If 1.59 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample?

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?

A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?

The formation of water-Insoluble silver chloride is useful in the analysis of chloride-containing substances. Consider the following unbalanced equation: BaCl2(aq) + AgNO3(aq) AgCI(s) + Ba(NO3)2(aq) (a) Write the balanced equation. (b) What mass of AgNO3, in grams, is required for complete reaction with 0.156 g of BaCI2? What mass of AgCI is produced?

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.

Determine the volume of sulfuric acid solution needed to prepare 37.4 g of aluminum sulfate, Al2(SO4)3, by the reaction 2Al(s)+3H2SO4(aq)Al2(SO4)3(aq)+3H2(g) The sulfuric acid solution, whose density is 1.104 g/mL, contains 15.0% H2SO4 by mass.

Determine the volume of sodium hydroxide solution needed to prepare 26.2 g sodium phosphate, Na3PO4, by the reaction 3NaOH(aq)+H3PO4(aq)Na3PO4(aq)+3H2O(l) The sodium hydroxide solution, whose density is 1.133 g/mL, contains 12.0% NaOH by mass.

Lactic acid, C3H6O3 is the acid present in sour milk. A 0.100-g sample of pure lactic acid requires 12.95 mL of 0.0857 M sodium hydroxide for complete reaction. How many moles of hydroxide ion are required to neutralize one mole of lactic acid?

A mixture consisting of only sodium chloride (NaCl) andpotassium chloride (KCl) weighs 1.0000 g. When the mixtureis dissolved in water and an excess of silver nitrate isadded, all the chloride ions associated with the originalmixture are precipitated as insoluble silver chloride (AgCl).The mass of the silver chloride is found to be 2.1476 g.Calculate the mass percentages of sodium chloride andpotassium chloride in the original mixture.

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?