Excess solid Na₂CO₃ is added to a solution containing 0.400 M (each) Mg²⁺ and Zn²⁺ ions. Ksp for MgCO₃ is 3.50 × 10⁻⁸ and Ksp for ZnCO₃ is 1.00 × 10⁻¹⁰. ZnCO₃, with the smaller Ksp, will be the least soluble and will begin precipitating first. What will be the [Zn²⁺] concentration when MgCO₃ just begins to precipitate? (Assume no volume change upon addition of the solid Na₂CO₃).
Excess solid Na₂CO₃ is added to a solution containing 0.400 M (each) Mg²⁺ and Zn²⁺ ions....
A solution contains 0.021 M Cl? and 0.017 M I?. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10-6, Ksp(CuI) = 5.1 × 10-12. please show work! A) 4 .8 × 10-5 M, CuCl B) 3 .0 × 10-10 M, CuI C) 3 .0 × 10-10 M, CuCl D)...
A solution is 0.0045 M in both Pb2+ and Ca2+. Solid Na2SO4 is added to precipitate the sulfates. What concentration of SO42‒ is needed to precipitate as much of the Pb2+ without precipitating the Ca2+? Ksp(PbSO4) = 1.6 × 10‒8, Ksp(CaSO4) = 2.4 × 10‒4
NONTON Aluminum ions may be precipitated from aqueous solution by the addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions, and hydroxide ions begin to form. How many grams of solid NaOH should be added to 10.0 mL of 0.131 M AICI: to just precipitate all the aluminum?
A solution of Na,C,0, is added dropwise to a solution that is 0.0658 M in Cd2+ and 0.000500 M in Agt. The Ksp of CdC204 is 1.42e-08. The Ksp of Ag2C204 is 5.4e-12. (a) What concentration of C2042- is necessary to begin precipitation? (Neglect volume changes.) [C2042-] = M. (b) Which cation precipitates first? Cd2+ Agt (c) What is the concentration of C,042- when the second cation begins to precipitate? [C20-21 = C M .
pt Solid Na SO, is added slowly to a solution that is 0.76M in Pb(NO3), and 0.45M in Ba (NO3),. In what order will solid PbSO4 and BaSO4 form? Calculate the percentage of Ba2+ that precipitates just before PbSo, begins to precipitate. Assume that Ksp (PbSO4) = 1.8 x 10-8 and Kg (BaSO4) = 1.1 x 10-20 will precipitate first. pe Percentage =
A solution contains 0.10 M concentrations of Ba2+, Ca2+, and Sr2+. Na2CO3 is slowly added to the solution. In what order will the ions begin to precipitate? What is the concentration of the first ion when the 2nd begins to precipitate? Ksp for BaCO3 = 2.58 x 10-9, for CaCO3 = 3.36 x 10-9, and for SrCO3 = 5.60 x 10-10.
solution containing Qir Solid Silver witrate (1.00-g, arka "Siluentes uitrate) was added to a solution excess sodium Chloride & A white precipitate forms with no meaning silver nitrate is solved. Write aj a balanced reaction. equation predicting the identity of the Solid that forms b) a a net ionic equation (NIE) and c) determine the mass solid that forms assuming 100% yield.
Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+. What is the concentration of silver when the lead (II) iodide just begins to precipitate? [Ksp (Pbi2) = 1.4 × 10–8; Ksp (Agi) = 8.3 × 10–17] Please show all work
Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4and BaCrO4are 1.1 × 10^-12 and1.2 ×10^-10, respectively. ANSWER SAYS 3.2 x 10^-4 M Can someone explain how they got the answer? (3.2 x 10^-4 M)
A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10-2 M Fe2+ and 1.49×10-2 M Cd2+. What concentration of CO32- is need to initiate precipitation? Neglect any volume changes during the addition. Ksp value: FeCO3: 2.10*10-11 Ksp value: CdCO3: 1.80*10-14 Which cation precipitates first? What is the concentration of CO32- when the second cation begins to precipitate?