in another test, when the original solution is mixed with an aqueous solution of sodium sulfide no precipitate. A chemist needed a solution that was approximately 0.5 M in HCl but could measure only 10.00 mL samples into a 50.00 mL volumetric flask. What distinguishes a weak electrolyte from a strong electrolyte? Explain how an aqueous solution that is strongly basic can have a pH, which is a measure of the acidity of a solution. Which statement is correct? KNO3 2. Predict whether mixing each pair of solutions will result in the formation of a precipitate. If the calcium oxide were obtained by the heating of calcium hydroxide, how much hydroxide would be needed to obtain the 15.0 g? 10.

When an aqueous solution suspected of containing Ba2+ or Pb2+ or both are mixed with sulfuric acid a precipitate forms. A solution of silver nitrate is dropped onto an aluminum plate.

Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO3)3? If a solution has a Ca(OCl)2 concentration of 3.4 g per 100 mL of solution, what is the molarity of hypochlorite? As the filling hardens, the gas can be released, causing pain and cracking the tooth. Write the balanced chemical equation for each reaction. Given the following salts, identify the acid and the base in the neutralization reactions and then write the complete ionic equation: What is the hydrogen ion concentration of each substance in the indicated pH range? How many milliliters of 0.223 M NaOH are needed to neutralize 25.00 mL of this final solution? Have questions or comments?

23. aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. What has been reduced? An electrolyte is any compound that can form ions when it dissolves in water. What are the advantages of using solutions for quantitative calculations? barium hydroxide 1. Here it is again in case you misplaced it. Propose a method for preparing the solution. A student was titrating 25.00 mL of a basic solution with an HCl solution that was 0.281 M. The student ran out of the HCl solution after having added 32.46 mL, so she borrowed an HCl solution that was labeled as 0.317 M. An additional 11.5 mL of the second solution was needed to complete the titration. oxalic acid c.) chlorous acid d.) nitric acid 2.

One graph corresponds to the titration of 100 mL 0.10 M Ba(OH)2 with 0.10 M H2SO4 , and the other corresponds to the titration of 100 mL of 0.10 M NaOH with 0.10 M H2SO4. When potassium chloride is added to the solution, a precipitate forms. Which elements in the periodic table tend to be good oxidants? How does this distribution affect its physical properties? What types of compounds dissolve in polar solvents?

Predict whether each compound will dissolve in water and explain why. (Assume the density of the solution is 1.00 g/mL.). Of water and toluene, predict which is the better solvent for each compound and explain your reasoning. Acetic acid contains a carboxylic acid group attached to a small alkyl group (a methyl group). KCl 3. A. You must tell the technician how to separate these three compounds from the mixture. Suggest a method for separating these three compounds. A strip of zinc is placed into a solution of HCl. If the ΔH for: CaC2(s) + 2H2O(l) = Ca(OH)2(s) + C2H2(g) is -127 kJ, then what is the enthalpy of formation for calcium, 10. A laboratory technician is given a sample that contains only sodium chloride, sucrose, and cyclodecanone (a ketone). Justify your answer. What do you predict if one is a strong oxidant and the other is a weak reductant? What is the pH of a solution prepared by diluting 25.00 mL of 0.879 M HCl to a volume of 555 mL?

1.00 M solution: dilute 41.20 mL of the concentrated solution to a final volume of 500 mL. Classify each compound as a strong acid, a weak acid, a strong base, or a weak base in aqueous solution. Give a plausible reason for this practice. Aluminum sulfate reacts with calcium hydroxide (from lime) to form aluminum hydroxide and calcium sulfate. If a patient has a prescribed dose of 900.0 mg, how many milliliters of the solution should be administered? $$2H^+ + 2NO_3^- + Ca^{2+} + 2OH^- \rightarrow Ca^{2+} + 2NO_3^- + H_2O$$ 4.7: Reactions in Aqueous Solution (Exercises), [ "article:topic", "showtoc:no", "license:ccbyncsa", "source-chem-24803" ], by Brown, LeMay, Busten, Murphy, and Woodward, 4.6: Solution Stoichiometry and Chemical Analysis, 4.8: Reactions in Aqueous Solution (Summary), 4.1: General Properties of Aqueous Solutions. Describe the charge distribution in liquid water. What are the concentrations of calcium and sulfate after equilibrium is reached? (In fact, the solubility of both butanol and pentanoic acid in water is quite low, only about 3 g per 100 g water at 25°C. how many grams of aluminum sulfate would be formed if 250g H2SO4 reacted with aluminum? When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. What is the complete ionic equation for each reaction? Under what circumstances is one of the products a gas? Identify the acid and the base in this reaction. Write the chemical formula for each of the following acids: a.) Vinegar is primarily an aqueous solution of acetic acid. The titration procedure is an application of the use of limiting reactants.

