3. A pipette is used to add 46 mL of 0.1 M Pb(NO3)2 to a 294.0...

3. A pipette is used to add 46 mL of 0.1 M Pb(NO3)2 to a 294.0 mL solution of 0.2 M NaF. Determine the equilibrium concentration of Pb2+(aq) in the final solution. Ksp(PbF2)=3.6E-8

Expert Solution

queen_honey_blossom answered 2 years ago

If we mix 19.0 mL of a 1.30 ✕ 10−3 M solution of Pb(NO3)2 with 18.6...

If we mix 19.0 mL of a 1.30 ✕ 10−3 M solution of Pb(NO3)2 with 18.6 mL of a 2.60 ✕ 10−3 M solution of NaBr, will a precipitate form? At this point we would identify the potential precipitate by switching the anions and using the solubility rules to decide if one of the potential products is potentially insoluble. Here the products would be PbBr2 and NaNO3. Of these, PbBr2 is considered "insoluble". The Ksp value for PbBr2 is 6.60 ...

A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL of...

A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL of .5 M NaF. Calculate the concentration of F- ions present at equilibrium. (Hint: First, write and balance the double displacement reaction taking place between Pb(NO3)2 and NaF to form PbF2(s). Perform the necessary stoichiometry (including finding which reactant is limiting) to calculate how much of each reactant remains after the reaction goes to completion. Remember that stoichiometry has to be done in moles. Once...

A solution is prepared by mixing 100 mL of .01 M Pb(NO3)2 and 100 mL of...

A solution is prepared by mixing 100 mL of .01 M Pb(NO3)2 and 100 mL of .001 M NaF. Will PbF2(s) precipitate in this reaction? Calculate the concentration of F- ions present at equilibrium. PbF2(s) <--> Pb2+(aq) + 2F-(aq) Kc= 3.7E-8 Please show all work! Thank you!

A student mixed 5.00 mL of 0.0120 M Pb(NO3)2 with 5.00 mL of 0.0300 M KI...

A student mixed 5.00 mL of 0.0120 M Pb(NO3)2 with 5.00 mL of 0.0300 M KI and observed a yellow precipitate. a. What is the molecular formula of the precipitate? PbI2 b. How many moles of Pb2+ are present initially? ___ c. How many moles of I- are present initially? ___ The concentration of I- at equilibrium is experimentally determined to be 8.0*10^-3 M. d. How many moles of I- are present in the solution (10mL)? ___ e. How many...

If 2.00 mL of 0.100 M Pb(NO3)2 are added to 1.00 L of 0.100 M KCl...

If 2.00 mL of 0.100 M Pb(NO3)2 are added to 1.00 L of 0.100 M KCl will a precipitate form? What will be the precipitate?

A student mixes 31.0 mL of 3.24 M Pb(NO3)2(aq) with 20.0 mL of 0.00217 M NaI(aq)....

A student mixes 31.0 mL of 3.24 M Pb(NO3)2(aq) with 20.0 mL of 0.00217 M NaI(aq). How many moles of PbI2(s) precipitate from the resulting solution? What are the values of [Pb2 ], [I–], [NO3–], and [Na ] after the solution has reached equilibrium at 25 °C?

A student mixes 31.0 mL of 3.06 M Pb(NO3)2(aq) with 20.0 mL of 0.00193 M Na2SO4(aq)....

A student mixes 31.0 mL of 3.06 M Pb(NO3)2(aq) with 20.0 mL of 0.00193 M Na2SO4(aq). How many moles of PbSO4(s) precipitate from the resulting solution? What are the values of [Pb2 ], [SO42–], [NO3–], and [Na ] after the solution has reached equilibrium at 25 °C? .......mol .....Ksp={PbSo4}=2.5 * 10^-8 part 2: what are the valuse of [Pb^+2], [SO4^-2], [NO3^+] after the solution has reached equilibrium at 25 C?

1. a.) A student mixes 47.0 mL of 3.30 M Pb(NO3)2(aq) with 20.0 mL of 0.00183...

1. a.) A student mixes 47.0 mL of 3.30 M Pb(NO3)2(aq) with 20.0 mL of 0.00183 M Na2C2O4(aq). How many moles of PbC2O4(s) precipitate from the resulting solution? What are the values of [Pb2 ], [C2O42–], [NO3–], and [Na ] after the solution has reached equilibrium at 25 °C? Ksp of PbC2O4 (s) is 8.5e^-9 M^2 b.) What are the values of [Pb^2+], [C2O4^2-], [NO3^-], and [Na^+] after the solution has reached equilibrium?

If we mix 40.0 mL of 3.00 M Pb(NO3)2 (aq) with 20.0 mL of 2.00 x...

If we mix 40.0 mL of 3.00 M Pb(NO3)2 (aq) with 20.0 mL of 2.00 x 10-3 M NaI (aq), does PbI2 (s) precipitate from solution? I yes, calculate how many moles of PbI2 (s) precipitate and the values of [Pb2+], [I-], [NO3-], and [Na+] at 25 C at equilibrium?

The following questions refer to the following system 3.5E2 ml of 3.2 M Pb (NO3)2 and...

The following questions refer to the following system 3.5E2 ml of 3.2 M Pb (NO3)2 and 2.0E2 mL of 0.020 M NaCl are added together. KSP for the chloride is 1.6E-5 a.) determine the ion product? b.) will precipitation occur? c.) What is the limiting reagent in the formation of lead chloride? d.) Determine the equilibrium concentration of the chloride ion?

Question