(a)
Interpretation:
Appropriate reagent solution should be determined in order to separate cations from a mixture of
Concept introduction:
Solubility is a chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent.
Insoluble components precipitates from the solution.
(b)
Interpretation:
Appropriate reagent solution should be determined in order to separate cations from a mixture of
Concept introduction:
Solubility is a chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent.
Insoluble components precipitates from the solution.
(c)
Interpretation:
Appropriate reagent solution should be determined in order to separate cations from a mixture of
Concept introduction:
Solubility is a chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent.
Insoluble components precipitates from the solution.
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EBK GENERAL CHEMISTRY
- One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?arrow_forwardYou mix 25.0 mL of 0.234-M FeCl3 solution with 42.5 mL of 0.453-M NaOH. Calculate the maximum mass, in grams, of Fe(OH)3 that will precipitate. Determine which reactant is in excess. Calculate the concentration of the excess reactant remaining in solution after the maximum mass of Fe(OH)3 has precipitated.arrow_forwardDescribe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.arrow_forward
- A 8.50 g sample of KCl is dissolved in 66.0 mL of water. The resulting solution is then added to 72.0 mL of a 0.280 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution.arrow_forwardThe cations Ba2+ and Sr2+ can be precipitated as very insoluble sulfates. (a) If you add sodium sulfate to a solution containing these metal cations, each with a concentration of 0.10 M, which is precipitated first, BaSO4 or SrSO4? (b) What will be the concentration of the first ion that precipitates (Ba2+ or Sr2+) when the second, more soluble salt begins to precipitate?arrow_forwardSuppose 50.0 mL of 0.250 M CoCl2 solution is added to 25.0 mL of 0.350 M NiCl2 solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive.arrow_forward
- A 300.0-g sample of a solid is made up of a uniform mixture of NaNO3, MgCl2, and BaCl2. A 100.0-g sample of the mixture is dissolved in water and treated with an excess of KOH. The precipitate from the reaction has a mass of 13.47 g. The remaining 200.0-g sample is also dissolved in water and treated with an aqueous solution of AgNO3. The resulting precipitate has a mass of 195.8 g. What are the masses of NaNO3, MgCl2, and BaCl2 in the 300.0-g sample?arrow_forwardCitric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?arrow_forward42. 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.arrow_forward
- An aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.arrow_forwardAn aqueous sample is known to contain either Sr2+ or Hg22+ ions. Use the solubility rules (see Table 4.1) to propose an experiment that will determine which ion is present.arrow_forwardThe Behavior of Substances in Water Part 1: a Ammonia, NH3, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols. b From everyday experience you are probably aware that table sugar (sucrose), C12H22O11, is soluble in water. When sucrose dissolves in water, it doesnt form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water. c Both NH3 and C12H22O11 are soluble molecular compounds, yet they behave differently in aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte. d Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water. e Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes? f Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte. g Classify each of the following substances as either ionic or molecular. KCl NH3 CO2 MgBr2 HCl Ca(OH)2 PbS HC2H3O2 h For those compounds above that you classified as ionic, use the solubility rules to determine which are soluble. i The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water. j Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water? k How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer. l Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m Are NaCl and HI strong electrolytes because they have similar behavior in aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case. Part 2: You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water. AX(aq)+H2O(l)AH2O+(aq)+X(aq)AY(aq)+H2O(l)AH2O+(aq)+Y(aq) a Explain how the relative amounts of AX(aq) and AY(aq) would compare if you had a beaker of water with AX and a beaker of water with AY. b How would the relative amounts of X(aq) and Y(aq) in the two beakers compare? Be sure to explain your answer.arrow_forward
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