What is the solubility of PbSO4 in a solution which originally was 0.050 M in Pb(NO3)2?
What is the solubility of PbSO4 in a solution which originally was 0.050 M in Pb(NO3)2?
A solution is prepared by mixing 0.050 M Pb(NO3)2 with 0.00350 M KBr. The Ksp for PbBr2 is 6.6 x 10-6 a. Write a balanced net ionic equation for this chemical reaction b. Determine where this solution will be unsaturated, saturated or super saturated.
Consider a saturated AgBr solution that is also 0.050 M Ca(NO3)2. Ca(NO3)2(aq) + Ca2+ (aq) + 2NO3 (aq) AgBr(s) Ag+ (aq) + Br-(aq) The thermodynamic solubility product (Kop) of AgBr is 5.0 x 10-13. What must be the molarity of Ag+ in the solution?
Consider a saturated AgBr solution that is also 0.050 M Ca(NO3)2. Ca(NO3)2(aq) + Ca2+ (aq) + 2NO3(aq) AgBr(s) + Ag+ (aq) + Br (aq) The thermodynamic solubility product (Kyp) of AgBr is 5.0 x 10-13. What must be the molarity of Ag+ in the solution?
12. A solution of 0.00016 M lead (II) nitrate, or Pb(NO3)2, was poured into 450 mL of 0.00023 M sodium sulfate, Na2S04. Would a precipitate of lead(II)sulfate, PbSO4, be expected to form if 250 mL of the lead nitrate solution were added? Write the equilibrium equation of PbSO4 dissociation in water.
show work please The molar solubility of PbF2 in 0.10 M Pb(NO3)2 solution is 2.85 x 10-4 M. What is the Ksp for PbF2? A. 1.2 x 10-6 B. 3.1 x 10-7 C. 9.6 x 10-13 D. 3.2 x 10-8 What is the molar solubility of PbI, in pure water? Ksp = 9.8 x 10-9 A. 2.1 x 10-3 B. 1.7 x 10-3 C. 4.9 x 10-5 D. 1.3 x 10-3 What is the molar solubility of PbI2 in 0.20...
2) Of the substances below, ________ will decrease the solubility of Pb(NO3)2 in a saturated solution. a)NaCl b)HCN c)NaCN d)Pb(CN)2 e)H2O2 Can anyone explain briefly explain them with the correct answer?
QUESTION 21 A solution is 0.012 Min Pb(NO3)2 and 0.20 Min Sr(NO3)2. Solid Na2SO4 is added until a precipitate just begins to form. The precipitate is and the concentration of sulfate ion at this point is Ksp for PbSO4 is 1.8 x 10-8 and for SrS04 is 2.8 x 10-7 PbSO4: 1.5 10 M SrS04; 1.4 x 10-6M PbSO4; 6.3 * 10 M "SrS04; 8.3 x 10-?M S-S04:2.6 x 10-7M
Calculate the solubility in grams per liter of CaCO3 in 0.050 M Ca(NO3)2. The Ksp for CaCO3 is 3.36 x 10-9.
What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2?
What is the solubility of M (OH)2 in a 0.202 solution of M(NO3)2 ? ksp = 9.05*10^-18