A10. 0.3455 g of A₂CO3 (A is an alkaline metal) was reacted with 50.0 mL 0.200 M hydrochloricacid (HCI) to form ACl(aq), H₂O(l) and CO₂(g): M₂CO3(aq)+2HCl(aq) → 2ACI(aq)+CO₂(g)+H₂O(l). The excess of HCI requires 50.0 mL of 0.100 M NaOH aqueous solution. Afterdetermining the molar mass of A₂CO3, identify A.A. LiB. CsD. NaE. RbC. K

Answered: Image /qna-images/answer/86fe6491-1688-42b3-a82c-ea142f55dca9.jpg

A10. 0.3455 g of A₂CO3 (A is an alkaline metal) was reacted with 50.0 mL 0.200 M hydrochloric acid (HCI) to form ACI(aq). H₂O(1) and CO₂(g): M₂CO3(aq)+2HCl(aq) → 2ACI(aq)+CO₂(g) +H₂O(1). The excess of HCI requires 50.0 mL of 0.100 M NaOH aqueous solution. After determining the molar mass of A₂CO3, identify A. A. Li B. Cs D. Na E. Rb C. K

A10. 0.3455 g of A₂CO3 (A is an alkaline metal) was reacted with 50.0 mL 0.200 M hydrochloric acid (HCI) to form ACI(aq). H₂O(1) and CO₂(g): M₂CO3(aq)+2HCl(aq) → 2ACI(aq)+CO₂(g) +H₂O(1). The excess of HCI requires 50.0 mL of 0.100 M NaOH aqueous solution. After determining the molar mass of A₂CO3, identify A. A. Li B. Cs D. Na E. Rb C. K

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) MnCl, (aq) + 2 H,0(1) + Cl, (g) How much MnO, (s) should be added to excess HCl(aq) to obtain 205 mL Cl, (g) at 25 °C and 805 Torr? mass of MnO,:
Commercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)4 (aq) + 3 H2 (g) If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?
25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction: K2S(aq) + 2HNO3(aq) → 2KNO3(aq) + H2S(g) The concentration of sulphide ion in the final solution is
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) MnCl, (aq) + 2 H,0(1) + Cl, (g) How much MnO, (s) should be added to excess HCl(aq) to obtain 205 mL CI, (g) at 25 °C and 735 Torr? mass of MnO2: g
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) - MnCl, (aq) + 2 H,O(1) + Cl, (g) How much Mn0, (s) should be added to excess HCI(aq) to obtain 235 mL Cl, (g) at 25 °C and 735 Torr? mass of MnO,: g
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 215 mL Cl2(g) at 25 °C and 765 Torr? mass of MnO2: ______________
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) → MNCI, (aq) + 2H,O(1) + CI, (g) How much MnO,(s) should be added to excess HCI(aq) to obtain 225 mL Cl, (g) at 25 °C and 765 Torr? mass of MnO,:
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5
What is the molarity of a hydrchloric acid, HCl, solution if it takes 26.90 mL of acid to neutralize 7.77 g of Fe(OH)3? The molar mass of Fe(OH)3 is 106.87 g/mol and the molar mass of HCl is 36.46 g/mol. The balanced chemical reaction is: 3 HCl (aq) + Fe(OH)3 (aq) → FeCl3 (aq) + 3 H2O (l)
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 285 mL Cl2(g) at 25 °C and 95 kPa?
For the chemical reaction HClO4(aq)+NaOH(aq)⟶H2O(l)+NaClO4(aq) write the net ionic equation, including the phases. Which ions are considered spectator ions for this reaction?
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 300.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 67.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.