What are the advantages to carrying out a reaction in solution rather than simply mixing the pure reactants? If 20.0 mL of 0.10 M NaOH are needed to neutralize 15.0 mL of gastric fluid, what is the molarity of HCl in the fluid? Justify your answers. The precipitate is filtered off and potassium sulfate is added to the remaining. Classify each reaction as an acid–base reaction, a precipitation reaction, or a redox reaction, or state if there is no reaction; then complete and balance the chemical equation: Which of the representations best corresponds to a 1 M aqueous solution of each compound? Why? Register now! If a reaction occurs, write the net ionic equation; then write the complete ionic equation for the reaction. 1.40 L of a 0.334 M solution or 1.10 L of a 0.420 M solution, 25.0 mL of a 0.134 M solution or 10.0 mL of a 0.295 M solution, 250 mL of a 0.489 M solution or 150 mL of a 0.769 M solution, 1.045 mol of magnesium bromide in 500 mL of solution, 0.146 mol of glucose in 800 mL of solution, 0.528 mol of potassium formate in 300 mL of solution, 0.378 mol of potassium iodide in 750 mL of solution, 8.7 g of calcium bromide in 250 mL of solution, 9.8 g of lithium sulfate in 300 mL of solution, 14.2 g of iron(III) nitrate hexahydrate in 300 mL of solution, 12.8 g of sodium hydrogen sulfate in 400 mL of solution, 7.5 g of potassium hydrogen phosphate in 250 mL of solution, 11.4 g of barium chloride in 350 mL of solution.
When potassium chloride is added to the solution, a precipitate forms. How many moles of solute are contained in each? The temp is 25 degrees Celsius.
Jai Ambe Gauri Book, How To Cancel Revive Superfoods, Shaft Driver Taylormade, Mini Goldendoodle Puppies For Sale Near Me, Yves Veggie Nuggets Costco, Jupyter Notebook Invalid Syntax, Reverse Counterbore Tool, Lion Rampant Army Lists, Series 8 Fitness Ball Inflation, Subnautica How To Cure Infection Cheat, The Suite Life Of Zack Cody Season 1 Episode 24, Sibling Names That Go With Oliver, Bdo Best Carrack, Marin Terra Linda 2, Kathy Ambush Wikipedia, Shiny Diamond Font Generator, How Did Ray Bolger Die, Betty Hawley Kelso, Simple Man Tabs Easy, Death Ann Serrano, Jacob Blyth Net Worth, Elegoo Mars Pro, Commencal Meta Ht Am Origin 2019, Warru By Jack Davis, Sathya Episode 28, Kyani Pyramid Scheme, Sonic Riders Zero Gravity Ps2 Iso, Pioneer Uk Dj, Prince Joseph Wenzel Of Liechtenstein Instagram, Nrg Unknown Height, Madelyn Cline Address, Stronger Than You Parodies, " />
in another test, when the original solution is mixed with an aqueous solution of sodium sulfide no precipitate. A chemist needed a solution that was approximately 0.5 M in HCl but could measure only 10.00 mL samples into a 50.00 mL volumetric flask. What distinguishes a weak electrolyte from a strong electrolyte? Explain how an aqueous solution that is strongly basic can have a pH, which is a measure of the acidity of a solution. Which statement is correct? KNO3 2. Predict whether mixing each pair of solutions will result in the formation of a precipitate. If the calcium oxide were obtained by the heating of calcium hydroxide, how much hydroxide would be needed to obtain the 15.0 g? 10.

When an aqueous solution suspected of containing Ba2+ or Pb2+ or both are mixed with sulfuric acid a precipitate forms. A solution of silver nitrate is dropped onto an aluminum plate.

Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO3)3? If a solution has a Ca(OCl)2 concentration of 3.4 g per 100 mL of solution, what is the molarity of hypochlorite? As the filling hardens, the gas can be released, causing pain and cracking the tooth. Write the balanced chemical equation for each reaction. Given the following salts, identify the acid and the base in the neutralization reactions and then write the complete ionic equation: What is the hydrogen ion concentration of each substance in the indicated pH range? How many milliliters of 0.223 M NaOH are needed to neutralize 25.00 mL of this final solution? Have questions or comments?

23. aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. What has been reduced? An electrolyte is any compound that can form ions when it dissolves in water. What are the advantages of using solutions for quantitative calculations? barium hydroxide 1. Here it is again in case you misplaced it. Propose a method for preparing the solution. A student was titrating 25.00 mL of a basic solution with an HCl solution that was 0.281 M. The student ran out of the HCl solution after having added 32.46 mL, so she borrowed an HCl solution that was labeled as 0.317 M. An additional 11.5 mL of the second solution was needed to complete the titration. oxalic acid c.) chlorous acid d.) nitric acid 2.

One graph corresponds to the titration of 100 mL 0.10 M Ba(OH)2 with 0.10 M H2SO4 , and the other corresponds to the titration of 100 mL of 0.10 M NaOH with 0.10 M H2SO4. When potassium chloride is added to the solution, a precipitate forms. Which elements in the periodic table tend to be good oxidants? How does this distribution affect its physical properties? What types of compounds dissolve in polar solvents?

Predict whether each compound will dissolve in water and explain why. (Assume the density of the solution is 1.00 g/mL.). Of water and toluene, predict which is the better solvent for each compound and explain your reasoning. Acetic acid contains a carboxylic acid group attached to a small alkyl group (a methyl group). KCl 3. A. You must tell the technician how to separate these three compounds from the mixture. Suggest a method for separating these three compounds. A strip of zinc is placed into a solution of HCl. If the ΔH for: CaC2(s) + 2H2O(l) = Ca(OH)2(s) + C2H2(g) is -127 kJ, then what is the enthalpy of formation for calcium, 10. A laboratory technician is given a sample that contains only sodium chloride, sucrose, and cyclodecanone (a ketone). Justify your answer. What do you predict if one is a strong oxidant and the other is a weak reductant? What is the pH of a solution prepared by diluting 25.00 mL of 0.879 M HCl to a volume of 555 mL?

1.00 M solution: dilute 41.20 mL of the concentrated solution to a final volume of 500 mL. Classify each compound as a strong acid, a weak acid, a strong base, or a weak base in aqueous solution. Give a plausible reason for this practice. Aluminum sulfate reacts with calcium hydroxide (from lime) to form aluminum hydroxide and calcium sulfate. If a patient has a prescribed dose of 900.0 mg, how many milliliters of the solution should be administered? $$2H^+ + 2NO_3^- + Ca^{2+} + 2OH^- \rightarrow Ca^{2+} + 2NO_3^- + H_2O$$ 4.7: Reactions in Aqueous Solution (Exercises), [ "article:topic", "showtoc:no", "license:ccbyncsa", "source-chem-24803" ], by Brown, LeMay, Busten, Murphy, and Woodward, 4.6: Solution Stoichiometry and Chemical Analysis, 4.8: Reactions in Aqueous Solution (Summary), 4.1: General Properties of Aqueous Solutions. Describe the charge distribution in liquid water. What are the concentrations of calcium and sulfate after equilibrium is reached? (In fact, the solubility of both butanol and pentanoic acid in water is quite low, only about 3 g per 100 g water at 25°C. how many grams of aluminum sulfate would be formed if 250g H2SO4 reacted with aluminum? When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. What is the complete ionic equation for each reaction? Under what circumstances is one of the products a gas? Identify the acid and the base in this reaction. Write the chemical formula for each of the following acids: a.) Vinegar is primarily an aqueous solution of acetic acid. The titration procedure is an application of the use of limiting reactants.

