If 50mg of CO32- and 50mg of Ca2+ are presentin1 L of water, what will be the final (equilibrium) concentration of Ca2+?
If 50mg of CO32- and 50mg of Ca2+ are presentin1 L of water, what will be the final (equilibrium) concentration of Ca2+?
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If 50mg of CO32- and 50mg of Ca2+ are presentin1 L of water, what will be the final (equilibrium) concentration of Ca2+?
If the equilibrium constant (Keq) for a reaction (CaCO3(s) → Ca2+ + CO32-) at 25 °C...
If the equilibrium constant (Keq) for a reaction (CaCO3(s) → Ca2+ + CO32-) at 25 °C is 3.3*10-9, what is the ΔG° for the reaction (round your answer to the nearest kJ/mol)?
The total hardness a water sample is 200 mg/l as CaCO3. The calcium (Ca2+) concentration is...
The total hardness a water sample is 200 mg/l as CaCO3. The calcium (Ca2+) concentration is 50 mg/l. Calculate the magnesium (Mg2+) concentration, in mg/l.
The total hardness a water sample is 200 mg/l as CaCO3. The calcium (Ca2+) concentration is...
The total hardness a water sample is 200 mg/l as CaCO3. The calcium (Ca2+) concentration is 150 mg/l. Calculate the magnesium (Mg2+) concentration, in mg/l.
What is the ionoc strength of the water? What are the activity coefficients? What is the...
What is the ionoc strength of the water?
What are the activity coefficients?
What is the equilibrium concentration of
CO3-2
1. Water from Thonon, France has the following composition Anions mg/L HCO3 Soa2 NOa CI- Cations mg/L 332 14 14 8.2 103.2 16.1 1.4 5.1 Ca2+ 0A 2+ Mg a) What is the ionic strength of this water b) What are the activity coefficients for HCO3 and cO32 in this water? c) Assuming an equilibrium constant for the dissociation of...
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 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+...
What is the concentration of Al+3 in a 1-L solution of DI water at equilibrium with...
What is the concentration of Al+3 in a 1-L solution of DI water at equilibrium with Al(OH)3 at pH 8.2
At 37 °C the equilibrium concentration of Ca2+ inside a cell is 0.098 M and outside...
At 37 °C the equilibrium concentration of Ca2+ inside a cell is 0.098 M and outside is 0.019 M. The cell membrane is permeable to Ca2+ and Cl–. The only ion present in addition to Ca2+ and Cl– is a protein (Prin+/–) inside the cell. The protein holds a single positive or negative charge. The Cl– is at equilibrium across the membrane while the protein is inside the cell and cannot permeate the membrane. What is the concentration of Prin+/–...
At 37 °C the equilibrium concentration of Ca2+ inside a cell is 0.067 M and outside...
At 37 °C the equilibrium concentration of Ca2+ inside a cell is 0.067 M and outside is 0.034 M. The cell membrane is permeable to Ca2+ and Cl–. The only ion present in addition to Ca2+ and Cl– is a protein (Prin+/–) inside the cell. The protein holds a single positive or negative charge. The Cl– is at equilibrium across the membrane while the protein is inside the cell and cannot permeate the membrane. What is the concentration of Prin+/–...
What is the ionoc strength of the water?
What are the activity coefficients?
What is the equilibrium concentration of
CO3-2
1. Water from Thonon, France has the following composition Anions mg/L HCO3 Soa2 NOa CI- Cations mg/L 332 14 14 8.2 103.2 16.1 1.4 5.1 Ca2+ 0A 2+ Mg a) What is the ionic strength of this water b) What are the activity coefficients for HCO3 and cO32 in this water? c) Assuming an equilibrium constant for the dissociation of...
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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