An AgNO_3 solution (44 ml/0.44 M) has been mixed with an NaCl solution (83 ml/1.35 times 10^{-2}...
Question:
An {eq}\rm AgNO_3 {/eq} solution {eq}\rm (44\ ml/0.44\ M) {/eq} has been mixed with an {eq}\rm NaCl {/eq} solution {eq}\rm (83\ ml/1.35 \times 10^{-2}\ M) {/eq}.
a) Determine the ion product of the precipitate(potential precipitate).
b) Would a precipitate be created? The {eq}\rm K_{SP} {/eq} of {eq}\rm AgCl(s) {/eq} proves to be {eq}\rm 1.8 \times 10^{-10} {/eq}.
Solubility Product Constant
The solubility product constant {eq}K_{sp} {/eq} is an equilibrium constant describing the dissociation of an insoluble salt.
Consider, for example, the dissociation of lead chloride {eq}\text{PbCl}_2 {/eq}:
{eq}\begin{align*} \text{PbCl}_2\text{(s)} \rightleftharpoons \text{Pb}^{2+}\text{(aq)} + \text{Cl}^-\text{(aq)} \end{align*} {/eq}
The {eq}K_{sp} {/eq} expression, which is just the equilibrium constant of the dissociation reaction, is given by:
{eq}\begin{align*} K_{sp} &= [\text{Pb}^{2+} ][\text{Cl}^- ]^2 \end{align*} {/eq}
Note that solids are excluded from the equilibrium expression.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThe salts being mixed are {eq}\text{AgNO}_3 {/eq}, which consists of {eq}\text{Ag}^+ {/eq} and {eq}\text{NO}_3^- {/eq}, and {eq}\text{NaCl} {/eq},...
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
- Identify whether there will be a precipitate when NaCl is mixed with AgNO3. If there is a precipitate, what will it be?
- Silver chloride has Ksp = 1.6 x 10^-10 and silver chromate has Ksp = 9.0 x 10^-12. We have 1.00 liter of a solution that contains both NaCl (0.10 M) and Na2CrO4 (0.10 M). Solid AgNO3 is added slowly and the solution is stirred well. Which salt precipitat
- When NaCl is mixed with AgNO3, will a precipitate form? If there is a precipitate, what will it be?
- For AgCl, Ksp = 1.8 x 10-10. What will occur if 250 mL of 1.5 x 10-3 M NaCl is mixed with 250 mL of 2.0 x 10-7 M AgNO3? a. A precipitate will form because P greater than Ksp. b. A precipitate will form because Ksp greater than P. c. No precipitate will fo
- Predict whether a precipitate will form if you mix 175.0 mL of a 0.0055 M KCI solution with 145.0 mL of a 0.0015 M AgNO_3 solution. Identify the precipitate, if any. K_sp AgCI = 1.77 x 10^-10
- A 3.60-L solution of 1.60 x 10^-3 M Pb(NO3)2 is mixed with a 0.60-L solution of 0.53 M NaCl. Calculate Qc for the dissolution of PbCl2 (Ksp = 1.6 x 10^-5). No precipitate has formed.
- The Ksp for Ag2CrO4 is 9.0 x 10-12. If 200 mL of 0.0050 M AgNO3 is combined with 300 mL of 0.0020 M K2CrO4, will a precipitate form? Explain.
- A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)
- Determine whether or not a precipitate will form if 75 mL of a 0.0500 M AgNO3 solution is mixed with 35 mL of a 0.0225 M NaBr solution.
- You have a solution consisting of 0.10 M Cl^- and 0.10 M CrO4^{-2}. You add 0.10 M silver nitrate dropwise to this solution. Given that the Ksp for Ag2CrO4 is 9.0 * 10^{-12} and that for AgCl is 1.6 * 10^{-10}, which of the following will precipitate firs
- NaCl is added slowly to a solution that is 0.010 M each in Cu^+, Ag^+, and Au^-. The K_{sp} for CuCl, AgCl, and AuCl are 1.9 times 10^{-7}, 1.8 times 10^{-10}, and 2.0 times 10^{-13}, respectively. Which compound will precipitate first?
