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![Question 20 [H3O+] = 7X10 PM At 2510 [OH-] [H3O+ ] = kW = 10-14 [OH-] = - - 1.8 10-11 M. 10-14 CH₃O+] 10-14 7810-4 Hence, the](http://img.homeworklib.com/questions/55a69c50-6fd0-11ea-bbca-13982fc08315.png?x-oss-process=image/resize,w_560)
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QUESTION 20 The concentration of H30 in a solution is 7 x...
QUESTION 21 A solution is 0.012 Min Pb(NO3)2 and 0.20 Min Sr(NO3)2. Solid Na2SO4 is added...
QUESTION 21 A solution is 0.012 Min Pb(NO3)2 and 0.20 Min Sr(NO3)2. Solid Na2SO4 is added until a precipitate just begins to form. The precipitate is and the concentration of sulfate ion at this point is Ksp for PbSO4 is 1.8 x 10-8 and for SrS04 is 2.8 x 10-7 PbSO4: 1.5 10 M SrS04; 1.4 x 10-6M PbSO4; 6.3 * 10 M "SrS04; 8.3 x 10-?M S-S04:2.6 x 10-7M
Question 32 2.5 Calculate the hydroxide ion concentration in an aqueous solution with a pH of...
Question 32 2.5 Calculate the hydroxide ion concentration in an aqueous solution with a pH of 5.33 at 25°C. E) 6.3 * 106M 2.1x10'M 4.7 x 10-10M A) 2.1 x 10-10M None • Previous
At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7....
At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7. The solubility product constant for strontium fluoride, SrF2, is 7.9 x 10-10. (a) What is the molar solubility of SrSO4 in pure water at 25 0C? (b) What is the molar solubility of SrF2 in pure water at 25 0C? (c) An aqueous solution of Sr(NO3)2 is added slowly to 1.0 litre of a well-stirred solution containing 0.020 mole F- and 0.10 mole SO42-...
QUESTION 18 1 points Save Answer Will a precipitate form when 20.0 mL of 1.8 x...
QUESTION 18 1 points Save Answer Will a precipitate form when 20.0 mL of 1.8 x 10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 x 10-4 M Na2SO4? The Ksp of (PbSO4) is 6.3 x 10-7. OA. yes, because the ion product > Ksp OB. no, because the ion product< OC.no, because the ion product > Ksp OD. 'yes, because the ion product < Ksp Ksp ОЕ. no, because Ksp is less than the ion product
Question 5 2 pts 15 ppb, equivalent to 7.2 x 10-8 M, is the maximum contaminant...
Question 5 2 pts 15 ppb, equivalent to 7.2 x 10-8 M, is the maximum contaminant level for Pb2+. At that lead concentration, what is the minimum phosphate concentration required to precipitate lead(1) phosphate? Pb3(PO4)2(s) = 3Pb2+(aq) + 2 PO43-(aq) Ksp = 1.5x 10-34 0 [PO43) = 1.3 x 10-6M O [PO43-]> 1.3 x 10-6M O [PO43-5) = 6.5 x 106M O [PO43]> 6.3x 10-7M O [PO43-) = 6.3x 10-7M 0 [PO43-> 6.5 x 10-6M
to answer number 28. you refer back to 24. but im stuck on it ans confused....
to answer number 28. you refer back to 24. but im stuck on it
ans confused.
2NaC1 HOH c. + MgC12 + H2S04> Na2S04+2HCI d. Ca(OH)2+ Pb(NO3)2> Ca(NO3)2 + Pb(OH)2 3 parts) What is the H+ concentration and pH of a 0.20 M solution of hypochlorous acid, Ka 3.5 x 10*? (SHOW ALL STEPS FOR CR CONC. AND SOLVE FOR 22.pH ) 20. ICE CHART, sOLVE FOR 21 23. What is the hydroxide ion concentration and pH of a 0.10...
please answer both question and box the answers QUESTION 2 What is the H30 ion concentration...
please answer both question and box the answers
QUESTION 2 What is the H30 ion concentration in an aqueous solution having an OH concentration of 1.0 x 10 M at 25 °C? а. 1.0x 102 M b. 13x 102 M C. 12x 10 2 M d. 12x 10 12 M 1.0x 10 12 M QUESTION 3 Which of the following salts has the lowest molar solubility in water? SrCO3 (Ksp-9.3 x 10-10) b. 1.8x 10-10) AgCl (Ksp C. 10-10 BaCrO4...
