The student filters and dries the precipitate of CaCO3 (molar mass 100.1 g/mol) and records the data in thetable below.Measured QuantityValueVolume of Na,CO; solution50.0 mLVolume of 1.0 M Ca(NO;), added100.0 mLMass of CaCO; precipitate collected0.93 gc) Determine the number of moles of Na;CO; in the original 50.0 mL of solution.d) The student realizes that the precipitate was not completely dried and claims that as a result, the calculated Na,CO;molarity is too low. Do you agree with the student's claim? Justify your answer.After the precipitate forms and is filtered, the liquid that passed through the filter is tested to see if it can conduct electricity.What would be observed? Justify your answer. 30. A student is given 50.0 mL of a solution of Na,CO; of unknown concentration. To determine the concentration of thesolution, the student mixes the solution with excess 1.0 M Ca(NO:),(ag), causing a precipitate to form. The balancedequation for the reaction is shown below.NazCO3(ag) + Ca(NO:)2(aq) --------> 2 NANO3(ag) + CaCO:(s)a) Write the net ionic equation for the reaction that occurs when the solutions of Na,CO; and Ca(NO;), are mixed.b) The diagram below is incomplete. Draw in the species needed to accurately represent the major ionic species remainingin the solution after the reaction has been completed.(Na*)(NO,(NO,(Na*(NO,(NO,Solid CaCO3

#30: The balanced molecular equation is: Na2CO3(aq) + Ca(NO3)2(aq) ----> 2NaNO3(aq) + CaCO3(s)

30. A student is given 50.0 mL of a solution of Na,CO; of unknown concentration. To determine the concentration of the solution, the student mixes the solution with excess 1.0 M Ca(NO:),(ag), causing a precipitate to form. The balanced equation for the reaction is shown below. NazCOs(ag) + Ca(NO:)2(aq) --------> 2 NaNO:(aq) + CaCO:(s) a) Write the net ionic equation for the reaction that occurs when the solutions of Na,CO; and Ca(NO:); are mixed. b) The diagram below is incomplete. Draw in the species needed to accurately represent the major ionic species remaining in the solution after the reaction has been completed. (Na+ (NO, (NO, (Na (NO, (NO, Solid CaCO3

30. A student is given 50.0 mL of a solution of Na,CO; of unknown concentration. To determine the concentration of the solution, the student mixes the solution with excess 1.0 M Ca(NO:),(ag), causing a precipitate to form. The balanced equation for the reaction is shown below. NazCOs(ag) + Ca(NO:)2(aq) --------> 2 NaNO:(aq) + CaCO:(s) a) Write the net ionic equation for the reaction that occurs when the solutions of Na,CO; and Ca(NO:); are mixed. b) The diagram below is incomplete. Draw in the species needed to accurately represent the major ionic species remaining in the solution after the reaction has been completed. (Na+ (NO, (NO, (Na (NO, (NO, Solid CaCO3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 154CP: Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution:...

See similar textbooks

Similar questions

4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity is 1.37 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.23 per pound. (a) Write the balanced chemical equation for this process. (b) Determine the cost that the firm will incur from this use of slaked lime.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
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?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?
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?
There are many ionic compounds that dissolve in water to a very small extent. One example is lead(II) chloride. When it dissolves an equilibrium is established between the solid salt and its component ions. Suppose you stir some solid PbCl2 into water. Explain how you would prove that the compound dissolves but to a small extent? Is the dissolving process product-favored or reactant-favored? pbcl2(s)pb2+(aq)+2cl(aq)
The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to MnO2. A solution of H2SO4 and KI is then added to convert the MnO2 to Mn2+, and the iodide ion is converted to I2. The I2 is then titrated with standardized Na2S2O3. (a) Balance the equation for the reaction of Mn2+ ions with O2 in basic solution. (b) Balance the equation for the reaction of MnO2 with I in acid solution. (c) Balance the equation for the reaction of S2O32 with I2. (d) Calculate the amount of O2 in 25.0 mL of water if the titration requires 2.45 mL of 0.0112 M Na2S2O3 solution.