- 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
- Predict whether a precipitate will form if you mix 175.0 mL of a 0.0055 M KCl solution with 145.0 mL of a 0.0015 M AgNO_3 solution. Identify the precipitate, if any.
- Predict whether or not a precipitate will form upon mixing 175.0 mL of a 0.0055 M KCl solution with 145.0 mL of a 0.0015 M AgNO3 solution. Identify the precipitate, if any.
- A very dilute solution of silver nitrate (AgNO_3) is added dropwise to a solution that contains equal concentrations of sodium chloride (NaCl) and potassium bromide (KBr). Explain which salt will precipitate first.
- The Ksp of AgCl at 25 degrees Celsius is 1.6 x 10-10. Consider a solution that is 1.0 x 10-5 M CaCl2 and 1.0 x 10-6 M AgNO3. A. Q greater than Ksp and a precipitate will form. B. The solution is saturated. C. Q less than Ksp and a precipitate will not for
- Would a mixture of aqueous solutions of AgNO3 and NaCH3CO2 form a precipitate? Explain.
- 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
- Show whether or not a precipitate will form when a solution containing 1 times 10^{-2} M Pb^{2+} ions is added to a 2 times 10^{-4} M solution of I^- ions. The K_{sp} of PbI_2 is 9.8 times 10^{-9}.
- A solution is 0.10 M Pb(NO_3)_2 and 0.10 M AgNO_3. If solid NaCl is added to the solution what is [Ag^+] when PbCl_2 begins to precipitate? (K_{SP} PbCl_2 = 1.7 times 10^{-5}; AgCl = 1.8 times 10^{-10}).
- Solid silver nitrate is slowly added to a solution that is 0.0010 M each in NaCl, NaBr, and NaI. Calculate the Ag^+ required to initiate the precipitation of each of the silver halides. For AgI, K_{sp} = 1.5 \times 10^{-16}; for AgBr, K_{sp} = 3.3 \tim
- Consider a solution made by dissolving 1.0 x 10-4 M AgNO3 and 1.0 x 10-4 M NaCl. Will a precipitate of AgCl form? (Ksp = 1.6 x 10-10 for AgCl)
- NaCl reacting with Cu(NO3)2: Precipitate or No Precipitate?
- Predict whether or not a precipitate will form if Na2CrO4 reacts with AgNO3. If a precipitate will form, write its formula.
- Which will precipitate first when AgNO3 is added to a solution containing equal concentrations of Br-, Cl-, and I- ions? A. AgBr B. AgCl C. AgI D. AgNO3 E. No precipitate will form.
- Determine whether a precipitate will form if 1.7 g of solid AgNO_3 and 14.5 g of solid NaCl are dissolved in 200 mL of water to form a solution at 25 degrees C. Use K_{sp} of 1.8 times 10^{-10}.
- AgNO3 reacting with Na3PO4 : Precipitate or No Precipitate?
- A solution containing 0.10 L of 0.12 M NaCl and 0.23 L of 0.18 M MgCl2 is precipitated with AgNO3. What volume of 0.20 M AgNO3 would be needed to precipitate all of the chloride?
- Suppose 125 mL of a 0.020 M Pb(NO3)2 solution is mixed with 75 mL of a 0.020 M NaCl solution. Will a precipitate form? The Ksp for PbCl2 is 1.6 x 10-5.
- The Ksp of AgI is 8.3 10-17. You titrate 25.00 mL of 0.08900 M NaI with 0.05010 M AgNO3. Calculate pAg after the following volumes of AgNO3 are added: (a) at 36.20 mL (b) at Ve (c) at 47.50 mL
- Determine whether a mixture of AgNO3 and KI will produce a precipitate.
- A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp(AgCl) = 1.77 x 10-10.