Ksp for SrSO4 = 3.2 x 10^-7 A solution contains 0.0210 M Pb2 + (aq) and...
Ksp for SrSO4 = 3.2 x 10^-7
A solution contains 0.0210 M Pb2 + (aq) and 0.0210 M Sr2 + (aq). If you add so - (aq), what will be the concentration of Pb2 + (aq) when Srso,() begins to precipitate? [Pb2+] = M
QUESTION 3 Calculate the pH of solution that has an H30+ ion concentration of 3.4 x...
QUESTION 3 Calculate the pH of solution that has an H30+ ion concentration of 3.4 x 10-9 M. 7.0 3.4 09 8.47 -8.47
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and...
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and the Cl- ion concentration is 3.2 x 10-4 M. Which of the following statements is true given that the Ksp for AgCl is 1.8 x 10^-10? A)No AgCl(s) will precipitate because Qsp<Ksp. B)No AgCl(s) will precipitate because the Ksp value indicates that AgCl is infinitely soluble in water. C)A precipitate of AgCl(s) will form because Qsp>Ksp. D)Insufficient data is given to make a prediction...
QUESTION 21 A solution is 0.012 Min Pb(NO3)2 and 0.20 Min Sr(NO3)2. Solid Na2SO4 is added until a precipitate just begins to form. The precipitate is and the concentration of sulfate ion at this point is Ksp for PbSO4 is 1.8 x 10-8 and for SrS04 is 2.8 x 10-7 PbSO4: 1.5 10 M SrS04; 1.4 x 10-6M PbSO4; 6.3 * 10 M "SrS04; 8.3 x 10-?M S-S04:2.6 x 10-7M
Question 32 2.5 Calculate the hydroxide ion concentration in an aqueous solution with a pH of 5.33 at 25°C. E) 6.3 * 106M 2.1x10'M 4.7 x 10-10M A) 2.1 x 10-10M None • Previous
QUESTION 18 1 points Save Answer Will a precipitate form when 20.0 mL of 1.8 x 10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 x 10-4 M Na2SO4? The Ksp of (PbSO4) is 6.3 x 10-7. OA. yes, because the ion product > Ksp OB. no, because the ion product< OC.no, because the ion product > Ksp OD. 'yes, because the ion product < Ksp Ksp ОЕ. no, because Ksp is less than the ion product
Question 5 2 pts 15 ppb, equivalent to 7.2 x 10-8 M, is the maximum contaminant level for Pb2+. At that lead concentration, what is the minimum phosphate concentration required to precipitate lead(1) phosphate? Pb3(PO4)2(s) = 3Pb2+(aq) + 2 PO43-(aq) Ksp = 1.5x 10-34 0 [PO43) = 1.3 x 10-6M O [PO43-]> 1.3 x 10-6M O [PO43-5) = 6.5 x 106M O [PO43]> 6.3x 10-7M O [PO43-) = 6.3x 10-7M 0 [PO43-> 6.5 x 10-6M
to answer number 28. you refer back to 24. but im stuck on it
ans confused.
2NaC1 HOH c. + MgC12 + H2S04> Na2S04+2HCI d. Ca(OH)2+ Pb(NO3)2> Ca(NO3)2 + Pb(OH)2 3 parts) What is the H+ concentration and pH of a 0.20 M solution of hypochlorous acid, Ka 3.5 x 10*? (SHOW ALL STEPS FOR CR CONC. AND SOLVE FOR 22.pH ) 20. ICE CHART, sOLVE FOR 21 23. What is the hydroxide ion concentration and pH of a 0.10...
please answer both question and box the answers
QUESTION 2 What is the H30 ion concentration in an aqueous solution having an OH concentration of 1.0 x 10 M at 25 °C? а. 1.0x 102 M b. 13x 102 M C. 12x 10 2 M d. 12x 10 12 M 1.0x 10 12 M QUESTION 3 Which of the following salts has the lowest molar solubility in water? SrCO3 (Ksp-9.3 x 10-10) b. 1.8x 10-10) AgCl (Ksp C. 10-10 BaCrO4...
Ksp for SrSO4 = 3.2 x 10^-7
A solution contains 0.0210 M Pb2 + (aq) and 0.0210 M Sr2 + (aq). If you add so - (aq), what will be the concentration of Pb2 + (aq) when Srso,() begins to precipitate? [Pb2+] = M
QUESTION 3 Calculate the pH of solution that has an H30+ ion concentration of 3.4 x 10-9 M. 7.0 3.4 09 8.47 -8.47
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