A solution contains 1.36 times 10^{-2} M lead nitrate and 8.64 times 10^{-3} M silver acetate....
Question:
A solution contains {eq}\displaystyle \rm 1.36 \times 10^{-2} \ M {/eq} lead nitrate and {eq}\displaystyle \rm 8.64 \times 10^{-3} \ M {/eq} silver acetate. Solid ammonium chromate is added slowly to this mixture. What is the concentration of chromate ion when this precipitation first begins?
Solubility Product:
It can be evaluated from the product of the molar concentrations of the charged species present in the solution at an equilibrium state. It is expressed by an equilibrium constant for a substance dissolved in a liquid.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerGiven data:
{eq}\left[ {{\rm{Pb}}{{\left( {{\rm{N}}{{\rm{O}}_{\rm{3}}}} \right)}_{\rm{2}}}} \right] = 1.36 \times {10^{ - 2}}\;{\rm{M}} {/eq}
Calcu...
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
Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations
from
Chapter 11 / Lesson 5
17K
Learn about solubility product constant. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp.
Related to this Question
- A solution contains 1.23 x 10-2 M silver nitrate and 1.07 x 10-2 M lead acetate. Solid ammonium chloride is added slowly to this mixture. What is the concentration of silver ion when lead ion begins to precipitate?
- A solution contains 5.72 * 10^{-3} M manganese(II) nitrate and 6.51 * 10^{-3} M lead acetate. Solid ammonium carbonate is added slowly to this mixture. What is the concentration of lead ion when manganese(II) ion begins to precipitate?
- A solution contains 1.36 times 10^{-2} M lead nitrate and 8.64 times 10^{-3} M silver acetate. Solid ammonium chromate is added slowly to this mixture. What is the formula of the substance that precipitates first?
- A solution contains 1.04 \times 10^{-2} M sodium chromate and 1.11 \times 10^{-2} M ammonium phosphate. Solid lead nitrate is added slowly to this mixture. What is the concentration of phosphate ion when chromate ion begins to precipitate?
- A solution contains 1.20 times 10^{-2} M zinc acetate and 1.15 times 10^{-2} M nickel(II) nitrate. Solid potassium cyanide is added slowly to this mixture. What is the concentration of nickel ion when zinc ion begins to precipitate?
- A solution contains 1.32 \times 10^{-2} M barium acetate and 5.72 \times 10^{-3} M lead nitrate. Solid potassium sulfate is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of sul
- A solution contains 9.50�10-3 M silver nitrate and 1.13 * 10-2 M lead acetate. Solid potassium chloride is added slowly to this mixture. What is the concentration of silver ion when lead ion begins t
- 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 1.24 * 10^{-2} M sodium phosphate and 6.69 * 10^{-3} M sodium chromate. Solid barium acetate is added slowly to this mixture. What is the concentration of phosphate ion when chromate ion begins to precipitate?
- A solution contains 7.00 x10-3 M potassium hydroxide and 1.05 x10-2 M ammonium sulfide. Solid iron(II) acetate is added slowly to this mixture. What is the concentration of sulfide ion when hydroxide ion begins to precipitate?
- A solution contains 5.94 x 10-3 M lead nitrate and 1.27 x 10-2 M silver acetate. Solid ammonium bromide is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of bromide ion when this
- A solution contains 1.04 x 10-2 M silver acetate and 1.21 x 10-2 M barium nitrate. Solid ammonium sulfate is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of sulfate ion when th
- A solution contains 6.81 x 10^{-3} M barium nitrate and 1.30 x 10^{-2} M silver acetate. Solid ammonium sulfate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? B. What is the concentration of sulfate ion
- A solution contains 7.70 x 10-3 M ammonium phosphate and 7.51 x 10-3 M potassium hydroxide. Solid chromium(III) acetate is added slowly to this mixture. What is the concentration of hydroxide ion when phosphate ion begins to precipitate?
