Question 2I2.1The Ksp of Ca3(PO4), is 1.3 × 10-26. Estimate the solubility of this salt in units of g. L-1.You must show any reaction equation(s) that you may think are necessary.If a sample of solid Ca (PO,)2 is stirred into exactly one litre of a 0.550M solution of Na P04,how will the solubility of the salt compare with the answer that you have obtained in question2.1? Explain you answer in a short sentence.2.2

Given: Ksp of Ca3(PO4)2 = 1.3x 10-26

Answered: Question 2 2.1 The Ksp of Ca3 (PO4), is…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 53QAP: The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The...

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Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
For a product to be called vinegar, it must contain at least 5.0% acetic acid, HC2H3O2, by mass. A 10.00-g sample of a raspberry vinegar is titrated with 0.1250 M Ba(OH)2 and required 37.50 mL for complete neutralization. Can the product be called a vinegar?
In order to determine the purity of ammonium sulfate, a sample with a mass of 0.850 g is dissolved in KOH. The equation for the reaction that takes place is NH4+(aq)+OH(aq)NH3(aq)+H2OThe ammonia liberated is distilled into a flask that contains 50.00 mL of 0.250 M HCI. Not all the HCI is consumed. The excess HCI reacts with 17.3 mL of 0.120 M NaOH. What is the mass percent of (NH4)2SO4 in the sample?
An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.
4-33 When a solution of hydrochloric acid, HCl, is added to a solution of sodium sulfite, Na.2S03, sulfur dioxide gas is released from the solution. Write a net ionic equation for this reaction. An aqueous solution of HCl contains H+ and Cl- ions, and Na2SO3 exists as dissociated ions in aqueous solution.
A sample of limestone weighing 1.005 g is dissolved in 75.00 mL of 0.2500 M hydrochloric acid. The following reaction occurs: CaCO3(s)+2 H+(aq)Ca2+(aq)+CO2(g)+H2O It is found that 19.26 mL of 0.150 M NaOH is required to titrate the excess HCI left after reaction with the limestone. What is the mass percent of CaCO3 in the limestone?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The unbalanced equation for the reaction is H3AsO3(aq)+I2(aq)+H2O2 I(aq)+H3AsO4(aq)+2 H+(aq)A 243-mL solution of aqueous iodine is prepared by dissolving iodine crystals in water. A fifty-mL portion of the solution requires 15.42 mL of 0.134 M H3AsO3 for complete reaction. What is the molarity of the solution? How many grams of iodine were added to the solution?
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
Oranges and grapefruits are known as citrus fruits because their acidity comes mainly from citric acid, H3C6H5O7. Calculate the concentration of citric acid in a solution if a 30.00-mL sample is neutralized by 15.10 mL of 0.0100 M KOH. Assume that three acidic hydrogens of each citric acid molecule are neutralized in the reaction.

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