CrO 4 2- , 0.10 M CO 3 2- , and 0.010 M Cl - . If solid AgNO3 is added slowly to the solution without changing the total volume of the solution, in what order will the precipitates, Ag2CrO4, Ag2CO3, and AgCl, form?

a. 1st: Ag2CO3        2nd: Ag 2CrO4         3rd: AgCl

b. 1st: Ag2CrO4       2nd: Ag 2CO3          3rd: AgCl

c. 1st: AgCl              2nd: Ag 2CrO4         3rd: Ag 2CO3

d. 1st: AgCl              2nd: Ag  2CO3          3rd: Ag 2CrO4

e. 1st: Ag2CO3        2nd: AgCl               3rd: Ag  2CrO4

Next
Practice Problems
A solution contains 0.015 M Ba2+ and 0.015 Ag+ . N...
Consider a solution containing the group III catio...
Consider the following Ksp values for metal sulfid...
Ksp = 6.3 x 10-5 for the following hypothetical eq...
For BaCrO4 (Ksp = 1.17 × 10–10), will a precipitat...
When equal volumes of each solution are mixed, whi...
Ksp for CaF2 is 3.9 × 10−11. Would a precipitate o...
A solution containing AgNO3 is mixed with a soluti...
A solution contains 0.021 M Cl- and 0.017 M I -. A...
Will a precipitate form when 10 mL of 0.015 M [Hg ...
Give the equation for an unsaturated solution in c...
Will a precipitate form when 10 mL of 0.015 M [Hg ...
Solutions of 0.00024 M aqueous sodium iodide and 0...
What will be the result if 100 mL of 0.06 M Mg(NO ...
A solution contains 0.20 M CrO 4 2- , 0.10 M CO 3 ...
Selective precipitation. In this example Cu2+ i...
Predict whether or not a precipitate will form upo...
Potassium hydroxide is used to precipitate each of...
Potassium hydroxide is used to precipitate each of...
If a precipitate forms when HCl is added to an aqu...
Consider a solution that is 2.3×10−2 M in Fe2 + ...
Consider a solution that is 2.3×10−2 M in Fe2 + ...
Calculate the concentration of I- in a solution ob...
What volume of 0.116 M sodium carbonate solution ...
For a given solution containing an ionic compound,...
What is selective precipitation? What are the cond...
Will Ca(OH)2 precipitate from solution if the pH ...
Fluoridation of drinking water is employed in many...
Calculate the minimum pH needed to precipitate Mn(...
Give the equation for a saturated solution in comp...
What is the value of Q when the solution contains ...
Consider the relative saturation of a solution. If...
A solution is 5.0 x 10-5 M in each of these ions: ...
Consider the solubility of lead (II) chloride, Th...
Which of the following compounds precipitates from...
A 1.0 M Na2SO4 solution is slowly added to 10.0 mL...
Calculate the concentration of Tl+ when TlCl just ...
Calculate the concentration of sulfate ion when Ba...
Calculate the concentration of Sr2+ when SrF2 star...
Calculate the concentration of PO43− when Ag3PO4 s...
Calculate the concentration of F– required to begi...
A solution containing sodium fluoride is mixed wit...
Calculate the concentration of Ag+ required to beg...
A solution containing potassium bromide is mixed w...
The concentration of Mg2+ in seawater is 0.052 M. ...
Potassium hydroxide is used to precipitate each of...
What [Ag+] is required to reduce [CO32−] to 8.2 × ...
A solution of 0.075 M CoBr2 is saturated with H2S ...
What [F–] is required to reduce [Ca2+] to 1.0 × 10...
A 0.125-M solution of Mn(NO3)2 is saturated with H...
Determine the minimum concentration of the precipi...
Will a precipitate form when 100.0 mL of 4.0 X 10 ...
Determine the minimum concentration of the precipi...
A volume of 0.800 L of a 2 × 10–4-M Ba(NO3)2 solut...
Determine the minimum concentration of the precipi...
To a 0.10-M solution of Pb(NO3)2 is added enough H...
Consider a solution that is 1.3×10−2 M in Ba2+ and...
To a 0.10-M solution of Pb(NO3)2 is added enough H...
Consider a solution that is 1.3×10−2 M in Ba2+ and...
Consider a solution that is 1.3×10−2 M in Ba2+ and...
Consider a solution that is 2.3×10−2 M in Fe2+ and...
A solution contains 1.0 X 10 -5 M Ag+ and 2.0 X 10...
What mass of NaCN must be added to 1 L of 0.010 M ...
Iron concentrations greater than 5.4 × 10–6 M in w...
A solution is prepared by mixing 100.0 mL of 1.0 X...
A solution is 0.010 M in both Cu2+ and Cd2+. What ...
A solution is 0.15 M in both Pb2+ and Ag+. If Cl– ...
A solution contains 2.0 X 10 -3 M Ce3+ and 1.0 X 1...
The following question is taken from a Chemistry A...
Predict whether or not a precipitate forms upon mi...
You have an aqueous solution of chromium(III) nitr...
Under what conditions does an ionic compound preci...
Gout-a condition that results in joint swelling an...
Pseudogout, a condition with symptoms similar to t...
A solution contains 1.0 X 10 -5 M Na 3PO4. What is...
A volume of 50 mL of 1.8 M NH3 is mixed with an eq...
An insoluble salt MX has a Ksp of 1.0  10-16. Two ...
A solution is 1 X 10 -4 M in NaF, Na 2S, and Na3PO...
A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(...
Describe how you could separate the ion in the fol...
Describe how you could separate the ion in the fol...
A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to...
The calcium ions in human blood serum are necessar...
Describe how you could separate the ion in the fol...
Does any solid Cu(OH)2 form when 0.075 g of KOH is...
Does any solid PbCl2 form when 3.5 mg of NaCl is d...
Does any solid Ba(IO3)2 form when 7.5 mg of BaCl2 ...
Does any solid Ag2CrO4 form when 2.7×10−5 g of AgN...
Magnesium metal (a component of alloys used in air...
Hydrogen sulfide is bubbled into a solution that i...
A solution containing lead(II) nitrate is mixed wi...
A solution containing lead(II) nitrate is mixed wi...
A solution is 0.025 M in Pb2+. What minimum concen...
The magnesium and calcium ions present in seawater...
What mass of Ca(NO3)2 must be added to 1.0 L of a ...
A solution is 0.085 M in Pb2+ and 0.025 M in Ag+. ...
A solution is 0.085 M in Pb2+ and 0.025 M in Ag+. ...
Which of the following compounds precipitates from...
Ammonium chloride, NH4Cl, is a very soluble salt i...
A solution contains 2.1×10−4 M  Ag+ and 1.6×10−3 M...
Sodium sulfate is slowly added to a solution conta...When 12.0 mL of a 6.38 x 10^-4 M manganese (II) su...When 18.0 ml of a 2.19 x10-4 M lead acetate soluti...A solution is 5.0 x 10-5 M in each of these ions: ...