- A solution contains 8.65 x 10-3 M silver acetate and 9.83 x 10-3 M chromium(III) nitrate. Solid sodium hydroxide is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of hydroxide io
- 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
- A solution contains 9.10 * 10^{-3} M potassium hydroxide and 1.41 * 10^{-2} M potassium cyanide. Solid zinc acetate is added slowly to this mixture. What is the concentration of hydroxide ion when cyanide ion begins to precipitate?
- A 0.00037 M solution of silver nitrate, AgNO3, is slowly titrated with a dilute sodium iodide solution, NaI(aq). At what iodide ion concentration, [ I - ], will precipitation of AgI first begin? Note:
- 1. A solution contains 7.65 x 10^-3 M ammonium carbonate and 1.21x 10^-2 M potassium hydroxide. Solid copper(II) nitrate is added slowly to this mixture. What is the concentration of hydroxide ion whe
- 1. Solid silver acetate is slowly added to 175 mL of a 0.0390 M ammonium sulfite solution. The concentration of silver ion required to just initiate precipitation is ..... M. 2. Solid barium nitrate
- Silver nitrate (AgNO3) is added to a solution of 0.020 M sodium carbonate. At what concentration of AgNO3 does a precipitate start to form?
- A solution containing 0.1 M Pb(NO3)2 and 0.1 M AgNO3 has solid NaI added to it until one of the compounds is about to precipitate. Which compound will precipitate first, and what is the concentration of I^- ions when this occurs?
- What must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO_4, from a solution that is 0.0034 M Sr^2+?
- What is the silver ion concentration in a solution prepared by mixing 357 mL of 0.374 M silver nitrate with 473 mL of 0.413 M sodium chromate? The Ksp of silver chromate is 1.2 x 10-12.
- What is the silver ion concentration in a solution prepared by mixing 385 mL of 0.380 M silver nitrate with 467 mL of 0.409 M sodium chromate? The Ksp of silver chromate is 1.2 x 10-12.
- What is the silver ion concentration in a solution prepared by mixing 379 mL of 0.372 M silver nitrate with 415 mL of 0.527 M sodium chromate? The Ksp of silver chromate is 1.2 x 10-12.
- What is the silver ion concentration in a solution prepared by mixing 469 mL of 0.373 M silver nitrate with 393 mL of 0.591 M sodium chromate? The Ksp of silver chromate is 1.2 x 10-12.
- If 0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO_3 and 0.50 M Ba(NO_3)_2. What is the Ag^+ concentration when BaCrO_4 just starts to precipitate? The K_{SP} for Ag_2Cr
- Strontium chromate (K_{sp}=3.6 times 10^{-5}) can be prepared by mixing solutions containing strontium ions and chromate ions, where the concentrations are high enough to precipitate. Explain whether a precipitate will form when initial concentrations are
- A solution contains 0.0150 M lead(II) ion. A concentrated sodium iodide solution is added dropwise to precipitate lead iodide (assume no volume change). a. At what concentration of I^- does precipitate start to form? b. When (I^-) = 2.0 times 10^-3 M, wha
- 0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO_3 and 0.50 M Ba(NO_3)_2. What is the Ag^+ concentration when BaCrO_4 just starts to precipitate? The K_{SP} for Ag_2CrO_4
- Silver nitrate (AgNO_3) is added to a solution of 0.060 M sodium carbonate. At what concentration of AgNO_3 does a precipitate start to form?
- The silver-ion concentration in a saturated solution of silver(I) chromate is 1.3 X 10-4M. What is Ksp for silver(I) chromate?
- A solution contains 2.24 \times10-2 M zinc acetate and 2.24\times10-2 M nickel(II) nitrate. Solid sodium cyanide is added slowly to this mixture. What is the concentration of nickel ion when zinc ion
- ew A solution contains 1.26 10 2 M lead nitrate and 5.74 10 3 M zinc acetate. Solid potassium sulfide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? B. What is the concentration of sulfide
- The silver-ion concentration in a saturated solution of silver(I) chromate is 1.3 times 10^{-4} M. What is K_{sp} for silver(I) chromate?