What are the advantages to carrying out a reaction in solution rather than simply mixing the pure reactants? If 20.0 mL of 0.10 M NaOH are needed to neutralize 15.0 mL of gastric fluid, what is the molarity of HCl in the fluid? Justify your answers. The precipitate is filtered off and potassium sulfate is added to the remaining. Classify each reaction as an acid–base reaction, a precipitation reaction, or a redox reaction, or state if there is no reaction; then complete and balance the chemical equation: Which of the representations best corresponds to a 1 M aqueous solution of each compound? Why? Register now! If a reaction occurs, write the net ionic equation; then write the complete ionic equation for the reaction. 1.40 L of a 0.334 M solution or 1.10 L of a 0.420 M solution, 25.0 mL of a 0.134 M solution or 10.0 mL of a 0.295 M solution, 250 mL of a 0.489 M solution or 150 mL of a 0.769 M solution, 1.045 mol of magnesium bromide in 500 mL of solution, 0.146 mol of glucose in 800 mL of solution, 0.528 mol of potassium formate in 300 mL of solution, 0.378 mol of potassium iodide in 750 mL of solution, 8.7 g of calcium bromide in 250 mL of solution, 9.8 g of lithium sulfate in 300 mL of solution, 14.2 g of iron(III) nitrate hexahydrate in 300 mL of solution, 12.8 g of sodium hydrogen sulfate in 400 mL of solution, 7.5 g of potassium hydrogen phosphate in 250 mL of solution, 11.4 g of barium chloride in 350 mL of solution.
When potassium chloride is added to the solution, a precipitate forms. How many moles of solute are contained in each? The temp is 25 degrees Celsius.
Jai Ambe Gauri Book, How To Cancel Revive Superfoods, Shaft Driver Taylormade, Mini Goldendoodle Puppies For Sale Near Me, Yves Veggie Nuggets Costco, Jupyter Notebook Invalid Syntax, Reverse Counterbore Tool, Lion Rampant Army Lists, Series 8 Fitness Ball Inflation, Subnautica How To Cure Infection Cheat, The Suite Life Of Zack Cody Season 1 Episode 24, Sibling Names That Go With Oliver, Bdo Best Carrack, Marin Terra Linda 2, Kathy Ambush Wikipedia, Shiny Diamond Font Generator, How Did Ray Bolger Die, Betty Hawley Kelso, Simple Man Tabs Easy, Death Ann Serrano, Jacob Blyth Net Worth, Elegoo Mars Pro, Commencal Meta Ht Am Origin 2019, Warru By Jack Davis, Sathya Episode 28, Kyani Pyramid Scheme, Sonic Riders Zero Gravity Ps2 Iso, Pioneer Uk Dj, Prince Joseph Wenzel Of Liechtenstein Instagram, Nrg Unknown Height, Madelyn Cline Address, Stronger Than You Parodies, " />

# a solution of calcium hydroxide is added to a solution of potassium sulfate

Which organic groups result in aqueous solutions that conduct electricity? How many grams of zinc(II) nitrate and sodium sulfide were consumed to produce this quantity of product?

Must a molecule have an asymmetric charge distribution to be polar? Complete the following table for 500 mL of solution. The alkyl group is rather large, consisting of a 4-carbon chain. Free LibreFest conference on November 4-6! K2SO4 4.

A solution of copper(II) sulfate is added to a solution of barium hydroxide. The precipitate is filtered off and potassium sulfate is added to the remaining . When potassium chloride is added to the solution, a precipitate forms.

You can view more similar questions or ask a new question.

Balance each redox reaction under the conditions indicated. In this subset, what is oxidized and what is reduced? Commercial vinegar typically contains 5.0 g of acetic acid in 95.0 g of water. Which representation in Problem 3 best corresponds to an aqueous solution originally containing each of the following? What specific point does the Brønsted–Lowry definition address? If an amalgam contains zinc, however, water can contaminate the amalgam as it is being manipulated, producing hydrogen gas under basic conditions. Which of the following is a strong electrolyte, a weak electrolyte, or a nonelectrolyte in an aqueous solution? 0.13 M HCl; magnesium carbonate, MgCO3, or aluminum hydroxide, Al(OH)3. 1) Sodium reacts with iron(lll)oxide to produce sodium oxide and iron. Derive an equation to relate the hydroxide ion concentration to the molarity of a solution of. Malonic acid is a dicarboxylic acid; propose a structure for malonic acid. wrong reason. Write the balanced chemical equation for each of these reactions. Which graph corresponds to which titration? What information can be obtained from a complete ionic equation that cannot be obtained from the overall chemical equation? How many moles of NaOH are needed for the neutralization? In addition to these publicly available questions, access to private problems bank for use in exams and homework is available to faculty only on an individual basis; please contact Delmar Larsen for an account with access permission. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739.

