Using Ksp's from your textbook, calculate the solution concentration of Ca2+ and Mg2+ required to form...
Using Ksp's from your textbook, calculate the solution concentration of Ca2+ and Mg2+ required to form a precipitate at pH 12. We would be forming the amorphous Mg(OH)2.
Mg(OH)2 Ksp = 6x10-10
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Using Ksp's from your textbook, calculate the solution
concentration of Ca2+ and Mg2+ required to
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A solution contains 0.020 M Mg2+ and 0.10 M Ca2+. Can 99.90% of Mg2+ be precipitated...
A solution contains 0.020 M Mg2+ and 0.10 M Ca2+. Can 99.90% of Mg2+ be precipitated by addition of NaOH without precipitation of Ca2+? Note: use Ksp = 7.1 x 10-12 for Mg(OH)2 Ksp= 5.5 x 10^-6 CaOH2
If the concentration of Mg2+ ion in seawater is 1.21x103 mg/L, what OH- concentration is required...
If the concentration of Mg2+ ion in seawater is 1.21x103 mg/L, what OH- concentration is required to precipitate Mg(OH)2 ? Ksp(Mg(OH)2)=5.6x10-12 -OH concentration must be greater than _____ M.
Can you please solve this Sodium hydroxide is added to a solution containing Mg2+ to produce...
Can you please solve this
Sodium hydroxide is added to a solution containing Mg2+ to produce a pH of 11.0 and form a precipitate of Mg(OH)2. (a) Given the Ksp of Mg(OH)2(s) is 6.0 x 10", calculate the molar concentration of Mg?* in solution. (b) The K, for Ca(OH),(s) is 6.5 x 10º. Explain how pH adjustment can be used to distinguish the presence of Mg from Ca“ in an EDTA titration of "hard" water containing both cations.
Water Hardness by EDTA Titration Objective: To determine [Ca2+,MG2+] and [Mg2+] concentration in an unknown water...
Water Hardness by EDTA Titration Objective: To determine [Ca2+,MG2+] and [Mg2+] concentration in an unknown water sample A 0.0107 molarity solution of EDTA is prepared for the experiment. 25 mL of an unknown is pipetted and diluted 100 mL with distilled water and adjusted to a pH between 8 and 10 with NH4OH. A 10.00 mL portion of the diluted unknown is transferred to a 250 mL flask with 3 mL of pH 10 ammonia buffer and tiny amount of...
Determine whether a precipitate form in the following reaction conditions: a. A solution containing lead (II)...
Determine whether a precipitate form in the following reaction conditions: a. A solution containing lead (II) nitrate is mixed with one containing sodium bromide to form a solution that is 0.0150 M in Pb(NO3)2 and 0.00350 M in NaBr. Does a precipitate form in the newly mixed solution? Ksp PbBr2 = 4.67 x 10-6 . b. A solution containing iron (II) nitrate is mixed with one containing sodium phosphate to form a solution that is 0.0365 M in Fe(NO3)2 and...
If the concentration of Mg2+ ion in seawater is 1.29 × 103 mg/L, what OH concentration...
If the concentration of Mg2+ ion in seawater is 1.29 × 103 mg/L, what OH concentration is required to precipitate Mg(OH)2? Ksp (Mg(OH)2) 5.6x 10-1 OH- concentration must be greater than M.
"Hard" water contains mainly salts of Ca2+ and Mg2+, both of which form many insoluble salts....
"Hard" water contains mainly salts of Ca2+ and Mg2+, both of which form many insoluble salts. You have a water sample and need to determine whether it contains Ca2+ and/or Mg2+. When you add ammonia to the solution, followed by ammonium chloride and ammonium oxalate, a white precipitate of CaC2O4 should form if Ca2+ is present. What is the purpose of adding the ammonium chloride to the reactant mixture? a. The chloride ion helps to form the calcium chloride precipitate....
Purifying Mg2+ from sea water. Aqueous sodium hydroxide is added to an aqueous solution that contains...
Purifying Mg2+ from sea water. Aqueous sodium hydroxide is added to an aqueous solution that contains 0.0099 M magnesium chloride and 0.021 M calcium chloride. What will be the concentration of the metal ion that precipitates first (as M(OH)2) at the time the second metal ion begins to precipitate? Ksp (Mg(OH)2) = 6.3 x 10-10 and Ksp (Ca(OH)2) = 6.5 x 10-6 Hint: Use Ksp values to determine the solubility of each product to determine the order of precipitation.
In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3...
In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3 M The equilibrium is represented by the equation MgF2 -->Mg 2+ + 2 F-. A.Write the expression for the solubility product constant, Ksp. B.Calculate the value of Ksp at 16°C for MgF2 Note: Your answer is assumed to be reduced to the highest power possible. C.Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 16°C to which 0.450 mole of...
The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and [Ca2+] = 0.011...
The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and [Ca2+] = 0.011 MM) can be separated by selective precipitation with KOH. Part A If the concentration of Mg2+ in the solution were 0.036 M, what minimum [OH−] triggers precipitation of the Mg2+ ion? (Ksp=2.06×10^−13) Express your answer to two significant figures and include the appropriate units.
Can you please solve this
Sodium hydroxide is added to a solution containing Mg2+ to produce a pH of 11.0 and form a precipitate of Mg(OH)2. (a) Given the Ksp of Mg(OH)2(s) is 6.0 x 10", calculate the molar concentration of Mg?* in solution. (b) The K, for Ca(OH),(s) is 6.5 x 10º. Explain how pH adjustment can be used to distinguish the presence of Mg from Ca“ in an EDTA titration of "hard" water containing both cations.
If the concentration of Mg2+ ion in seawater is 1.29 × 103 mg/L, what OH concentration is required to precipitate Mg(OH)2? Ksp (Mg(OH)2) 5.6x 10-1 OH- concentration must be greater than M.
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