- A solution contains 8.10 10 3 M potassium sulfide and 9.92 10 3 M sodium hydroxide. Solid iron (III) nitrate is added slowly to this mixture A. What is the formula of the substance that precipitates first? B. What is the concentration of iro
- If iron(III) acetate is added to be 1 times 10^{-10} M in a solution that is 0.10 M NH_3, what is Q_{sp} and will Fe(OH)_3 precipitate? The K_{sp} of Fe(OH)_3 is 4 times 10^{-38} and K_b for NH_3 is 1.8 times 10^{-5}.
- The addition of sodium hydroxide solution to a solution containing three solutes- lead nitrate, ammonium nitrate, and silver nitrate- will cause formation of what precipitate?
- Silver chromate is sparingly soluble in aqueous solutions. The K_sp of Ag_2CrO_4 is 1.12 times 10^-12. What is the solubility (in mol/L) of silver chromate (a) in 1.30 M potassium chromate aqueous solution? (b) in 1.30 M silver nitrate aqueous solution? (
- 1.00 M solutions of silver nitrate, ammonium chlorate, and sodium acetate are mixed together. Which precipitate is formed?
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12 x 10-12. What is the solubility (in mol/L) of silver chromate in a 1.50 M silver nitrate aqueous solution?
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12 x 10-12. What is the solubility (in mol/L) of silver chromate in a 1.00 M silver nitrate aqueous solution?
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12 x 10-12. What is the solubility (mol/L) of silver chromate in a 1.10 M silver nitrate aqueous solution?
- A solution contains 0.144 M sodium fluoride and 0.111 M sodium bromide. Lead nitrate is added to this solution until precipitation occurs. a) Which salt, lead bromide or lead fluoride, will precipitate out first? b) At what concentration of lead nitrate w
- Strontium chromate (K_{sp}=3.6 times 10^{-5}) can be prepared by mixing solutions containing strontium ions and chromate ions, where the concentrations are high enough to precipitate. Calculate the molar solubility of Mg(OH)_2 in a solution with pH=12.20.
- Does a precipitate form when aqueous solutions of lead(II) nitrate and potassium chromate are mixed? If so, write the formula of the precipitate.
- A solution contains .10 M Cl- and .10 M Br-. If Ag+ is added until AgCl just begins to precipitate, what are the concentrations of Ag+ and Br-? ( Ksp for AgCl=1.8x10^-10, Ksp for AgBr= 3.3x10^-13)
- 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 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
- A saturated solution of silver chromate was found to have a CrO4^2- ion concentration of 3.2 x 10^-4 M at 25 degrees C. What is the Ksp for silver chromate?
- Solid silver acetate is slowly added to 75.0 mL of a 0.0525 M potassium phosphate solution. What concentration of silver ion is required to just initiate precipitation?
- 400 mL of 0.5875 M aqueous silver nitrate are mixed with 500 mL of 0.290 M sodium chromate. a) What is the mass of the precipitate? b) What is the concentration of each of the ions remaining in solution? Indicate any assumptions or approximations.
- Strontium chromate (K_{sp}=3.6 times 10^{-5}) can be prepared by mixing solutions containing strontium ions and chromate ions, where the concentrations are high enough to precipitate. Explain whether a precipitate will form when 275 mL of 6.0 times 10^{-3
- When aqueous solutions of silver nitrate (AgNO3) and potassium chromate (K2CrO3) are mixed, the blood-red precipitate silver chromate Ag2CrO3 is formed. If 10.0 mL of 0.25 M aqueous silver nitrate is
- Silver chromate is sparingly soluble in aqueous solutions. The K_{SP} of Ag_2CrO_4 is 1.12 times 10^{-12}. What is the solubility (in mol/L) of silver chromate in 1.4 M potassium chromate aqueous solu
- If the concentration of silver in silver chromate (Ag2CrO4) is equal to 1.3 x 10-4, what is the concentration of the chromate ion?
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12 x 10-12. What is the solubility (in mol/L) of silver chromate in a 1.80 M potassium chromate aqueous solution?
- Silver chromate is sparingly soluble in aqueous solutions. The K_sp of Ag_2CrO_4 is 1.2\times 10^-12. What is the solubility (in mol/l) of silver chromate in 1.50 M potassium chromate aqueous solution
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12 x 10-12. What is the solubility (mol/L) of silver chromate in a 1.10 M potassium chromate aqueous solution?