- Predict whether or not a precipitate will form if AgNO3 reacts with Na2SO4. If a precipitate will form, write its formula.
- Will a precipitate form if 500 ml of 2.5 x 10^-3 M AgNO3 is added to 500 ml of 3.8 x 10^-4 NaCl (Ksp of AgCl = 1.8 x 10^-10)?
- Predict whether or not a precipitate will form if NaNO3 reacts with AgNO3. If a precipitate will form, write its formula.
- A solution contains 0.15 mol/L of NaCl and 0.0034 mol/L of Pb(NO3)2. Does a precipitate form? Include a balanced equation for the formation of the possible precipitate.
- 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
- The likely precipitate formed by mixing BaCl2 and AgNO3 would have the formula: a) No precipitate will be formed. b) Ba(NO3)2 c) BaNO3 d) AgCl e) AgCl2
- The Ksp for AgCl is 1.8 x 10^-10. If NaCl is added to a 0.010 M solution of AgNO3 in water, at what concentration of Cl- does precipitation of AgCl begin to occur?
- A solution is 0.15 M in both Pb2+ and Ag+. If Cl- is added to this solution, what is the Ag+ when PbCl2 begins to precipitate? (Ksp of AgCl = 1.8 x 10-10, Ksp of PbCl2 = 1.7 x 10-5)
- Solid AgNO3 is slowly added to a solution that contains 0.24 M Cl- and 0.13 M Br- (assume volume does not change). What is (Br-) (in M) when AgCl(s) starts to precipitate? The Ksp of AgCl is 1.8 x 10-10. The Ksp for AgBr is 5.0 x 10-13.
- A solution is 0.015 M in I- ions and 0.015 M in Br- ions. Ag+ ions are introduced to the solution by the addition of solid AgNO3. Determine (a) which compound will precipitate first, Agl or AgBr, and (b) the percentage of the halide ion in the first preci
- A. A 3.10-L solution of 1.60 times 10^{-3} M Pb(NO_3)_2 is mixed with a 0.60-L solution of 0.95 M NaCl. Calculate Q_c for the dissolution of PbCl_2 (K_{sp} = 1.6 times 10^{-5}). No precipitate has formed. B. Is the solution supersaturated, saturated, or
- Use your experimentally determined value of Ksp and show, by calculation, that Ag2CrO4 should precipitate when 5 mL of 0.0040 M AgNO3 are added to 5 mL of 0.0024M K2CrO4
- Predict whether or not a precipitate will form if Na2SO3 reacts with AgNO3. If a precipitate will form, write its formula.
- Predict whether or not a precipitate will form if NaNO2 reacts with AgNO3. If a precipitate will form, write its formula.
- 1. For Silver Chloride, the reaction is AgCl \leftrightarrow Ag+ and Cl- and k_{sp} \ = 1.8 \times 10^{-10} a. Determine the concentration of Chloride ions in a saturated (at equilibrium) solution
- A solution is 5.0 x 10^-5 M in each of these ions: Ag^+, SO_4^2-, Cl^-, CO3^2 Which precipitate will form? Ag_2SO_4 (K_sp= 1.12 x 10^-5) AgCl (K_sp = 1.77 x 10^-10) Ag_2CO_3 (K_sp= 8.46 x 10^-12)
- If 25.8 mL of a AgNO3 solution is needed to precipitate all of the Cl- ions in a 0.795-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution?
- Problem 17.75 If a dilute AgNO_3 solution is slowly added to the solution, what is the first compound to precipitate: Ag_2CrO_4 ( Ksp = 1.2 x 10^-12), Ag_2CO_3 ( Ksp = 8.1 x 10^-12), or AgCl ( Ksp = 1
- A solution is prepared by mix 0.11 L of 0.14 M NaCl with 0.23 L of a 0.16 MgCl2 solution. What volume of 0.20 M AgNo is required to precipitate all the Cl^- ion in the solution as AgCl ?
