A solution is known to contain 38.04 ± 0.03 mM KCl, and you have taken an aliquot of this solution using a pipette calibrated to deliver 20.013 ±0.006 m L. Determine the number of moles of KCl that are delivered in the aliquot, including the absolute uncertainly in that value.

Suppose 50.00 mL of 2.0 X 10–6 M T(NO3)3 is added to 50.00 mL of 2.0 X 10–4 M ZIO3.  Which of the following statements is true?  For T(IO3)3, Ksp = 1.0 X 10–14. Note:  T(NO3)3 and ZIO3 are nonexistent, ionic compounds. Group of answer choices A) A precipitate forms because Qc > Ksp. B) No precipitate forms because Qc > Ksp. C) A precipitate forms because Qc < Ksp. D) No precipitate forms because Qc < Ksp. E) No precipitate forms because Qc = Ksp.

4. A certain barium halide exists as the hydrated salt BaX2.2H2O, where X is the halogen. The barium content of the salt can be determined by gravimetric methods. A sample of the halide (0.2650 g) was dissolved in water (200 cm3) and excess sulfuric acid added. The mixture was then heated and held at boiling for 45 minutes. The precipitate (barium sulfate) was filtered off, washed and dried. Mass of precipitate obtained = 0.2533 § Determine the identity of X. 3 g.

Solubility Curves of Selected Compounds 150 140 130 120 110 100 NaNO 90 3 80 70 60 NHC 50 40 Naci 30 20 KCIÓ, 10 Ce(sO 20 30 40 50 60 70 80 90 100 Temperature (C) At one point, ammonia and potassium nitrate have the same solubility. At that point the solubility of the compounds is: O 77 g/100 g water O 44 g /100 g water O 40 g/ 100 g water O 25 g/100 g water 1 4 8. 9 DELL %23 Grams of solute

Calculate the maximum solubility of calcium fluoride, CaF2 in g/L when in the presence of 0.077 M Ca(NO3)2. The solubility product of CaF2 is 4.2x1011 and CaF2 has a molar mass of 78.08 g/mol. Express your answer to the correct number of significant figures, in scientific notation and include the unit with your answer.

The solubility product (Ksp) of Ca3(PO4)2 is 1.3 ×10. In a 0.02 M solution of Ca(NO3)2, the solubility of Ca3(PO4)2 (in units of M) is

2. A typical cup of tea (150.0 mL) is prepared. One teaspoon of glucose (C6H12O6; m.w. = 180.156 g mol-¹) is added (approximately 4.0 g of sugar). The resulting volume of solution is 152.6 mL, your standard cup of tea. Treating the sugar as the solute and the tea as water, the solvent. Calculate the following concentrations: a) M b) m c) % by mass d) mol fraction

10) How many miligrams of BaSO4 are dissolved in a 225 mL sample of BaSO4(aq)? (Hint: calculate the solubility of a slightly soluble solute) Ksp= 1.1x 10-10

Predict whether a lead (II) iodide precipitate will form when 325.0 mL of a 0.00350 mol/L aqueous solution of lead (II) nitrate, Pb(NO3)2 (aq), is mixed with 50.0 mL of a 0.00800 mol/L aqueous solution of sodium iodide, Nal (aq) (Ksp of lead (II) iodide = 8.5 x 10-⁹) UPLOAD A FULL SOLUTION WITH THE NECESSARY BALANCED CHEMICAL REACTION(S), CALCULATIONS, AND A FINAL ANSWER.

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