Calculate the solubility (in g/L) of CaSO,(s) in 0.500 M Na, SO, (aq) at 25°C. The Ksp of CaSO, is 4.93 x 10-5. solubility: g/L

The Ksp of PbBr, is 6.60 × 10-6. What is the molar solubility of PbBr, in pure water? molar solubility: M What is the molar solubility of PbBr, in 0.500 M KBr solution? molar solubility: M What is the molar solubility of PbBr, in a 0.500 M Pb(NO,), solution? molar solubility: M

An acidic solution containing 0.020 M La+ is treated with NaOH until La(OH), precipitates. At which pH does this occur? Ksp for La(OH), is 2 × 10-21. pH =

If 14.00 mL of 0.10 M Ba(NO3), are added to 30.00 mL of 0.10 M Na,CO3 a precipitate of BaCO3 will form. O a precipitate of NaNO3 will form. O no precipitation occurs because both possible products are soluble. no precipitate forms because Q< Ksp-

Calculate the solubility (in g/L) of CaSO, (s) in 0.300 M Na, SO,(aq) at 25°C. The K5p of CaSO, is 4.93 x 10-5. The molar mass of CaSO4 is 136.14 g mol-l. solubility: g/L

Calculate the solubility (in g/L) of CaSO4(s) in 0.400 M Na₂SO (aq) at 25°C. The Ksp of CaSO4 is 4.93 × 10-5. 4 solubility: g/L

A solution is prepared by mixing 75.0 mL of 0.020 M BaCl, and 110. mL of 0.040 M K,SO4. What are the concentrations of barium and sulfate ions in this solution? Kp for BaSO4(s) = 1.5×10°. Assume that only SO, ions (no HSO4) are present. 2- [Ba"] = M [So,?]=|

Calculate the value of Q and determine if a precipitate of CaCO, will form when 65.0 mL of 0.035 M CaCl, is added to 45.0 mL of 0.095 M Na,CO,? Ksp CaCO, = 8.7 x 109.