If we have a solution that contains 0.022 M Calcium and 0.014 M Magnesium and we have to use...
Question:
If we have a solution that contains 0.022 M Calcium and 0.014 M Magnesium and we have to use potassium hydroxide to selectively precipitate one of the ions, while leaving the other ion in the solution.
A) Which metal will precipitate first? ( this metal will be referred to as " first ion")
B) What minimum concentration of KOH is necessary to begin precipitation of "first ion"?
C) What molarity of "first ion" remains in solution at the point when the second ion begins to precipitate?
D) As we set up the second trial for this same experiment, we realized that we ran out of potassium hydroxide. All we have in the storage cabinet is potassium carbonate. Would this be a good titrant to use for the selective precipitation? Why or why not? (Ksp of Mg(OH){eq}_2 {/eq} = 6.3 x 10{eq}^{-10} {/eq}, Ksp of Ca(OH){eq}_2 {/eq} = 6.5 x 10{eq}^{-6} {/eq})
Selective Precipitation:
The process by which any specific reagent would precipitate a given ion among a mixture of ions in an aqueous solution based on their solubility product is known as the selective precipitation of ions.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerGiven Data
{eq}{\rm K_{sp}}\; {/eq} of {eq}\;\rm Mg{\left( {\rm OH} \right)_2} {/eq} = {eq}6.3 \times {10^{ - 10}} {/eq}
{eq}{\rm...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
The Common Ion Effect and Selective Precipitation
from
Chapter 11 / Lesson 6
79K
Learn about the common ion effect on solubility. Learn what a common ion is, examine a common ion chart, and work through examples of the common ion effect.
Related to this Question
- Solutions of lead acetate, calcium nitrate, and magnesium chloride are mixed. The resulting solution is 0.055 M in Pb(C2H3O2)2, 0.015 M in Ca(NO3)2, and 0.035 M in MgCl2. Will a precipitate form in the mixed solution? If so, identify the precipitate.
- A solution is 0.022 M in Fe^{2+} and 0.014 M in Mg^{2+}. a. If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? What minimum concentration of K_2CO_3
- Consider a solution that is 2.3 x 10-2 M in Fe2+ and 2.0 x 10-2 M in Mg2+. a. If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? b. What minimum con
- A solution of lead acetate, calcium nitrate, and magnesium chloride are mixed. The resulting solution is 0.055 M in Pb(C_2H_3O_2)_2, 0.015 M in Ca(NO_3)_2 and 0.035 M in MgCl_2. Will a precipitate form in the mixed solution? If so, identify the precipitat
- A solution contains 0.50 M lead ions, P b 2 + , and 0.00010 M zinc ions, Z n 2 + . If solid N a 2 S is slowly added to the solution, which salt precipitates first, P b S or Z n S ? What is the concentration of the first ion that precipitates when t
- Consider a solution that is 2.5 * 10^-2 M in Fe2+and 1.3 * 10^-2 M in Mg2+. A. If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution,
- A solution contains an unknown mass of dissolved silver ions. When potassium chloride is added to the solution, a white precipitate forms. The precipitate is filtered and dried and then found to have
- You are given two unlabelled colorless solutions: AgNO3(aq) and Ca(NO3)2. Which ion when added to each unlabelled solution would produce a precipitate with the calcium and silver ions?