The first sample does not dissolve in water, the second sample dissolves only slightly in ethanol, and the third sample dissolves completely in toluene. If the amount of a substance required for a reaction is too small to be weighed accurately, the use of a solution of the substance, in which the solute is dispersed in a much larger mass of solvent, allows chemists to measure the quantity of the substance more accurately. The other product is water. $$H^+ + I^- + Cs^+ + OH^- \rightarrow Cs^+ + I^- + H_2O$$. Please be sure you are familiar with the topics discussed in Essential Skills 3 (section 4.1 "Aqueous Solutions"0) before proceeding to the Numerical Problems. Calcium carbide (CaC2) reacts with water to form acetylene (C2H2) gas and calcium hydroxide (Ca(OH)2). When a strong electrolyte dissolves in water, it dissociates completely to give the constituent ions. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. Why or why not? If the 15.0 g of calcium oxide in the above problems were allowed to react with water, what, I really need help for my homework on how to write the balanced equation for the following reactions. A neutralization reaction gives calcium nitrate as one of the two products. Explain your reasoning.

in another test, when the original solution is mixed with an aqueous solution of sodium sulfide no precipitate. A chemist needed a solution that was approximately 0.5 M in HCl but could measure only 10.00 mL samples into a 50.00 mL volumetric flask. What distinguishes a weak electrolyte from a strong electrolyte? Explain how an aqueous solution that is strongly basic can have a pH, which is a measure of the acidity of a solution. Which statement is correct? KNO3 2. Predict whether mixing each pair of solutions will result in the formation of a precipitate. If the calcium oxide were obtained by the heating of calcium hydroxide, how much hydroxide would be needed to obtain the 15.0 g? 10.

When an aqueous solution suspected of containing Ba2+ or Pb2+ or both are mixed with sulfuric acid a precipitate forms. A solution of silver nitrate is dropped onto an aluminum plate.

Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO3)3? If a solution has a Ca(OCl)2 concentration of 3.4 g per 100 mL of solution, what is the molarity of hypochlorite? As the filling hardens, the gas can be released, causing pain and cracking the tooth. Write the balanced chemical equation for each reaction. Given the following salts, identify the acid and the base in the neutralization reactions and then write the complete ionic equation: What is the hydrogen ion concentration of each substance in the indicated pH range? How many milliliters of 0.223 M NaOH are needed to neutralize 25.00 mL of this final solution? Have questions or comments?

23. aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. What has been reduced? An electrolyte is any compound that can form ions when it dissolves in water. What are the advantages of using solutions for quantitative calculations? barium hydroxide 1. Here it is again in case you misplaced it. Propose a method for preparing the solution. A student was titrating 25.00 mL of a basic solution with an HCl solution that was 0.281 M. The student ran out of the HCl solution after having added 32.46 mL, so she borrowed an HCl solution that was labeled as 0.317 M. An additional 11.5 mL of the second solution was needed to complete the titration. oxalic acid c.) chlorous acid d.) nitric acid 2.

One graph corresponds to the titration of 100 mL 0.10 M Ba(OH)2 with 0.10 M H2SO4 , and the other corresponds to the titration of 100 mL of 0.10 M NaOH with 0.10 M H2SO4. When potassium chloride is added to the solution, a precipitate forms. Which elements in the periodic table tend to be good oxidants? How does this distribution affect its physical properties? What types of compounds dissolve in polar solvents?

