Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by aprocess called liming, in which limestone(CaCO3) is added to the acidified water.Constants | Periodic TablePart AWhat mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is1 9x10-5 M in H, SO, and 8,9x10-6 M in HN03?Express your answer using two significant figures.?kgSubmitPrevious Answers Request AnswerIncorrect; Try Again: 29 attempts remainingNext >Provide FeedbackP PearsonCopyright © 2021 Pearson Education Inc. All rights reserved. Ierms of Use | Privacy Policy | Permissions I Contact Us I0 11:27

The question is based on the concept of reaction stoichiometry. We have to calculate mass of calcium…

Lakes that have been acidified by acid rain ( HNO3 and Ha SO4) can be neutralized by a process called liming, in which limestone (CaCO3) is added to the acidified water. Constanta I Periodic Table Part A What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 19x10-5 M in H,SO, and 8.9x10-6 M in HNO3? Express your answer using two significant figures. O回 ? m 3= kg Submit Previous Answers Request Answer Incorrect; Try Again; 29 attempts remaining Next> Provide Feedback Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use Privacy Pollcy | Permissions I Contact Us O 11:27

Lakes that have been acidified by acid rain ( HNO3 and Ha SO4) can be neutralized by a process called liming, in which limestone (CaCO3) is added to the acidified water. Constanta I Periodic Table Part A What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 19x10-5 M in H,SO, and 8.9x10-6 M in HNO3? Express your answer using two significant figures. O回 ? m 3= kg Submit Previous Answers Request Answer Incorrect; Try Again; 29 attempts remaining Next> Provide Feedback Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use Privacy Pollcy | Permissions I Contact Us O 11:27

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. Zinc reacts with hydrochloric acid to make zinc chloride and hydrogen. Zn + HCI 220g elain what will happen to the mass of the flask and its contents as the reaction proceeds.
Suppose the following reaction was carried out in the presence of excess Al. Al + Cl2 ---> AlCl3 How many moles of Al are consumed if 9.07 moles of Cl2 were fully reacted?
4. An old antacid commercial claimed that each tablet of their product could "neutralize 47 times its mass in stomach acid". The active ingredient in the antiacid tablet, NaAl(OH)₂CO3, reacts with HCl in stomach acid according to this balanced reaction: NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl³ + 3 H₂O + CO₂ How many moles of HCl can a 1.03 g of antiacid tablet neutralize if the tablet contains 0.246 g of the active ingredient? If stomach acid has a concentration of 0.14 M HCl, assuming the density of stomach acid to be similar to that of water (1.00 g/mL), what is the mass of stomach acid that the 1.03 g of antiacid tablet can neutralize? Does this number support the claim in the commercial?
7) The reaction HNO3(aq) + NaOH(aq) NaN03(aq) + H2O() is an example of A) an acid-base reaction B) a precipitation reaction C) a combustion reaction 8) Which is the correct balanced reaction for the combustion of octane? A) C8H18(g) + 12.502(g) → 8CO2(g) + 9H2O(g) B) C8H18(g) + 250(g) → 8CO2(g) + 9H2O(g) C) 2C8H18(g) + 2502(g) → 16CO2(g) + 18H2O(g)
O Chemical Reactions Solving for a reactant in solution 0/5 Bis One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200. mL sample of groundwater known to be contaminated with iron(II) chloride, which would react with silver nitrate solution like this: FeCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Fe(NO3)2(aq) The chemist adds 72.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 5.9 mg of silver chloride. Calculate the concentration of iron(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg X 5
Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. LiCI(aq) + K:PO:(aq) –
If 23.1 g of NaOH (MM = 40.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of NaOH in the resulting solution? What quantity in moles of NaI are in 55.8 grams of NaI ?
O SIMPLE REACTIONS Identifying precipitation, combustion and acid-base reactions Classify each chemical reaction: type of reaction (check all that apply) reaction O combination O precipitation O single replacement O double replacement O decomposition combustion CH, (g) + 20, (g) → co, (g) + 2H,0(g) O acid-base O combination Oprecipitation O single replacement O double replacement HI(aq) + NaOH (aq) - Nal (aq) + H,0(1) O combustion acid-base decomposition combination O precipitation Fes o, (aq) + PbCl, (aq) → FeCl, (aq) + PbSO,(s) O single replacement O combustion double replacement O acid-base decomposition combination Oprecipitation 4Na(s) + 0, (g) → 2Na,0(s) O single replacement O combustion double replacement Oacid-base decomposition O O Oロ□
Consider the following reaction: ___ HCl (aq) + ___ Ca(OH)2 (aq) ---> ___ CaCl2 (aq) + ___ H2O (l) . What is the coefficient in front of the water molecule, when the reaction is balanced to lowest whole number coefficients? A. 3 B. 1 C. 2 D. 4
65. Lead ions can be precipitated from solution with NaCl according to the reaction: Pb²+ (aq) + 2 NaCl(aq) PbCl₂(s) + 2 Na+ (aq) When 135.8 g of NaCl are added to a solution containing 195.7 g of Pb²+, a PbCl2 precipitate forms. The precipitate is filtered and dried and found to have a mass of 252.4 g. Determine the limiting reactant, theoretical yield of PbCl2, and percent yield for the reaction.
Barium (Ba) can be analyzed in solutions by forming BaSo4 (s) precipitate. Ba 2+ + SO4 2- = BaSo4 (s) When a 1.0 g sample of a barium compound was treated with H2So4, it formed 0.605 g of BaSo4 (s) percipitate. a) What is the percent by weight of barium (Ba 2+) in the barium compound? b) What is the identity of the sample barium compound?
If a solution containing 58 g of mercury(II) nitrate is allowed to react completely with a solution containing 16.642 g of sodium sulfate according to the equation below: Hg(NO3)2(aq)+Na2SO4(aq)------2NaNO3(aq)+HgSO4(s) A. How many grams of solid precipitate will be formed if the reaction has a 100% yield? B. How many grams of the excess reagent will remain after the reaction? C. If the reaction has only an 80% yield, how many grams of solid precipitate will be formed?