- For precipitate to form, ion product must be a) less than the Ksp. b) equal to the Ksp. c) equal or greater than the Ksp. d) none of the above.
- Will silver iodide precipitate from a solution that is 0.0045 M AgNO_3, 0.15 M NaI, and 0.20 M KCN?
- What possible precipitate might form by mixing 50.0 mL of 1.0 x 10-4 M NaCl with 50.0 mL of 1.0 x 10-6 M AgNO3?
- 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?
- If the K_sp of AgCl is 1.5 * 10^-8, calculate the concentration (molarity) of AgCl in a saturated solution. Calculate the solubility of AgCl in a solution that contains .10 M Cl^-(aq).
- 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
- Predict whether or not a precipitate will form if BaCl2 reacts with AgNO3. If a precipitate will form, write its formula.
- 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
- Ag+ is added to a solution of 0.0021 M Cl- and 0.0011 M SCN-. The AgSCN precipitates first (K{sp} = 1.0 x 10{-12}), followed by the AgCl (K{sp} = 1.8 x 10{-10}). What percentage of the SCN- is still in solution (not precipitated) when the AgCl just starts
- If 26.0 mL of AgNO_3 is needed to precipitate all the Cl^- ions in a 0.795 mg sample of KCl (forming AgCl), what is the molarity of the AgNO_3 solution?
- If 25.2 mL of AgNO_3 is needed to precipitate all the Cl^- ions in a 0.750-mg sample of KCl (forming AgCl ), what is the molarity of the AgNO_3 solution?
- If 26.0 mL of AgNO_3 is needed to precipitate all the Cl^- ions in a 0.800-mg sample of KCl (forming AgCl), what is the molarity of the AgNO_3 solution?
- Silver ions may be recovered from used photographic fixing solution by precipitating it is as silver chloride. The solubility of silver chloride is 1.6 x 10-3 g/L. Calculate the Ksp in for silver chlo
- 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
- An excess of aqueous AgNO_3 reacts with 24.5 mL of 5 M K_2CrO_4(aq) to form a precipitate. What is the precipitate? 1. AgNO_3. 2. Ag_2CrO_4. 3. KNO_3. 4. K_2CrO_4.
- What if any precipitate will form from the mixing of these pairs of solutions? A) MgCl2 and AgNO3 B) KCl and (NH4)2SO4
- What is the solubility of AgCl, when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for the
- Calculate the Q_{sp} or K_{sp}, as indicated, and determine whether a precipitate will form when each of the following mixtures is prepared. 14.95 mL 3.65 times 10^{-3} M Pb(NO_3)_2 is mixed with 34.89 mL 1.745 times 10^{-4} M Na_2SO_4. (K_{sp} for PbSO_4
- If you could explain it thoroughly it would help immensely. Determine whether a precipitate will form if 75 mL of 0.0500 M AgNO3 is mixed with 50 mL of 0.0225 M NaBr and justify your decision. a. Ye
- You have 310. mL of a 5.75 x 10-5 M Pb(NO3)2 solution. How many moles of NaCl must be added to precipitate a solid? The Ksp of PbCl2 is 1.6 x 10-5.
- The Ksp of AgCl is 1.6x10-10 what is the (Ag+) and (Cl-) in a saturated solution of AgCl?
- Calculate the Q_{sp} or K_{sp}, as indicated, and determine whether a precipitate will form when each of the following mixtures is prepared. 50.27 mL 2.53 times 10^{-2} M Pb(NO_3)_2 is mixed with 25.11 mL 4.68 times 10^{-5} M NaBr. (molar solubility of Pb
- If you mix a 0.200 M NaClO3 solution with a 0.100 (NH4)2SO4 solution, will a precipitate be produced? If there is a precipitate, identify the precipitate.
- Predict whether or not a precipitate will form if NaI reacts with AgNO3. If a precipitate will form, write its formula.
- Calculate the concentrations of all ions after 50.0 ml of a 0.100 M AgNO_3 solution is mixed with 100.0 ml of a 1.00 M Na_2SO_4 solution.For Ag_2SO_4 K_{SP} = 1.2 times 10^{-5}.
