Homework Answers
Reaction Quotient, Q = [Ca2+] [CO32- ] = 1.4 mM x 0.05 mM = 7.0 x 10-8 M
(1 mM = 10-3 M)
Q > K (K = 10-8.34)
Therefore the reaction will go backward and hence CaCO3 will precipitate.
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2. In a city's water distribution for supplying drinking water, the concentration of Ca' is 1.4...
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+...
2. Applying fundamental chemistry concepts to potable water treatment. Precipitation of lead hydroxide Pb(OH)2 on the i...
2. Applying fundamental chemistry concepts to potable water treatment. Precipitation of lead hydroxide Pb(OH)2 on the inside wall of water pipes is used to decrease the concentration of dissolved lead (Pb2+) in drinking water. Assume that a water treatment plant adjusts the pH of the finished drinking water before it enters the water distribution system, which contains old lead pipes. Which pH would result in a lower concentration of dissolved lead in drinking water: pH 7 and pH 8? Prove...
Consider the following reaction, which depicts the equilibrium found in most drinking water distribution pipes. 1....
Consider the following reaction, which depicts the equilibrium found in most drinking water distribution pipes. 1. What would happen with this equilibrium if acid (H+) is added? 2. What might be a health-related outcome of adding acid to this equilibrium? Pb3(CO3)2(OH)2(s) + 2H+ + 3Pb2+ + 2003-(aq) + H2O(1)
at must be the equilibrium concentration of Question 1 (5 pts). A. If the equilibrium concentration...
at must be the equilibrium concentration of Question 1 (5 pts). A. If the equilibrium concentration of Ce is 0.00010 M, what must be the oqu Cod in the solution? K (Ce (CO)) -59% 10%. (Answer: 3.9 x 10M] B. If the concentration of Ca?" of the solution in 1A is in will some CaCO, begin to precipitate? K (Caco) -1.3 x 10". (Hint: What is the the association of Caland Co, at these concentrations and how does that compare...
4. Solid calcium iodate, Ca(IO3)2, (MW = 389.9 g/mol) is only slightly soluble in cold water....
4. Solid calcium iodate, Ca(IO3)2, (MW = 389.9 g/mol) is only slightly soluble in cold water. Measurements indicate that only 0.12 g of the compound dissolve for every 100 ml of solution at 5C. Write the dissolution equation, the K expression, then determine the value of the equilibrium constant for calcium iodate dissolving in water at 5C.
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+...
In the environment, the equilibrium between calcite and dissolved calcium and carbonate is defined by this...
In the environment, the equilibrium between calcite and
dissolved calcium and carbonate is defined by this reaction: CaCO3
(s) ⇌ Ca2+ + CO3 2- .
The answer to the question above could be obtained by comparing
the reaction quotient Q (based on a specific solution composition)
to the thermodynamic constant K.
a. Calculate the thermodynamic constant K from on the standard
Gibb free energy of reaction ΔGº r.
b. A water sample contains 0.22 mmol Ca kg-1 and 0.05 mmol...
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+...
Question 2 (1 point) Consider the following dissolution reaction in water: Ca(103)2 --> Ca2+ + 2...
Question 2 (1 point) Consider the following dissolution reaction in water: Ca(103)2 --> Ca2+ + 2 103 K = 2.1 x 10-7 What is the concentration of Ca2+ in a solution that is saturated with Ca(103)2? 0 3.74 x 10-3 M. 0 7.59 x 10-4 M 04.44 x 10-6 M O 5.41 x 10-3M
8. Consider what happens when Ca(OH)2, dissolves in water. Write the balanced equation for the reaction....
8. Consider what happens when Ca(OH)2, dissolves in water. Write the balanced equation for the reaction. What can we say about the size of the equilibrium constant for this reaction? What is the [OH-] in a 3.25 mM solution of calcium hydroxide? POH? d. What is the pH of the above solution? [H30]?! What is the concentration of a calcium hydroxide solution with pH = 9.25?
2. Applying fundamental chemistry concepts to potable water treatment. Precipitation of lead hydroxide Pb(OH)2 on the inside wall of water pipes is used to decrease the concentration of dissolved lead (Pb2+) in drinking water. Assume that a water treatment plant adjusts the pH of the finished drinking water before it enters the water distribution system, which contains old lead pipes. Which pH would result in a lower concentration of dissolved lead in drinking water: pH 7 and pH 8? Prove...
Consider the following reaction, which depicts the equilibrium found in most drinking water distribution pipes. 1. What would happen with this equilibrium if acid (H+) is added? 2. What might be a health-related outcome of adding acid to this equilibrium? Pb3(CO3)2(OH)2(s) + 2H+ + 3Pb2+ + 2003-(aq) + H2O(1)
at must be the equilibrium concentration of Question 1 (5 pts). A. If the equilibrium concentration of Ce is 0.00010 M, what must be the oqu Cod in the solution? K (Ce (CO)) -59% 10%. (Answer: 3.9 x 10M] B. If the concentration of Ca?" of the solution in 1A is in will some CaCO, begin to precipitate? K (Caco) -1.3 x 10". (Hint: What is the the association of Caland Co, at these concentrations and how does that compare...
In the environment, the equilibrium between calcite and
dissolved calcium and carbonate is defined by this reaction: CaCO3
(s) ⇌ Ca2+ + CO3 2- .
The answer to the question above could be obtained by comparing
the reaction quotient Q (based on a specific solution composition)
to the thermodynamic constant K.
a. Calculate the thermodynamic constant K from on the standard
Gibb free energy of reaction ΔGº r.
b. A water sample contains 0.22 mmol Ca kg-1 and 0.05 mmol...
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+...
Question 2 (1 point) Consider the following dissolution reaction in water: Ca(103)2 --> Ca2+ + 2 103 K = 2.1 x 10-7 What is the concentration of Ca2+ in a solution that is saturated with Ca(103)2? 0 3.74 x 10-3 M. 0 7.59 x 10-4 M 04.44 x 10-6 M O 5.41 x 10-3M
8. Consider what happens when Ca(OH)2, dissolves in water. Write the balanced equation for the reaction. What can we say about the size of the equilibrium constant for this reaction? What is the [OH-] in a 3.25 mM solution of calcium hydroxide? POH? d. What is the pH of the above solution? [H30]?! What is the concentration of a calcium hydroxide solution with pH = 9.25?
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