-Part A What volume of 0.115 M HCIO4 solution is needed to neutralize 55.00 mL of 0.0890 M NaOH ? Express the volume in milliliters to two significant figures. V = Submit Request Answer mL Part B What volume of 0.120 M HCI is needed to neutralize 2.64 g of Mg(OH)2 ? Express the volume in liters to two significant figures. VN Submit Part C Request Answer L If 26.8 mL of an AgNO3 solution is needed to precipitate all the CI ions in a 760-mg sample of KC1 (forming AgCl), what is the molarity of the AgNO3 solution Express the molarity in the moles of a solute per liters of a solution to three significant figures. Molarity= Submit Part D VU Be <+ 10 = 17 Request Answer M If 45.9 mL of 0.120 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution? Express the mass in grams to three significant figures. 9 Submit Request Answer ? 8

-Part A What volume of 0.115 M HCIO4 solution is needed to neutralize 55.00 mL of 0.0890 M NaOH ? Express the volume in milliliters to two significant figures. V = Submit Request Answer mL Part B What volume of 0.120 M HCI is needed to neutralize 2.64 g of Mg(OH)2 ? Express the volume in liters to two significant figures. VN Submit Part C Request Answer L If 26.8 mL of an AgNO3 solution is needed to precipitate all the CI ions in a 760-mg sample of KC1 (forming AgCl), what is the molarity of the AgNO3 solution Express the molarity in the moles of a solute per liters of a solution to three significant figures. Molarity= Submit Part D VU Be <+ 10 = 17 Request Answer M If 45.9 mL of 0.120 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution? Express the mass in grams to three significant figures. 9 Submit Request Answer ? 8

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 38CR

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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?
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
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.
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
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.
A student wants to prepare 1.00 L of a 1.00-M solution of NaOH (molar mass = 40.00 g/mol). If solid NaOH is available, how would the student prepare this solution? If 2.00 M NaOH is available, how would the student prepare the solution? To help ensure three significant figures in the NaOH molarity, to how many significant figures should the volumes and mass be determined?
Two beakers sit on a balance; the total mass is 167.170 g. One beaker contains a solution of KI; the other contains a solution of Pb(NO3)2. When the solution in one beaker is poured completely into the other, the following reaction occurs: 2 KI(aq) + Pb(NO3)2(aq) 2 KNO3(aq) + PbI2(s) What is the total mass of the beakers and solutions after reaction? Explain completely.