A student mixes 100.0 mL of 0.0055 M Mg(NO3)2 with 100.0 mL of 0.0015 M Na2CO3. Calculate Qsp
A student mixes 100.0 mL of 0.0055 M Mg(NO3)2 with 100.0 mL of 0.0015 M Na2CO3....
A student mixes 39.0 mL of 2.88 M Pb(NO3)2(aq) with 20.0 mL of 0.00197 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?
Will a precipitate form when 100.0 mL of 6.8 x 10-4 M Mg(NO3)2 is added to 100.0 mL of 1.2 x 10-4 M NaOH? The ion product for Mg(OH)2 is 1. Since Q is than Ksp, Mg(OH)2 precipitate from the solution.
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C. A student mixes 5.12 mL of 4.02 x 10...
student mixes 35.0 mL of 3.18 M Pb(NO3)2(aq) with 20.0 mL of 0.00151 M Nal(aq). How many moles of Pbl2(s) precipitate from the resulting solution? Number 3.02x 10-5mol What are the values of [P NO3, and [Na'] after the solution has reached equilibrium at 25 °C? Number Number Pb2.02 111-114.84 ×10-9 IM Number Number NO4.05
A 100.0 mL sample of 0.292 M Na2CO3 is mixed with a 100.0 mL sample of 0.292 M X(ClO4)2. Both solutions are at 20.0C before mixing. The temperature of the mixture rises to 29.0C. Determine the enthalpy of reaction (in kJ), per mole of Na2CO3 reacted.
You prepare a solution by mixing 400.0 mL of 1 x 10-4 M Mg(NO3)2 and 500.0 mL of 1.00 x 10-4 M NaF. What is the observed outcome? For MgF2, Ksp = 6.4 x 10-9. A. A precipitate forms because Qsp > Ksp. B. No precipitate forms because Qsp > Ksp. C. No precipitate forms because Qsp = Ksp. D. No precipitate forms because Qsp < Ksp. E. A precipitate forms because Qsp < Ksp.
Calculate Qsp for calcium fluoride (Ksp = 3.9x10-11) when 100.0 mL of a 6.05x103 M solution of Ca(NO3)2 is added to 275.0 mL of a 6.50x10 Msolution of KF.
A student mixes 41.0 mL of 2.84 M Pb(NO3)2(aq) with 20.0 mL of 0.00235 M Nal(aq). How many moles of Pbla(s) precipitate from the resulting solution? Number K,,[Pb12()] – 9810 mol What are the values of [Pb2+), [1]. [NO3-), and [Na*) after the solution has reached equilibrium at 25 °C? Number Number [Pb?*] = Number Number [no; ]- 0 M [nat)-
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN. The student finds that the equilibrium concentration of FeSCN2+ is 5.6 x 10-4M. a. Set up the Kc expression for the following equation. Fe3+ + SCN- ↔ FeSCN2+b. What is the total volume of the solution? _______ mL c. Fill in the following table for the moles of each species.d. Find the concentration for the above ions. e. Calculate Kc for the reaction.
A 25.00 mL solution of 0.03190 M Na2CO3 is titrated with 0.02660 M Ba(NO3)2 . Calculate pBa2+ following the addition of the given volumes of Ba(NO3)2 . The ?sp for BaCO3 is 5.0×10−9 . 15.50 mL pBa2+= ?ep Ba2+= 35.50 mL pBa2+