- A solution contains one or more of the following ions: Hg2^2+, Ba^2+, and Fe^2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no
- A solution contains one or more of the following ions: Hg22+, Ba2+, and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no pre
- A solution contains the following ions: Hg22+ and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the rem
- A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO3)_2. Will a precipitate form in the mixed solution? If so, identify the precipitate. Express your answer as a
- A solution contains 8.50 x 10^{-3} M lead acetate and 1.20 x 10^{-2} M magnesium nitrate. Solid sodium hydroxide is added slowly to this mixture. What is the concentration of lead ion when magnesium ion begins to precipitate? (Pb^{2+})
- A solution contains one or more of the following ions: Hg^2+, Ba^2+, and Fe^2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no p
- A solution contains 0.25 M Ni(NO_3) and 0.25 M Cu(NO_3)_2. Can metal ions be separated by slowly adding Na_2CO_3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begin to precipitate, and assume t
- A solution contains one of more of the following ions: Hg_2^2+, Ba^2+, Fe^2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no pre
- A precipitate will be formed when an aqueous carbonic acid solution is added to what other aqueous solution? A. Ammonium chloride B. Calcium hydroxide C. Sodium Chloride D. Potassium carbonate
- A solution contains 0.20 M Cl^- and 0.20 M SO_4^{2-}. a) Identify a cation that could be added to the solution to give a precipitate with only one of these anions. b) Write the net ionic equation
- Base is added to a solution containing Ca+2, Na+, and K+ and a precipitate forms. What is the chemical formula of the precipitate?
- What precipitate will form when aqueous solutions of sodium carbonate (Na2CO3) and calcium chloride (CaCl2) are mixed? a) NaCl(s) b) CaCO3(s) c) CaCl2(s) d) Na2CO3(s)
- A precipitate is expected when an aqueous solution of potassium iodide is added to an aqueous solution of \\ A. calcium nitrate B. barium hydroxide C. lead perchlorate D. Iron(ll) chloride E. Sodium sulfate
- A solution contains 0.01 M Ba^2+ and 0.01 M Ag^+. Can 99.92% of either ion be precipitated by chromate (CrO_4^2-) without precipitating the other metal ion? The K_sp for BaCrO_4 is 2.1 times 10^-10 and K_sp for Ag_2CrO_4 is 1.2 times 10^-12.
- A solution contains Ag^+ and Hg^2+ ions. The addition of 0.100 L of 1.10 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 25.6 g. Find the mass of AgI in the precipitate.
- An aqueous solution of calcium nitrate is allowed to react with an aqueous solution of potassium carbonate. The net ionic equation contains which of the following species? (a) 2 K ( a q ) (b) C a 3 + ( a q ) (c) 2 N O 3 ( a q ) (d) 2 C a 3 + (e
- An aqueous sample is known to contain Pb2+, Cu2+, or Na+ ions. Treatment of the sample with both NaOH and LiCl solution produces a precipitate. a. Which of the metal cations does the solution contain? Explain your reasoning. b. Write all net ionic equatio
- A solution is 0.020 M in Pb2+ and 0.020 M in Ag+. As Cl- is introduced to the solution by the addition of solid NaCl, determine (a) which substance will precipitate first, AgCl or PbCl2, and (b) the fraction of the metal ion in the first precipitate that
- What precipitate will form when aqueous solutions of sodium carbonate and calcium chloride are mixed?
- A solution contains 0.17 M potassium cyanide and 0.17 M sodium hydroxide. Solid nickel(II) nitrate is added slowly to this mixture. What ionic compound precipitates first from the solution? Solubility
- A solution contains 0.020 M Cu^{2+} and 0.020 M Hg^+. Can 99.90% of either ion be precipitated by chromate (CrO_4^{2-}) without precipitating the other metal ion? K_{sp} for CuCrO_4 = 3.6 times 10^{-6} and K_{sp} for Hg_2CrO_4 = 2.0 times 10^{-9}.
- Does a precipitate form when aqueous solutions of calcium nitrate and sodium chloride are mixed? If so, write the formula of the precipitate.
