Calculate the molar solubility of Ag2CO3 in a solution of 0.015 M Na2CO3. The solution is aqueous at 25°C. Ksp (Ag2CO3)=8.12 x 10-12 [HINT: Ag=+1] a) 1.16 x 10-5 b) 2.73 x 10-4 c) 7.15 x 10-6 d) 5.78 x 10-4 e7.99 x 10-6 8.12 x 10-3 g) 1.22 x 10-6 h) 3.51 x 104

Calculate the mass of precipitate formed after 54 mL of 0.68M Na3PO4 is mixed with 34 mL of 0.84M CaBr₂ ab Edit Format Table 12pt Paragraph esc s lock A control ! 1 Q A 1 option BIUA 2 N W S #3 X E command D ✓ T² v $ 4 R C % 5 F ܀ I T V 8 MacBook Pro < 6 G Y B & 7 H U * : 0 0 words 8 N J ( 1 a 9 K M ) 0 O MOSISO

For which salt should the aqueous solubility be most sensitive to pH? O Ca(NO3)2 O Cal2 O CaF2 CaCl2 CaBr2

Which of the following salts has the highest molar solubility in pure water? 1 2 3 4 5 O O 1 3 4 5 02 Salt Cd(OH)2 PbCrO4 Mn(OH)2 Ni(OH)2 AgBr Ksp 5.3x10-15 1.8x 10-14 2.0 x 10-13 2.0 x 10-15 5.0 x 10-13

If Ks (Ksp) refers to the dissolved solution at equilibrium and Q refers to the dissolved solution in general which of the following is true? Q, > Kg [Ag*] Q, = Kg Qg Ks the solution is supersaturated thus crystals will form. O a, b and c O b only O a only O b and c equilibium states

Determine if precipitation of Cu2O (s) will occur when 120.0mL of 4.00 x 10^-9 M (NH4)2O is added to 70.0mL of 5.00 x 10 ^-9 M Cu2SO4. Assume that both dissolve 100% in water. Ksp Cu2O=2.00 x 10^-28 Cu2O in Equilibrium with 2Cu+ and O2-

Determine the molar solubility for Ag2SO4 (Ksp= 1.5 x 10-5) in a solution that already contains 0.200 M AgNO3.

Answer the following questions regarding chloroform (CHCl3) and methanol (CH3OH). A.Estimate the boiling points of methanol and chloroform. B.Based on your knowledge of intermolecular forces, are your calculations consistent with what you would have predicted regarding the boiling points of the two liquids?

If 360 mL of 2.66 x 10-4M Pb(NO3)2 is added to 275 mL of 8.37 x 10-5 M NaI (in aqueous solution) will a precipitate form? Ksp of PbI2 = 1.4 x 10-8

A 0.01 M AgNO3 was added dropwise to a solution containing 0.1 M each of NaCl, NaCN and Na2CrO4. AgCl Ksp= 1.8 x 10-10 Ag2CrO4 = 9 x 10-12 AgCN = 1.2 x 10-16   AgCN ppts first. What is the %CN- remaining when second ion precipitate starts?   A. 9 x 10-12 B. 9 x 10-9 C. 6.67 x 10-7 D. 6.67 x 10-5     Which of the following solvents can diffrentiate acid strengths of HCl, HBr and HI.   A H2O B. NH3 C. CH3COOH.