- 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 .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)
- Write the formula for the precipitate that forms (if any) in the reaction between AgNO3 and (NH4)2S.
- You could add solid KCl to the solution to precipitate out AgCl(s). What mass of KCl is needed to precipitate the silver ions from 13.0 mL of 0.180 M AgNO3 solution?
- 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?
- An excess of aqueous AgNO3 reacts with 41 mL of 5 M K2CrO4(aq) to form a precipitate. What is the precipitate?
- You could add HCl (aq) to the solution to precipitate out AgCl (s). What volume of a 0.200 M HCl (aq) solution is needed to precipitate the silver ions from 13.0 mL of a 0.180 M AgNO3 solution?
- Calculate the mass of solid NaCl that must be added to 1.5 L of 0.100 M AgNO_3 solution to precipitate all the Ag^+ ions in the form of AgCl?
- Identify the precipitate(s) of the reaction that occurs when a silver nitrate solution is mixed with a sodium chloride solution. Check all that apply.
- For the following chemical reaction, determine the precipitate produced when the two reactants listed below are mixed together. Indicate none if no precipitate will form. AgNO_3(aq) + KCl (aq) to
- 24.6 mL of 0.488 M NaCl is added to 24.6 mL of 0.312 M AgNO3. How many moles of AgCl would precipitate? What would be the concentrations of each of the ions in the reaction mixture after the reaction?
- Will a precipitate form when 1.00 g of AgNO_3 is added to 50.0 mL of 0.050 M NaCl? If so, would you expect the precipitate to be visible?
- Calculate the solubility of Ag2SO4 (Ksp = 1.2 x 10-5) in a 2.0 M AgNO3 solution.
- If you mixed a silver nitrate solution with a sodium chloride solution, would you precipitate a silver salt? Explain.
- How many milliliters of a 0.200M AgNO3 solution are required to precipitate most of the Cl^(-) ions from a solution containing 0.855 g of NaCl?
- The solubility of AgCl is 0.000013 mol / L. Calculate the K_{sp} for AgCl.
- 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?
- Will a precipitate of Ca(lO_3)_2 form when 400. mL of 0.015 M CaCl_2 M of are added to 300. mL of 0.15Ml NaIO_3? The Ksp of Ca(IO_3)_2 is 6.47x10^-5. a) What is the reaction for the solubility of Ca
- A solution is prepared by mixing 0.11 L of 0.12 M sodium chloride with 0.26 L of a 0.19 M MgCl2 solution What volume of a 0.21 M silver nitrate solution is required to precipitate all the Cl- ion in t
- 1.55 g of CaCl_2 is added to 5.25 L of a 4.75 \times 10^{-6} M solution of Na_2CO_3. Will a precipitate of CaCO_3(s) form? K_{sp} of CaCO_3 (s) = 2.8 \times 10^{-9}.
- Lanthanum iodate, La(IO3)3, has Ksp = 6.2 x 10-12. If 10 mL of a 0.0050 M La(NO3)3 solution is mixed with 10 mL of a 0.0050 M NaIO3 solution, will La(IO3)3 precipitate? Explain.
- Lanthanum iodate La(IO3)3 has Ksp = 6.2 x 10-12. If 50 mL of a 0.125 M La(NO3)3 solution is mixed with 50 mL of a 0.050 M NaIO3 solution, will La(IO3)3 precipitate? Explain.
- Lanthanum iodate, La(IO3)3, has Ksp = 6.2 x 10-12. If 50 mL of a 0.00050 M La(NO3)3 solution is mixed with 50 mL of a 0.0050 M NaIO3 solution, will La(IO3)3 precipitate? Explain.
- Does a precipitate form when aqueous solutions of silver nitrate and sodium chloride are mixed? If so, write the formula of the precipitate.
Explore our homework questions and answers library
Browse
by subject