- If a solution contains 0.01 M Ca^{2+} and 0.01 M Ni^{2+} ions and you want to separate them using aqueous (NH_4)_2C_2O_2 which ion will precipitate firs as an oxalate? CaC_2O_4 or NiC_2O_4? K_{sp} CaSO_4 = 1.3\times10^{-9} K_{sp} NiC_2O_4 = 4\times10^{-10
- A mixture of lead, magnesium, nitrate and chromate ions are present in a solution. What will the precipitate be? A. MgPb B. Pb(NO_3)_2 C. PbCrO_4 D. MgCO_3
- A solution contains one or more of the following ions: Pb2+, Ca2+, and Zn2+. When sodium chloride is added to the solution, a precipitate forms. This precipitate is filtered off and sodium sulfate is added to the solution, but no precipitate forms. When s
- Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCl_2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was added. The precipitate of calcium oxalate, CaC_2O_4, we
- Solid potassium chromate is slowly added to 50.0 mL of a 0.210 M calcium acetate solution until the concentration of chromate ion is 0.0317 M. The mass of calcium ion remaining in solution is _______g
- A solution contains Ag^+ and Hg^2+ ions. The addition of 0.100 L of 1.41 M NaI solution is just enough to precipitate all the ions as AgI and HgI_2. The total mass of the precipitate is 32.6 g. Find the mass of AgI in the precipitate. Express your answer
- A solution contains 0.20 M potassium sulfide and 0.20 M potassium carbonate. Solid nickel(II) nitrate is added slowly to this mixture. What ionic compound precipitates first from the solution? (Hint: It is not necessary to do a calculation, a general ex
- An aqueous solution contains the following ions: Cl-, Ag+, Pb2+, NO3-, and SO42-. More than one precipitate will form. Identify the precipitates.
- Aqueous potassium chloride will react with which of the following aqueous solutions to produce a precipitate? a. calcium nitrate b. sodium bromide c. lead(II) nitrate d. barium nitrate e. sodium chloride
- A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation, 99% of metal ion must be precipitated before the other metal ion begins to precipitate, and assume no
- A solution contains 0.010 M Ba2+ and 0.010 M Ag+. Given that the Ksp for BaCrO4 is 2.1 x 10-10 and the Ksp for Ag2CrO4 is 1.2 x 10-12, can 99.91% of either ion be precipitated by chromate (CrO42-) without precipitating the other metal ion?
- A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.44 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 33.3 g. Find the
- An aqueous solution is analyzed and found to contain potassium ions and sulfate ions. Write the equation for the dissolution of the salt that produced this solution. If the solution contains 0.600 mol
- A solution contains both Ca^2+ and Ba^2+, each present at a concentration of 0.0100 M. We wish to remove the calcium ion from solution, while leaving the barium ions essentially untouched (still dissolved) by adding solid NaF. What concentration of F- is
- Does a precipitate form when aqueous solutions of potassium hydroxide and magnesium bromide are mixed? If so, write the empirical formula of the precipitate.
- A solution contains Ag+, Pb2+, and Hg22+. A white precipitate forms on the addition of 6 M HCI. The precipitate is partially soluble in hot water, and the remaining precipitate dissolves completely in aqueous ammonia. Which of the ions are present, which
- A solution contains 1 x 10^{-3} M Li+ and 1 x 10^{-3} M Ba^{2+}. Is it possible to precipitate one of the ions while maintaining the other in solution using F^- as the precipitating agent? Assume 1 x 10^{-6} M as the concentration for complete removal of
- Assume you had a solution that contained a mixture of silver ions and strontium ions. Come up with three different reaction plans that would allow you to precipitate either the silver ion or strontium ion, but the other ion would remain in solution.
- An aqueous sodium hydroxide solution mixed with an aqueous magnesium nitrate solution yields which of the following products? a) magnesium hydroxide(aq). b) magnesium dihydroxide(s). c) magnesium hydroxide(s). d) dimagnesium hydroxide(s). e) sodium nitrat
- A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO_3)_2. Will a precipitate form in the mixed solution? I
- If I have a solution of lithium chloride, with which of the following solutions could I mix it to get a precipitate? A. iron(III) bromide B. magnesium nitrate C. lead (II) acetate D. potassium iodide E. none of the above
- A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 Min KBr and 0.0035 M in Pb(C_2H_3O_2)_2. Does a precipitate form in the mixed solution? If so, identify the precipitate.
- A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C_2H_3O_2). Will a precipitate form in the mixed solution? If so, identify the precipitate. Express your an
- A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C_2H_3O_2)_2. Will a precipitate form in the mixed solution? If so, identify the precipitate.
- A solution of magnesium chloride is mixed with a solution of sodium hydroxide. Predict any precipitates that are formed.
