How many Mg2+ ions would be present in 3.0 L of seawater that is 0.052 M in Mg2+?
Molarity = moles/ V in mL
Mg2+ = 0.052 M
Volume = 3.0 L
moles = M*V
= 0.052*3.0
= 0.156 moles
1 mole of Mg2+ contains -------> 6.023*10^23 ions
0.156 moles of Mg2+ contains ------> 6.023*10^23*0.156
= 9.39*10^22 ions
Number of Mg2+ ions would be present in 3.0 L of seawater that is 0.052 M in Mg2+ = 9.39*10^22 ions
How many Mg2+ ions would be present in 3.0 L of seawater that is 0.052 M...
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.
The magnesium and calcium ions present in seawater (Mg2+] = 0.059 M and (Ca2+] = 0.011 M) can be separated by selective precipitation with KOH. If the concentration of Mg2+ in the solution were 0.018 M, what minimum (OHtriggers precipitation of the Mg2+ ion? (Ksp = 2.06 x 10-13.) Express your answer to two significant figures and include the appropriate units. 03 O ? Value M
The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and (Ca2+] = 0.011 M) can be separated by selective precipitation with KOH. Part A If the concentration of Mg2+ in the solution were 0.021 M. what minimum (OH-] triggers precipitation of the Mg2+ ion? (Ksp = 2.06 x 10-13.) Express your answer to two significant figures and include the appropriate units. | НА w ? Value Units Submit Previous Answers Request Answer
enodic Table The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and (Ca2+] = 0.011 M) can be separated by selective precipitation with КОН. You may want to reference (Pages 775 - 778) Section 17.6 while completing this problem. Part A If the concentration of Mg2+ in the solution were 0.018 M, what minimum (OH) triggers precipitation of the Mg2+ ion?( Ksp = 2.06 x 10-13.) Express your answer to two significant figures and include the appropriate...
Using the principle of constant proportions, if there were 4 grams of Mg2+ in a seawater sample, how many grams of Na+ would be present? Show your work.
Na+=0.47 M, Mg2+=0.053 M, Ca2+=0.010 M magnesium is isolated from seawater by adding a strong base that cause the magnesium ions to precipitate. determine the minimum final hydroxide concentration that is needed to precipitate 99.9% of the magnesium ions from a sample of sea water at 25 C will any sodium ions ppt from seawater at the hydroxide ion concentration? will any calcium ions ppt from the seawater at hydroxide ion concentration ?
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.
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.
How many mL of 18.1 M H2SO4 stock solution would be needed to form 3.0 L of 0.100 M H2SO4 solution?
The typical concentration of Mg2+ in blood is 3 mEq/L. How many milligrams of Mg2+ are in 380 mL of blood?