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(a) 100 mg of lead (II) hydroxide is added to 10 L of water. Does the...
9. (a) 100 mg of lead (1) hydroxide is added to 1.0 L of water. Does...
9. (a) 100 mg of lead (1) hydroxide is added to 1.0 L of water. Does the solid completely dissolve? What is the pH7 (b) What is the minimum amount of milliers of 1,00 M sodium hydroxide must be added to dissolve the precipitate? (12 pts.) No it does not Pb (OH)₂ 15 = P6tean + 204 cm completely dissolve t2x kap=1.2 X 10-15 H UH 2x 1.2X10-15 = (x) (2x)² = 4 x3 the X= 6.69x10-6 the pH =...
If 75 mg of lead(II) sulfate is placed in 250 mL of pure water, does all...
If 75 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves? (Ksp for lead(II) sulfate = 6.3 x 10-7)
A solution contains 1.26x10-2 M lead acetate and 8.96x10-M iron(III) nitrate. Solid sodium hydroxide is added slowly to...
A solution contains 1.26x10-2 M lead acetate and 8.96x10-M iron(III) nitrate. Solid sodium hydroxide is added slowly to this mixture. What is the concentration of iron(III) ion when lead ion begins to precipitate? [Fe3+]=
A solution contains 2.40×10-2 M nickel(II) nitrate and 2.40×10-2 M iron(II) acetate. Solid sodium hydroxide is...
A solution contains 2.40×10-2 M nickel(II) nitrate and 2.40×10-2 M iron(II) acetate. Solid sodium hydroxide is added slowly to this mixture. What is the concentration of nickel ion when iron(II) ion begins to precipitate? Solubility product constant data is found in the Chemistry References. [Ni2+] = M
Ca(OH)2 is added to water to reach a concentration of 53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and it reacts...
Ca(OH)2 is added to water to reach a concentration of 53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and it reacts with Ca(OH)2 according to equation below. Assume SO4-2 is in excess. What are the final dissolved Ca2+and Mg 2+ concentrations? What is the initial and final hardness? What is the Mg(OH)2 precipitate concentration? Answer should be (28.6 mg/L, 0 mg/L, 12.5 mg CaCO3/L, 71.5 mg CaCO3 /L, 7.28 mg/L). Mg2+ + SO42- + Ca(OH)2 = Mg(OH)2 +Ca2+...
14. What minimum mass of cobalt(II) nitrate must be added to 60.0 mL of a 0.0890...
14. What minimum mass of cobalt(II) nitrate must be added to 60.0 mL of a 0.0890 M phosphate solution in order to completely precipitate all of the phosphate as solid cobalt(II) phosphate? 2PO4 (aq) + 3Co(NO3)2(aq) - Co3(PO4)2(s) + 6NO3 (aq)
2. A dose of 41 mg/L of alum is used in coagulating a turbid water at...
2. A dose of 41 mg/L of alum is used in coagulating a turbid water at a water treatment plant treating a flow rate of 32 million gallons per day (mgd). The natural alkalinity of the source water is 10 mg/L (as CaCO3). a. Will the alkalinity be completely consumed in the reaction? If not, then how much alkalinity will be left? If so, then what concentration of caustic soda (NaOH) must be added to avoid a change in the...
********PLEASE PLEASE PLEASE ANSWER 1-3****** THANK YOUU!!! 1a.When 22.0 mL of a 8.66×10-4 M cobalt(II) iodide...
********PLEASE PLEASE PLEASE ANSWER 1-3****** THANK YOUU!!! 1a.When 22.0 mL of a 8.66×10-4 M cobalt(II) iodide solution is combined with 25.0 mL of a 1.92×10-4 M ammonium sulfidesolution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to______ 1b.When 22.0 mL of a 6.52×10-4M ammonium iodide solution is combined with 12.0 mL of a 1.05×10-4M lead acetatesolution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to_____. 2a.A...
Ca(OH)2 is added to water to reach a concentration of 53 mg/L. Initially, the water had...
Ca(OH)2 is added to water to reach a concentration of 53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and it reacts with Ca(OH)2 according to equation below. Assume SO4-2 is in excess. What are the final dissolved Ca2+and Mg 2+ concentrations? What is the initial and final hardness? What is the Mg(OH)2 precipitate concentration? Answer should be (28.6 mg/L, 0 mg/L, 12.5 mg CaCO3/L, 71.5 mg CaCO3 /L, 7.28 mg/L). Mg2+ + SO42- + Ca(OH)2 = Mg(OH)2 +Ca2+...
Ca(OH)2 is added to water to reach a concentration of 53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and it reacts...
Ca(OH)2 is added to water to reach a concentration of
53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and
it reacts with Ca(OH)2 according to equation 61a. Assume
SO4-2 is in excess. What are the final
dissolved Ca2+and Mg 2+ concentrations? What
is the initial and final hardness? What is the Mg(OH)2
precipitate concentration? (28.6 mg/L, 0 mg/L, 12.5 mg CaCO3/L,
71.5 mg CaCO3 /L, 7.28 mg/L).
Precipitation of noncarbonate Mg, leaving Ca from lime in solution. Mf+...
9. (a) 100 mg of lead (1) hydroxide is added to 1.0 L of water. Does the solid completely dissolve? What is the pH7 (b) What is the minimum amount of milliers of 1,00 M sodium hydroxide must be added to dissolve the precipitate? (12 pts.) No it does not Pb (OH)₂ 15 = P6tean + 204 cm completely dissolve t2x kap=1.2 X 10-15 H UH 2x 1.2X10-15 = (x) (2x)² = 4 x3 the X= 6.69x10-6 the pH =...
A solution contains 1.26x10-2 M lead acetate and 8.96x10-M iron(III) nitrate. Solid sodium hydroxide is added slowly to this mixture. What is the concentration of iron(III) ion when lead ion begins to precipitate? [Fe3+]=
14. What minimum mass of cobalt(II) nitrate must be added to 60.0 mL of a 0.0890 M phosphate solution in order to completely precipitate all of the phosphate as solid cobalt(II) phosphate? 2PO4 (aq) + 3Co(NO3)2(aq) - Co3(PO4)2(s) + 6NO3 (aq)
2. A dose of 41 mg/L of alum is used in coagulating a turbid water at a water treatment plant treating a flow rate of 32 million gallons per day (mgd). The natural alkalinity of the source water is 10 mg/L (as CaCO3). a. Will the alkalinity be completely consumed in the reaction? If not, then how much alkalinity will be left? If so, then what concentration of caustic soda (NaOH) must be added to avoid a change in the...
Ca(OH)2 is added to water to reach a concentration of
53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and
it reacts with Ca(OH)2 according to equation 61a. Assume
SO4-2 is in excess. What are the final
dissolved Ca2+and Mg 2+ concentrations? What
is the initial and final hardness? What is the Mg(OH)2
precipitate concentration? (28.6 mg/L, 0 mg/L, 12.5 mg CaCO3/L,
71.5 mg CaCO3 /L, 7.28 mg/L).
Precipitation of noncarbonate Mg, leaving Ca from lime in solution. Mf+...
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