- A solution contains 0.46 M P b ( N O 3 ) 2 and 0.1 M A g N O 3 . As solid K I is slowly added to the solution, one of the metal iodides begins to precipitate. What is the concentration of A g + remaining in solution when the second metal iodide beg
- Consider a solution that is 0.022 M in F e^2+ and 0.014 in Mg^2+ . a) If K_2CO_3 is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation wi
- Aqueous solutions of iron(III) chloride and sodium hydroxide are mixed together to form a combined solution that is 0.015 M FeCl3 and 0.010 M NaOH. a. Determine whether a precipitate forms in this solution. If so, what will be the precipitate? b. Would th
- A solution contains the metal ions listed below, all at the same concentration. The addition of thioacetamide, CH3CSNH2, produces sulfide ion, S2-, causing the ions to precipitate as the sulfides. Each sulfide begins to precipitate at a different concentr
- What is the precipitate of calcium nitrate, Ca(NO3)2, and sodium chloride, NaCl? Sodium nitrate and calcium chloride are both soluble in water.
- A solution contains Ba2+(aq) and Ca2+(aq), both in concentrations of 0.0010 M. A solution of Na3PO4(aq) is then added very slowly dropwise. Which solid will precipitate first? By the time the SECOND precipitate forms, how much of the first cation (which p
- Suggest a procedure that can be used to precipitate Ba+2(aq) and Pb+2(aq) separately from a solution that contains both ions. Include net ionic equations for each step.
- An aqueous solution of calcium nitrate is allowed to react with an aqueous solution of potassium carbonate. The net ionic equation would contain which of the following species? a) \ 2 Ca^{2+} (aq) \\ b) \ 2NO^{3-}(aq) \\ c) \ Ca^{2+}(aq) \\ d) \ NO^{3-}
- A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C2H3O2)2. Will a precipitate form in the mixed solution? If so, identify the precipitate.
- When aqueous solutions of iron (III) sulfate, (Fe_2(SO_4)_3) and sodium hydroxide were mixed, a precipitate is formed. What is the precipitate?
- Does a precipitate form when aqueous solutions of sodium hydroxide and potassium chloride are mixed? If so, write the formula.
- A solution contains I^-, \space Br^- \space and \space OH^- ions. If Ag^+ is added, what will the precipitate (s) be?
- A solution contains an unknown amount of dissolved magnesium. Addition of 0.0877 mol of Na_2CO_3 causes complete precipitation of all of the magnesium. What mass of magnesium was dissolved in the solution?
- If a solution is 4.3x10-4 M in magnesium nitrate, Mg(NO3)2, and 5.2x10-2 M in aqueous ammonia, NH3, will Mg(OH)2 precipitate? (Ksp =1.5x10-11 for Mg(OH)2, Kb =1.8x10-5 for NH3)
- When a precipitate reaction occurs, the ions that do not form the precipitate _____ (a) Are left dissolved in solution (b) Are cation only (c) Are called ions (d) Evaporate (e) Both a and c
- A solution contains the sodium salt of an anion. The following tests are performed to identify the anion. (a) The solution is treated with silver nitrate solution. A white precipitate forms. List all
- Will a precipitate form when aqueous solutions of sodium chloride and potassium hydroxide are mixed? If so, write the formula of the precipitate.
- A solution contains one or more of the following ions: Ag^+, Ca^{2+}, and Cu^{2+}. When sodium chloride is added to the solution, no precipitate occurs. When sodium sulfate is added to the solution, a white precipitate occurs. The precipitate is filtered
- Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO_3)_3? 1. KNO_3. 2. KCl. 3. K_2SO_4. 4. KOH.
- A solution contains one or more of the following ions: Ag+, Ca2+, and/or Cu2+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off an
- A solution contains 1.41 x 10-2 M potassium sulfite and 1.50 x 10-2 M sodium chromate. Solid silver nitrate is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of silver ion when t
- If HBr was added to a solution containing lead(II) ions, sodium ions, nickel(II) ions, and potassium ions, which ions would precipitate? Explain.
