5 1 X MasteringChemistry erty.edu/webapps/assessment/take/launch.jsp?course_assessment_id%=_1575667_1&course_id%3_592130_1&content_id= 39106439 18 puTube Maps M Gmail YouTube 2 Maps ¥ Question Completion Status: Which is more basic - an aqueous solution of borax or an equivalent concentration aqueous solution of lime water? [H*] (M) pH pOH [OH ] (M) 1 (1x10) 0.0 14.0 1x10-14 Stomach acid 1x10-1 1.0 13.0 1x10 13 Lemon juice Cola, vinegar 1x10-2 2.0 12.0 1x10-12 1x10-3 3.0 11.0 1x10-11 Wine Tomatoes 1x10-4 4.0 10.0 1x10-10 Black coffee 1x10-5 5.0 9.0 1x10-9 Rain Saliva Milk 1×10-6 6.0 8.0 1×10-8 1×10-7 7.0 7.0 1×10-7 Human blood 1×10-8 8.0 6.0 1x10-6 Seawater 1x10-9 9.0 5.0 1x10-5 Borax 1x10-10 10.0 4.0 1x10-4 Lime water 1x10-11 11.0 3.0 1x10-3 Household ammonia Household bleach 1x10-12 12.0 2.0 1x10-2 1x10-13 13.0 1.0 1x10-1 1x10-14 14.0 0.0 1 (1x10) pH + pOH = 14 %3D [H*][OH¯]= 1×10 14 A. borax B. household ammonia C. lime water D. the two solutions will have equivalent pH at equivalent concentrations Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save 80 000 000 DD F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 Increasing acid strength Increasing base strength

5 1 X MasteringChemistry erty.edu/webapps/assessment/take/launch.jsp?course_assessment_id%=_1575667_1&course_id%3_592130_1&content_id= 39106439 18 puTube Maps M Gmail YouTube 2 Maps ¥ Question Completion Status: Which is more basic - an aqueous solution of borax or an equivalent concentration aqueous solution of lime water? [H] (M) pH pOH [OH ] (M) 1 (1x10) 0.0 14.0 1x10-14 Stomach acid 1x10-1 1.0 13.0 1x10 13 Lemon juice Cola, vinegar 1x10-2 2.0 12.0 1x10-12 1x10-3 3.0 11.0 1x10-11 Wine Tomatoes 1x10-4 4.0 10.0 1x10-10 Black coffee 1x10-5 5.0 9.0 1x10-9 Rain Saliva Milk 1×10-6 6.0 8.0 1×10-8 1×10-7 7.0 7.0 1×10-7 Human blood 1×10-8 8.0 6.0 1x10-6 Seawater 1x10-9 9.0 5.0 1x10-5 Borax 1x10-10 10.0 4.0 1x10-4 Lime water 1x10-11 11.0 3.0 1x10-3 Household ammonia Household bleach 1x10-12 12.0 2.0 1x10-2 1x10-13 13.0 1.0 1x10-1 1x10-14 14.0 0.0 1 (1x10) pH + pOH = 14 %3D [H][OH¯]= 1×10 14 A. borax B. household ammonia C. lime water D. the two solutions will have equivalent pH at equivalent concentrations Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save 80 000 000 DD F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 Increasing acid strength Increasing base strength

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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17 E4 Analysis of lons Revised(1) copy Home Insert Draw Layout Review View Times New Roma 12 B. IUA. A, 三 =: |マ PART B: ANION TESTS Section 4: Test for Carbonate (CO? ) ions. Your conclusion for each test will be that CO was present or absent in the sample tested. In the conclusion box write that CO? was present or absent. OPERATION OBSERVATION CONCLUSION 6 M HCl with Na2CO3 Bubbling Present 6 M HCl with NaCl Clear solution 6 M HCl with Na2SO4 Clear solution 6 M HCl with Na3PO4 Clear solution 6 M HCl with Clear solution unknown Section 5: Test for Chloride (Cl-) ions After HNO3 added AgNO3 with Na2CO3 / HNO3 White precipitate Clear solution AgNO3 with NaCl / HNO3 White precipitate Precipitate stays AgNO3 with N22SO4/ HNO3 Clear solution i Clear solution AGNO3 with Na3PO4/ HNO3 White precipitate Clear solution AGNO3 with unknown / HNO3 White precipitate Clear solution 7 |Page Yes It's
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I Review I Constants Periodic Table • Part A Calculate the molar concentration of OH ions in a 0.087 M solution of ethylamine (CH;NH Ku = 6.4 x 10-4) Express your answer to two significant figures. e kevboard shortcuts Help Templates Symbols undo redo (OH ] = 7.0 • 10-3 M Submit Prevlous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
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reaction: NaHCO3(aq) + HCl(aq) ® NaCl(aq) + CO2(g) + H2O(l) How would your results be affected if the residue in the beaker wasn’t completely dry?