Will a precipitate occur in a solution that is initially 1.30 x 10-5 M Co+2(aq) and 2.48 x 10-5 M CO3-2(aq)? Ksp = 1.4 x 10-13
CoCO3(s) ↔ Co+2(aq) + CO3-2(aq)
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Will a precipitate occur in a solution that is initially 1.30 x 10-5 M Co+2(aq) and...
Calculate the equilibrium concentration of Co3+ (aq) in a solution that is initially 0.0300 M CO(NO3)2 and 0.500M NH3. The formation constant for CO(NH3)6]** (aq) is Kf= 2.3 x 1033 ICO(NL) I Costa
For the reaction Ba(OH)2 (s) -- Ba2+ (aq) + 2 OH (aq) a precipitate will form if Q< K. Select one: True False Into a solution of 0.10 M KBr and 0.10 M KCYOA you add 0.050 M silver nitrate dropwise until a precipitate forms. Ksp for Ag2Cronis 9.0 x 10-12. Ksp for AgBr is 5.0 x 10-13. Which of the following will precipitate first? Select one or more: a. silver chromate b. no precipitate will form C. silver bromide...
An acidic solution is 0.01 M in Mg2+, Cu2+, and Fe2+. The pH of the solution is adjusted by adding NaOH. What is the maximum pH that removes only the Cu2+? Mg(OH)2(s) ↔ Mg2+(aq) + 2OH–(aq) Ksp = 6.3 x 10–10 Fe(OH)2(s) ↔ Fe2+(aq) + 2OH–(aq) Ksp = 4.1 x 10–15 Cu(OH)2(s) ↔ Cu2+(aq) + 2OH–(aq) Ksp = 2.2 x 10–20
For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 1.5 mL of 0.035 M lead nitrate is added to 13 mL of 0.010 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms.
1) For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.5 mL of 0.070 M lead nitrate is added to 19 mL of 0.018 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms. 2) Sodium phosphate is added to a solution that contains 0.0041 M aluminum nitrate and 0.028 M calcium chloride. The concentration of the first ion to...
Will Co(OH)2 precipitate from solution if the ph of a .020 M solution of Co(NO3)2 is adjusted to 8.5? If yes what is the ph needed to stop precipitation? If no what is the ph needed to start precipitation? Ksp Co(OH)2= 5.9* 10^-15
BaCO;(s)Ba2t(aq) +CO3 (aq) The solubility product is given by: Ksp = [Ba2+] [C0321-5.5 × 10-10 mol2 dm-6 If [Ba2+1 CO is greater than 5.5 x 10-10 mol2 dm-6 a precipitate will form. [CO,2-] is less than 5.5 x 10-10 mol2 dm-6 no If [Ba2+1[ precipitate will form. WORKED EXAMPLE Will a precipitate form if we mix equal volumes of solutionsof 1.00 × 10-4 mol dm-3 Na,co, and 5.00 × 10-5 mol dm-3 BaCl2? 9
A solution contains 0.0500 M Co^3+ (aq), 0.0310 M S^2- (aq), and 0.95 M NH_3. Cobalt(III) ions in aqueous solutions complex with NH_3 to produce Co(NH_3)_6^3+. (K_f = 5.0 times 10^31) What will be the concentration of Co^3+ (aq) when Co(NH_3)_6^3+ forms? Will CO_2 S_3 precipitate? (K_sp = 4.0 times 10^-21) precipitate forms no precipitate forms
Question 13 (5 points) Use IP to predict if a 2.5 x 10-5 M solution of PbCro, in a 1.7 x 10-M solution of Pb(NO3)2 will dissolve (ksp - 1.8 x 10-14). 8.1 x 10-15, dissolve 2.5 x 10-6; precipitate 4.7 x 10-12, dissolve 4.3 x 10-8; precipitate Question 14 (5 points) Use IP to predict if a 3.5 x 10-4 M solution of BaSO4 in a 0.035 M solution of Na,SOwill dissolve (ksp- 1.1 x 10-19). 4.3 x 10-10;...
Suppose a solution is made containing 7.3 x 10-3 M Sr(NO3)2(aq) and 8.3 x 102 M NaF (aq). Calculate Q and determine whether a precipitate of SrF2 (s) will form. (In other words, which of the following is entirely correct?) Ksp of SrF2 = 2.8 x 10-9 a. Q = 5.0 x 105, ppt forms b. Q = 5.0 x 10-5, no ppt c. Q = 2.0 x 104 ppt forms d. Q = 6.1 x 104.ppt forms e. Q...