A 185.0 mL sample of 1.200 M Pb(NO3)2 is mixed with 123.50 mL of 1.500 M NaCI, and the PbCl2 precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr, precipitate is also collected and dried. What is the mass (in grams) of the PbBr2 precipitate, assuming the yield in each precipitation step is 100%?

The solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp. If only 0.251 g of Ca(OH)2 dissolves in enough water to give 0.204 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?

Solid potassium hydroxide is slowly added to 150 mL of a 0.0538 M iron(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is  M.

Excess solid Ni(OH)2 was added to water and the resulting solution was allowed to stand for several days. The solution was then filtered to remove excess solid Ni(OH)2. A 0.250 L aliquot of the solution was then titrated with 10.54 mL of a standardized 0.000500 M HCl solution. What is the Ksp of Ni(OH)2?

A solution is prepared by adding 150.0 mL of a 0.0100 M Mg(NO3)2 solution to 250.0 mL of a 0.100 M NaF solution. Will anything precipitate from this solution and, if so, what is the precipitate?   a. No, nothing will precipitate.   b. Yes, MgF 2   c. There is not enough information to answer this question.   d. Yes, Mg(NO 3 ) 2   e. Yes, NaNO 3

Solid lead acetate is slowly added to 125 mL of a 0.0470 M ammonium bromide solution. The concentration of lead ion required to just initiate precipitation is M.

Silver chromate is sparingly soluble in aqueous solutions. The ?sp of Ag2CrO4 is 1.12×10−12 M^3 What is the solubility (in moles per liter) of silver chromate in a 1.10 M silver nitrate aqueous solution? M=

Will a precipitate of SrF2 form if you mix 25 mL of 7.1 x 10^-2 M Sr(NO3)2 (aq) with 85 mL of 3.2 x 10^-3 M NaF (aq)?

Solid ammonium fluoride is slowly added to 175 mL of a 0.0682 M lead nitrate solution. The concentration of fluoride ion required to just initiate precipitation is M.

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)