Predict whether each compound will dissolve in water and explain why. (Assume the density of the solution is 1.00 g/mL.). Of water and toluene, predict which is the better solvent for each compound and explain your reasoning. Acetic acid contains a carboxylic acid group attached to a small alkyl group (a methyl group). KCl 3. A. You must tell the technician how to separate these three compounds from the mixture. Suggest a method for separating these three compounds. A strip of zinc is placed into a solution of HCl. If the ΔH for: CaC2(s) + 2H2O(l) = Ca(OH)2(s) + C2H2(g) is -127 kJ, then what is the enthalpy of formation for calcium, 10. A laboratory technician is given a sample that contains only sodium chloride, sucrose, and cyclodecanone (a ketone). Justify your answer. What do you predict if one is a strong oxidant and the other is a weak reductant? What is the pH of a solution prepared by diluting 25.00 mL of 0.879 M HCl to a volume of 555 mL?

1.00 M solution: dilute 41.20 mL of the concentrated solution to a final volume of 500 mL. Classify each compound as a strong acid, a weak acid, a strong base, or a weak base in aqueous solution. Give a plausible reason for this practice. Aluminum sulfate reacts with calcium hydroxide (from lime) to form aluminum hydroxide and calcium sulfate. If a patient has a prescribed dose of 900.0 mg, how many milliliters of the solution should be administered? $$2H^+ + 2NO_3^- + Ca^{2+} + 2OH^- \rightarrow Ca^{2+} + 2NO_3^- + H_2O$$ 4.7: Reactions in Aqueous Solution (Exercises), [ "article:topic", "showtoc:no", "license:ccbyncsa", "source-chem-24803" ], by Brown, LeMay, Busten, Murphy, and Woodward, 4.6: Solution Stoichiometry and Chemical Analysis, 4.8: Reactions in Aqueous Solution (Summary), 4.1: General Properties of Aqueous Solutions. Describe the charge distribution in liquid water. What are the concentrations of calcium and sulfate after equilibrium is reached? (In fact, the solubility of both butanol and pentanoic acid in water is quite low, only about 3 g per 100 g water at 25°C. how many grams of aluminum sulfate would be formed if 250g H2SO4 reacted with aluminum? When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. What is the complete ionic equation for each reaction? Under what circumstances is one of the products a gas? Identify the acid and the base in this reaction. Write the chemical formula for each of the following acids: a.) Vinegar is primarily an aqueous solution of acetic acid. The titration procedure is an application of the use of limiting reactants.

What are the advantages to carrying out a reaction in solution rather than simply mixing the pure reactants? If 20.0 mL of 0.10 M NaOH are needed to neutralize 15.0 mL of gastric fluid, what is the molarity of HCl in the fluid? Justify your answers. The precipitate is filtered off and potassium sulfate is added to the remaining. Classify each reaction as an acid–base reaction, a precipitation reaction, or a redox reaction, or state if there is no reaction; then complete and balance the chemical equation: Which of the representations best corresponds to a 1 M aqueous solution of each compound? Why? Register now! If a reaction occurs, write the net ionic equation; then write the complete ionic equation for the reaction. 1.40 L of a 0.334 M solution or 1.10 L of a 0.420 M solution, 25.0 mL of a 0.134 M solution or 10.0 mL of a 0.295 M solution, 250 mL of a 0.489 M solution or 150 mL of a 0.769 M solution, 1.045 mol of magnesium bromide in 500 mL of solution, 0.146 mol of glucose in 800 mL of solution, 0.528 mol of potassium formate in 300 mL of solution, 0.378 mol of potassium iodide in 750 mL of solution, 8.7 g of calcium bromide in 250 mL of solution, 9.8 g of lithium sulfate in 300 mL of solution, 14.2 g of iron(III) nitrate hexahydrate in 300 mL of solution, 12.8 g of sodium hydrogen sulfate in 400 mL of solution, 7.5 g of potassium hydrogen phosphate in 250 mL of solution, 11.4 g of barium chloride in 350 mL of solution.
When potassium chloride is added to the solution, a precipitate forms. How many moles of solute are contained in each? The temp is 25 degrees Celsius.

Questo sito si serve dei cookie di Google per l'erogazione dei servizi, la personalizzazione degli annunci e l'analisi del traffico. Le informazioni sul tuo utilizzo del sito sono condivise con Google. Se prosegui la navigazione acconsenti all'utilizzo dei cookie. più info

Questo sito utilizza i cookie per fonire la migliore esperienza di navigazione possibile. Continuando a utilizzare questo sito senza modificare le impostazioni dei cookie o clicchi su "Accetta" permetti al loro utilizzo.

Chiudi