Calculate the equilibrium concentrations of each ion in the final solution resulting from the mixing of 40.00 mL of 0.0450 M MgI2 and 60.00 mL of: b) 0.0500 M AgNO3 AgI 8.3 x 10-17 c) 0.0600 M Pb(NO3)2 PbI2 7.9 x 10-9
Calculate the equilibrium concentrations of each ion in the final solution resulting from the mixing of...
Calculate the equilibrium concentrations of each ion in the final solution resulting from the mixing of 40.00 mL of 0.0450 M MgI2 and 60.00 mL of: (3) Ksp a) 0.0400 M KOH Mg(OH)2 1.8 x 10-11 b) 0.0500 M AgNO3 AgI 8.3 x 10-17 c) 0.0600 M Pb(NO3)2 PbI2 7.9 x 10-9
Calculate Qip (ion product) for a mixture containing 25 mL of 5.0 × 10–9 M AgNO3 and 75 mL of 6.5 ×10–8 M KI. Decide whether AgI will precipitate from this mixture. The Ksp for AgI is 8.3 × 10–17 show all work
Suppose that a 10-mL sample of a solution is to be tested for I− ion by addition of 1 drop (0.2 mL) of 0.12 M Pb(NO3)2. What is the minimum number of grams of I−I− that must be present in order for PbI2(s)PbI2(s) (Ksp=8.49×10−9Ksp=8.49×10−9) to form? Express your answer using one significant figure.
4- (a) Calculate the concentration of Cd2+ ion in a solution prepared by mixing 2.0 mL of 1 M CA(NO3)2 solution with 1.0 L of 4.0 M NH3 solution. [Assume that the volume does not change after the addition of 2.0 ml of 1 M Cd(NO3)2] (b) Will you be able to see Ca(OH)2(6) precipitate in the solution? (Kr for Ca(NH3)42+ = 1.0 x 107, Kb for NH3 = 1.8 x 10-5; Ksp for Ca(OH)2 = 5.9 x 10-15 Cd2+...
A solution is prepared by mixing 47.00 mL of 0.024 M AgNO3 with 11.00 mL of 1.0×10-3M Na2CO3. Assume that volumes are additive. Calculate [Ag+], [CO32–], [Na+], and [NO3–] after equilibrium is established. [Ag+]= [CO32+]= [Na+]= [NO3-]=
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A solution is made by mixing 47.0 mL of 2.88 M Pb(NO), with 20.0 mL of 1.79 x 10°M Nal? K, for Pbl:(s) is 9.8 x 10" a) Will a solid form? Show reasoning. b) If you answered "yes" to part a) how many grams of Pbl (s) will form? c) What are the concentrations of [Pb 1,[11. [NO] and [Na') at equilibrium
A 25.00 mL solution of 0.08050 M NaI is titrated with 0.05000 M AgNO3 . Calculate pAg+ following the addition of the given volumes of AgNO3 . The ?sp of AgI is 8.3×10−17 . 35.80 mLpAg+= ?epAg+= 47.90 mLpAg+=
Need Help Calculate the final concentrations of Ba2+ and C2O42- in a solution prepared by mixing 0.100 L of 6.0x10-2 M K2C2O4 and 0.150 L of 1.0x10-2 BaBr2. Ksp (BaC2O4 = 2.3x10-8 M2)
5. A solution is made by mixing 200.0 ml of 1.5 x 10-4 M Cu(NO3)(aq) with 250.0 ml of 0.20 M NH3(aq). Calculate the concentration of copper ion (Cu? (aq)) in the solution when it reaches equilibrium. (Kr for [Cu(NH3)4]2+ = 1.7 x 1013)
HELP PLEASE 5 – Calculate the concentrations of H+, HCO3- and CO32- in a 0.025 M H2CO3 solution. 6 – Classify the following as a Lewis acid, Lewis base, both or neither:CO2, H2O, I-, SO2, NH3, OH-, H+, BCl37 – 7-Calculate the pH of a solution that is 0.20 M NH3 and 0.30 M NH4Cl.8 – 8-The pH of blood plasma is 7.40. Assuming the principal buffer system is HCO3-/H2CO3, calculate the ratio [HCO3-]/[H2CO3] . 9 – A 0.2688 g...