9 Assignment 5-Chapter 2: End of Chapter QueetionsReferences)Question 41 ptThis question has multiple parts. Work all the parts to get the most points.Question 51 ptPotassium nitrate (KNO:) is used as a fertilizer for certain crops. It is produced through the reactionQuestion 6 O 1 pt4 KCI + 4 HNO; + 0, → 4 KNO, + 2 Cl, + 2 H;0Question 7 O pr1 ptQuestion 81 ptCalculate the minimum mass of KCl required to produce 557 g KNOS.1 ptQuestion 9Question 10 O 1 ptSubmitQuestion 11 1 ptQuestion 121 ptQuestion 131 ptSubmit AnswerTry Anothar Verslon10 Itam attampts ramainingQuestion 141 ptQuestion 151 ptQuestion 161 ptQuestion 171 prQuestion 181 prQuestion 191 ptQuestion 201 ptQuestion 211 ptQuestion 221 ptQuestion 231 ptQuestion 241 ptQuestion 251 pt

Mass of KNO3, Potassium Nitrate = 557 g Reaction:- 4KCl + 4HNO3 + O2 -----> 4KNO3 + 2Cl2 + 2H2O

End of Chapter Quetions References) This question has multiple parts. Work all the parts to get the most points. Potassium nitrate (KNO; ) is used as a fertilizer for certain crops. It is produced through the reaction 4 KCI+ 4 HNO; +0, → 4 KNO, + 2 C, + 2 H,0 Cakulate the minimum mess of KCl required to produce 557 g KNO,. Submit Submit Answor Try Anothar arsion 10 Itam attempts ramaining

End of Chapter Quetions References) This question has multiple parts. Work all the parts to get the most points. Potassium nitrate (KNO; ) is used as a fertilizer for certain crops. It is produced through the reaction 4 KCI+ 4 HNO; +0, → 4 KNO, + 2 C, + 2 H,0 Cakulate the minimum mess of KCl required to produce 557 g KNO,. Submit Submit Answor Try Anothar arsion 10 Itam attempts ramaining

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 6ALQ: onsider separate aqueous solutions of HCI and H2S04 with the same concentrations in terms of...

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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?
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.
3.14 A number of compounds are used in cement, and reactions among them occur when water is added. In one, CaO reacts with Al2O3 and water to form Ca3Al2(OH)12. Write a bal- anced chemical equation for this process.
It is stated in Section 6.3 of the text that to balance equations by inspection you start “with the most complicated molecule.” What does this mean? Why is it best to do this?
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.
onsider separate aqueous solutions of HCI and H2S04 with the same concentrations in terms of molarity. You wish to neutralize au aqueous solution of’ NaOH. For which acid solution would you need to add more volume (in mL) to neutralize the base? The HCI solution. The H2SO4 solution. You need to know the acid concentrations to answer this question. You need to know the volume and concentration of’ the NaOH solution to answer this question. c and d plain your answer.
4.59 Aluminum dissolves in HCI according to the equation written below, whereas copper does not react with HCl. 2Al( s )+6HCl( aq ) 2AlCl 3 ( aq )+ 3H 2 ( g ) A 35.0-g sample of a copper—aluminum alloy is dropped into 750 mL of 3.00 M HCl, and the reaction above proceeds as far as possible. If the ahoy contains 77.1% Al by mass, what mass of hydrogen gas would be produced?
You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of KIO3 that can be used.
When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2formed can be determined by the reaction with hydrogen peroxide: H2O2(aq)+SO2(g)H2SO4(aq) The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1 .302-g sample of coal is burned, and the SO2is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000 M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.
Potatoes can be peeled commercially by soaking them in a 3-M to 6-M solution of sodium hydroxide, then removing the loosened skins by spraying them with water. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to reach the end point?