- A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a. At what concentration of F^- does precipitate start to form? b. When (F^-) = 9.5 times 10^-4
- When 1.0 mole of solid lead nitrate is added to 2.0 moles of aqueous potassium iodide, a yellow precipitate forms. After the precipitate settles to the bottom, does the solution above the precipitate conduct electricity?
- A solution contains 1.25 x 10-2 M sodium sulfate and 8.50 x 10-3 M potassium fluoride. Solid barium nitrate is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of barium ion when t
- When 12.0 mL of a 9.64 x 10-4 M potassium sulfate solution is combined with 15.0 mL of a 3.92 x 10-4 M calcium iodide solution, does a precipitate form?
- A solution is 0.010 M in both Br^- and SO_4. A 0.250 M solution of lead (II) nitrate is slowly added to it. The K_{sp} for PbSO_4 is 1.8 \times 10^{-8}. The K_{sp} for PbBr_2 is 6.0 \times 10^{-6}. \\ A. Which anion will precipitate first? B. What is th
- A solution containing potassium bromide is mixed with one containing lead (II) acetate to form a solution that is 0.013 M KBr and 0.0035 M in Pb(C_2H_3O_2)_2. Does a precipitate form in the mixed solu
- When solution of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation. 2AgNO_2(aq) + CaCl_2(aq) --> 2AgCl(s) + Ca(NO_2)_2 (aq) Part A
- What precipitate is likely to form when aqueous solutions of potassium sulfate (K2SO4) and calcium acetate (Ca(C2H3O2)2) are mixed, according to the general solubility rules? If it is unlikely that a precipitate will form, indicate which solubility rules
- Silver nitrate solution reacts with calcium chloride solution according to the equation 2AgNO_3 (aq) + CaCI_2 (aq) --> Ca(NO_3)_2 (aq) + 2AgCI (s) If a solution containing 6.30 g of AgNO_3 is mixed
- Of the metals below, which of the following will not dissolve in an aqueous solution containing nickel ions? A) Aluminum B) Chromium C) Barium D) Tin E) Potassium
- If the solution becomes ......................., it contains a precipitate.
- If an aqueous solution of ............ is added to a mixture of Pb^2+ and ba^2+, the lead ion will precipitate. but the barium ion will remain in solution. a. NaOH b. Na_2SO_4 c. K_3PO_4 d. KCO_3
- When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation: 2AgNO_3(aq) + CaCl_2(aq) => 2AgCl(s) + Ca(NO_3)_2(aq).
- When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO_3(aq) + CaCl_2(aq) ? 2AgCl(s) + Ca(NO_3)_2 (aq) Part A W
- Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO_3)_3? 1. KOH. 2. KCl. 3. K_2SO_4. 4. KNO_3.
- Does a precipitate form when aqueous solutions of barium chloride and sodium carbonate are mixed? If so, write the formula of the precipitate.
- A solution contains one or more of the following ions: silver, barium, and Copper (II). A student adds sodium chloride to a small sample of the solution of the unknown and a white precipitate is formed. He/she filters out the precipitate and then add sodi
- A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered, dried, and found to have a mass of 258 mg. What mass of barium was in the original solution
- Hard water often contains dissolved Ca^{2+} and Mg^{2+} ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from the solution. A solution is 0.050 M in calcium c
- A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered and dried and found to have a mass of
- Does a precipitate form when aqueous solutions of hydrochloric acid and sodium sulfide are mixed? If so, write the formula of the precipitate.
- A solution is 5.0 * 10^-5 M in each of these ions: Ag+, SO4 2-, Cl-, CO3 2-. which precipitate will form ? A) Ag2SO4 (Ksp = 1.12 * 10^^-5) B) AgCl (Ksp = 1.77 x 10^-10) C) Ag2CO3 (Ksp = 8.46 * 10^-1
- A beaker contains a solution that is 0.50 M in Au^{3+} ion and 0.25 M in Ag^+ ion. A solution of sodium chloride is slowly dripped into the beaker with stirring. Which ion will precipitate first, the
Explore our homework questions and answers library
Browse
by subject