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12 x 10-12. What is the solubility (in mol/L) of silver chromate in a 1.50 M potassium chromate aqueous solution?
- A solution is prepared so that the concentrations of manganese(II) nitrate, zinc(II) nitrate, mercury(II) nitrate, and copper(II) nitrate are all 0.100 M. If the solution is slowly titrated with 0.100 M sodium sulfide, which metal sulfide will precipitate
- Solid lead nitrate is slowly added to 175 mL of a 0.0579 M potassium hydroxide solution. The concentration of lead ion required to just initiate precipitation is___ M.
- Adding 10.0 mL of a dilute solution of zinc nitrate to 246 mL of 2.00 M sodium sulfide produced 0.279 grams of a precipitate. a. What was the concentration of each ion in the original solutions? b. What is the concentration of the sulfide ion in solution
- A solution contains 0.0200 M (aq) and 0.0200 M (aq). If we add (aq), what will be the concentration of (aq) when (s) begins to precipitate?
- At what molar ~[H_3O^+~] will PbS just start to precipitate from a solution consisting of 1.592 \times 10^{-6} M Pb(NO_3)_2 in 0.100 M H_2S (satd)? H_2S is bubbled through the solution to keep its concentration constant. PbS(s) \to Pb_2^+ (aq) + S_2^- (
- An aqueous solution that is 2.10 M in AgNO3 is slowly added from a buret to an aqueous solution that is 1.10 x 10-2 M in Cl- and 0.260 M in I-. When the second ion begins to precipitate, what is the remaining concentration of the first ion?
- What is the I^- concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl^- and 0.015 M I^-?
- Consider the following reaction: 100.0 mL of 2.50 M silver nitrate is mixed with 300.0 mL of 1.10 M sodium chromate. What are the concentrations of sodium ions, nitrate ions, silver ions, and chromate ions left in solution after the reaction is complete?
- Which of the following pairs of 0.1 M aqueous solutions would result in the formation of a precipitate upon mixing? a) lead(II) acetate + potassium hydroxide b) ammonium acetate + cadmium(II) nitrate
- Silver chromate is sparingly soluble in aqueous solutions. The K_sp of Ag_2CrO_4 is 1.12 * 10^-12. What is the solubility (in mol/L) of silver chromate (a) in 1.30 M potassium chromate aqueous soluti
- A chemist performed an experiment in which silver nitrate was used to precipitate all of the chromate ion as silver chromate, Ag2CrO4 from 200 mL of a solution of potassium chromate, K2CrO4. This proc
- A solution is made up by adding 0.839 g of silver(I) nitrate and 1.024 g of lead(II) nitrate to enough water to make 492 mL of solution. Solid sodium chromate, Na2CrO4, is added without changing the volume of the solution. A) Which salt will precipitate f
- You have a solution that contains 1.26 * 10^-2 M of lead nitrate and 5.74 * 10^-3 M of zinc acetate. You add solid potassium sulfide slowly to this mixture. What is the formula of the substance that precipitates first? Additionally, what is the concentrat
- Solid lead acetate is slowly added to 75.0 mL of a 0.0492 M sodium sulfate solution. What is the concentration of lead ion required to just initiate precipitation?
- Solid lead acetate is slowly added to 75.0 mL of a 0.0492 M sodium sulfate solution. What concentration of lead ion is required to initiate precipitation?
- An aqueous solution of 1.90 M AgNO3 is slowly added from a buret to an aqueous solution of 0.0100 M Cl- and 0.250 M I-. When the second ion begins to precipitate, what is the remaining concentration o
- Knowing that the concentration of Ag+ in a silver chromate solution is 1.5 times 10^-3 M, calculate its solubility product at 25 degrees Celsius.
- Given a solution containing 0.01 M of lead chloride and 0.01 M of lead chromate, calculate the concentration of Pb^{2+}. Using the K_{sp} (PbCl_2) = 1.7 times 10^{-5} and K_{sp} (PbCrO_4) = 1.77 times 10^{-14}. What is the solid remaining?
