Consider a solution containing 0.181 M lead ions and 0.174 M mercury(II) ions. The Ksp for lead sulfide is 3.4 x 10-28 and that for mercury(II) sulfide is 4.0 x 10-53. Calculate the maximum concentration of sulfide ions that can be in solution without precipitating any lead ions. The answer is 1.4 x 10-27

1a. For each combination of two aqueous solutions, predict whether or not a precipitate (solid product) will form. Put a check mark by those reactions that WILL form a precipitate. options:   Na2CO3 and CaCl2   NH4NO3 and SrCl2   KI and PbNO3   KBr and NH4Cl   1b. Kidney stones generally form from the double displacement reaction of two salts that form an insoluble compound, a precipitate. Which of the following salts will react in a double displacement reaction with Na3PO4 to form an insoluble precipitate(s):   Potassium chloride (KCl)   Potassium carbonate (K2CO3)   Magnesium sulfate (MgSO4)   Oxalic acid (H2C2O4)   Sodium acetate (CH3CO2Na)   1c. Dibasic sodium phosphate dihydrate (Na2HPO4⋅2H2O) is one of the compounds you may consider using. When it is dissolved in water, which ions will be present in significant amounts in solution? Select all that apply. Na2^+   HPO4^-1   HPO4^-2   PO4^-1…

A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.010 M in NaF and 0.014 M in Ca(NO3)2. The following table shows Kp values for a number of compounds. Formula K CACO, 4.96 x 10 CaF2 1.46 x 10-10 Ca(OH); 4.68 x 106 PBCO, 7.40 x 10 14 PbF; 3.3 x 10 Pb(OH); 1.43 x 10 30 MgCOs 6.82 x 106 5.16 x 10-11

Calculate the solubility of silver phosphate, Ag3PO4 in units of grams per liter. Ksp (Ag3PO4) = 1.3x10-20. solubility g/L

Calculate the solubility of PbCrO4 in water at 25 °C. You'll find K data in the ALEKS Data tab. Round your answer to 2 significant digits. 3012 x10 X Ś

A 160.0 mL solution of 3.041 M strontium nitrate is mixed with 205.0 mL of a 3.340 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. Assuming complete precipitation, calculate the final concentration of each ion: [Na +] [NO3-] [Sr2+] [F-]. If the ion is no longer in solution, enter a 0 for the concentration.

Do not give handwriting solution.

you would like to remove cadmium ions from a waste stream using precipitation. The final concentration of cadmium needs to be less than 0.001 mg/L. identify a chemical that could be used to precipitate cadmium out of solution to meet this goal. Show calculations and prove if it can be calculated.

A solution contains 7.19×103 M potassium carbonate and 1.47×10-2 M potassium bromide. Solid silver nitrate is added slowly to this mixture. What is the concentration of bromide ion when carbonate ion begins to precipitate? [bromide] = | M

11b.