50.00 cm3 of a 1.5784 mol.dm-3 solution of potassium hydroxide is transferred to an empty 700.00 cm3 volumetric flask. This flask is made up to the mark with distilled water and then shaken well. The concentration of the potassium hydroxide in this second flask is:

4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(1l) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) = Pb2+ (aq) +2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCI was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 2 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry A£CI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) CI- (aq) Pb2*(aq) [CI"] in PbCl2 solution, M [Pb2+] in PbCl, solution, M Ksp average Ksp solubility of PbCl2, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mL

Sodium nitrate contains 0.3% iodine in the form of calcium iodate, Ca(IO3)2. After the sodium nitrate in the niter is dissolved and recrystallized, the remaining solution contains 9 g/Lsodium iodate, NaIO3(aq). The NaIO3 is converted to iodine when it reactswith sulfur dioxide and water.2NaIO3 + 5SO2 + 4H2O → Na2SO4 + 4H2SO4 + I2a. How many liters of sodium iodate solution that contains 9 g of NaIO3 perliter would be necessary to form 127.23 kg of iodine, I2?

4. In a gravimetric determination of sulfur as BaSO4, 0.8863 g of the ignited precipitate is found to contain 7.71 mg of coprecipitated Na,SO4. Calculate the percentage error of the determination resulting from the presence of the Na,SO4-

0.376 grams of KHP are placed in an Erlenmeyer flask and some water and a drop of phenolphthalein is added to the flask.  The buret is filled with an NaOH (aq) solution of unknown concentration.  The NaOH solution is added dropwise to the flask containing KHP (aq).  After 12.78 mLs of the NaOH(aq) solution is added, the color of the solution is found to be faintly pink. What is the concentration (M) of the unknown NaOH solution based on this data alone?

A stock solution of Na2B having a concentration of 0.1486 M is used to prepare four calibration standards, A-D in the table below, by diluting the indicated volume of this solution to a total volume of 50.00 mL. Complete the table by entering the molarity of B2- for each standard solution. Show an illustrative calculation for tube ‘A’. Use the dilution formula and express each result to one more digit than allowed by applying the rules of significant figures.

Hydroxyapatite, Ca,(PO)(OH)₂, has a solubility constant of K-2.34 x 10-59, and dissociates according to Cao (PO)(OH)₂ (s) = 10 Ca² (aq) + 6PO (aq) + 2OH(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+ in this solution if JOH is fixed at 8.30 x 10M? |Ca²1 M

Construct the expression for Ksp for solid Ba³(PO4)2 in aqueous solution. Ba3(PO4)2(S) = 3 Ba²+(aq) + 2 PO4³-(aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one tile.. [Bas(PO4)2] [Ba²+] [PO4³-1² 2[Bas(PO4)2] 3[Ba²+] 3[PO4³] Ksp 3[Bas(PO4)2] [Ba²+]³ [PO4³-1³ = [Bas(PO4)2]² [PO4²-] [Bas(PO4)2]³ 2[PO4²-] [Bat] [PO4²-]² 3[Bat] [PO4³-] RESET [Ba+]³ 2[PO4³]

can be used as a standard solution for checking the concentration of a solution containing sulphuric acid, 8.7 cm' of sulphuric acid. Find the concentration of the sulphuric acid in both mol dm3 and g dm³. In a particular experiment 10,0 cm³ of a 0.50 mol dm³ solution of sodium ethanedioate was found to react with Q2. Sodium ethanedioate, Na;C¿O4, can be made into a solution of an exact and reliable concentration and so London ndon A.C.1.2

12a