TTTT 3. You dissolve 25 grams of MgBr2 into 250 ml of water. • Calculate the formula mass of MgBr₂ Calculate the moles of MgBr₂ Calculate the volume of water in liters. .Write the balanced dissociation equation • Calculate the molarity of MgBr2 in the solution. • Calculate the molarity of the Mg2+ and Br in the solution. Formula Mass of MgBr2 = Moles MgBr2 = = Volume (1) = Dissociation Equation [MgBr₂] = [Mg2+] = [Br] = Answer Your calculations & equations

TTTT 3. You dissolve 25 grams of MgBr2 into 250 ml of water. • Calculate the formula mass of MgBr₂ Calculate the moles of MgBr₂ Calculate the volume of water in liters. .Write the balanced dissociation equation • Calculate the molarity of MgBr2 in the solution. • Calculate the molarity of the Mg2+ and Br in the solution. Formula Mass of MgBr2 = Moles MgBr2 = = Volume (1) = Dissociation Equation [MgBr₂] = [Mg2+] = [Br] = Answer Your calculations & equations

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section3.10: Solution Concentration: Molarity

Problem 3.24E

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Similar questions

A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?
What is the difference between a solute and a solvent?
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?
When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
Twenty-five mL of a 0.388 M solution of Na2SO4 is mixed with 35.3 mL of 0.229 M Na2SO4. What is the molarity of the resulting solution? Assume that the volumes are additive.
A common method for determining how much chloride ion is present in a sample is to precipitate the chloride from an aqueous solution of the sample with silver nitrate solution and then to weigh the silver chloride that results. The balanced net ionic reaction is :math>Ag+(aq)+Cl(aq)AgCl(s) ppose a 5.45-g sample of pure sodium chloride is dissolved in water and is then treated with a solution containing 1.15 g of silver nitrate. Will this quantity of silver nitrate be capable of precipitating all the chloride ion from the sodium chloride sample?
Citric 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?
Molarity is a conversion factor relating moles of solute in solution to the volume of the solution. How does one use molarity as a conversion factor to convert from moles of solute to volume of solution, and from volume of solution to moles of solute present?
3.86 When a solution is diluted, solvent is added but solute is not. Explain how this idea leads to the equation frequently used in dilution calculations, M1V1= M2V2.
A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, BaSO4. How many grams of barium ion are in a 458-mg sample of the barium compound if a solution of the sample gave 513 mg BaSO4 precipitate? What is the mass percentage of barium in the compound?
3.106 Twenty-five mL of a 0.388 M solution of Na2SO4 is mixed with 35.3 mL of 0.229 M Na2SO4. What is the molarity of the resulting solution? Assume that the volumes are additive.

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