- 20.0 mL of a 2.2 M lead (II) nitrate solution is mixed with 100.0 mL of a 0.75 M magnesium sulfate solution. What is the concentration of nitrate ions in the resulting solution?
- What must the silver ion concentration be in order for precipitation to just begin when the silver ion is added to a 5.0 10 4 M N a 2 C O 3 solution? ( K s p = 8.1 10 12 for A g 2 C O 3 ). (a) 4.1 10 9 (b) 1.6 10 8 (c) 6.4 10
- Sodium phosphate is added to a solution that contains 0.0046 M aluminum nitrate and 0.051 M calcium chloride. The concentration of the first ion to precipitate (either Al^{3+} or Ca^{2+}) decreases as its precipitate forms. What is the concentration of t
- Sodium phosphate is added to a solution that contains 0.0046 M aluminum nitrate and 0.051 M calcium chloride. The concentration of the first ion to precipitate (either Al^{3+} or Ca^{2+}) decreases as its precipitate forms. What is the concentration of th
- Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0370 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4 (s) begins to precipitate?
- A solution consists of 0.050 M Fe(NO_3)_2 and 0.025 M Cu(NO_3)_2. Which species will precipitate first as NaoH is added to the solution? a) Cu(OH)_2 \\b) Fe(OH)_2 \\c) Fe(NO_3)_2 \\d) Fe(OH)_3 \\e) NaNO_3 \\f) No precipitate will form What concentration
- In a test tube, 10 mL of 0.100 M KI and 10 mL of 0.100 M Na2CO3 are mixed. Next, 0.10 M lead nitrate is added drop wise. What will be the concentration of CO3 2- when PbI2 first starts to precipitate? Ksp (PbCO3) = 1.5 x 10^-13 Ksp(PbI2) = 8.7 x 10^-9
- An aqueous solution contains 0.010 M Br- and 0.010 M I-. If Ag+ is added until AgBr(s) just begins to precipitate, what are the concentrations of Ag+ and I-? (Ksp of AgBr = 5.4 * 10-13, Ksp of AgI =
- In the process of separating Pb2+ ions from Cu2+ ions as sparingly soluble iodates, what is the Pb2+ concentration when Cu2+ begins to precipitate as sodium iodate is added to a solution that is initi
- Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag_2CrO_4 is 1.12 x 10^{-12}. What is the solubility (in mol/L) of silver chromate in 1.00 M potassium chromate aqueous solution?
- A solution contains .036 M Cu^2+ and .044 M Fe^2+. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. at what concentration of sulfide ion with
- If solid AgNO_3 is slowly added to a solution that is 0.05 M in NaI and 0.12 M in NaCl, what is the concentration of I^- when AgCl just begins the precipitate? (K_{sp} \text{ for } AgCl= 1.8
- It is necessary to add iodide ions to precipitate the lead(II) ions from 250 mL of 0.069 M Pb(NO3)2 (aq). What minimum iodide ion concentration is required for the onset of PbI2 precipitation? The solubility product of PbI2 is 1.4 ? 10-8. Answer in units
- 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
- 5 ml of 0.004 M silver nitrate is added to 5 ml of 0.0024 M potassium chromate. Calculate the concentration of silver and chromate.
- What is the I- concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.0500 M Cl- and 0.0500 M I-? (Ksp values: AgCl = 1.8 times 10-10; AgI = 1 tim
- What is the concentration of nitrate ions in a solution that contains 0.900 M aluminum nitrate?
- Does a precipitate form when aqueous solutions of silver nitrate and sodium hydroxide are mixed? If so, write the formula of the precipitate.
- A 1.000L solution is prepared in which Au+, Ag+, and Cu+ ions are present in solution as nitrates all at a concentration of 0.001M a solution of sodium chloride is slowly added. Which compound will begin to precipitate first? Ksp of AuCl = 2.0x10^-13, Ag
- (a) What is a net ionic equation for the reaction between potassium chromate and lead acetate? (b) Determine whether or not this reaction will lead to a precipitate.
Explore our homework questions and answers library
Browse
by subject