Calculate the solubility of Sr2+ in water at 25ºC in equilibrium with strontianite (SrCO3) and atmospheric CO2 (PCO2=10-...
Calculate the solubility of Sr2+ in water at 25ºC in equilibrium with strontianite (SrCO3) and atmospheric CO2 (PCO2=10-3.5) for pH 4, 7, and 10. Log Ks0 for strontianite is -11.42. Write a short explanation of why the Sr+2 concentration changes with pH.
Homework Answers
Add Answer to:
Calculate the solubility of Sr2+ in water at 25ºC in equilibrium with strontianite (SrCO3) and atmospheric CO2 (PCO2=10-...
In 2017, the concentration of CO2 in the atmosphere reached 405 ppm (pCO2 = 4.05×10-4 atm)....
In 2017, the concentration of CO2 in the atmosphere reached 405 ppm (pCO2 = 4.05×10-4 atm). The pH of ocean water in 2017 was 8.10. If the atmospheric concentration of CO2 continues to increase at a rate of 2.3 ppm/year, what pH do you expect to observe in the oceans in the year 2037? You may assume that [HCO3-] ≈ constant because the oceans are well-buffered.
Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.420 atm (a...
Calculate the solubility of carbon dioxide in water at an
atmospheric pressure of 0.420 atm (a typical value at high
altitude).
Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.420 atm (a typical value at high altitude). Atmospheric Gas Mole Fraction N2 7.81 x 10-1 ky mol/(L*atm) 6.70 x 10-4 1.30 x 10-3 02 2.10 x 10-1 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 x 10-4 3.50 x 10-2 CH4 2.00 x 10-6...
2. What is the PCO2 and CO3 (aq) concentration of a 5 °C ground water sample with pH= 6.5, and 50 mg L HCO; (aq)? 3...
2. What is the PCO2 and CO3 (aq) concentration of a 5 °C ground water sample with pH= 6.5, and 50 mg L HCO; (aq)? 3. In 1960 the average concentration of CO2(g) is 316.91 ppm. What was the pH of acid rain then. 4. Henry's constant for CO2(g) decreases with temperature, and therefore the solubility of CO2(g) also decreases with temperature. Use enthalpy data at 25 °C and Le Chatelier's principle to explain why and how equilibrium shifts with...
iSee Periodic Table See Hint Calculate the solubility of nitrogen in water at an atmospheric pressure...
iSee Periodic Table See Hint Calculate the solubility of nitrogen in water at an atmospheric pressure of 0.370 atm (a typical value at high altitude) Atmospheric GasMole FractionKH mol/(L'atm) 02 Ar CO2 CH4 7.81x 10-1 2.10x 101 9.34 x 10% 3.33x 10-4 2.00 x 106 5.00x 10-7 6.70x 10-4 1.30 x 10-3 1.40 x 10-3 3.50x 102 1.40 x 103 7.80 x 104
Atmospheric CO2 (g) is in equilibrium with dissolved CO, (aq), CO2(g) CO2 (aq) CO: (aq) then can react with water t...
Atmospheric CO2 (g) is in equilibrium with dissolved CO, (aq), CO2(g) CO2 (aq) CO: (aq) then can react with water to become H_CO. CO2 (aq) + H:0 (1) ~ HCO, (aq) (2) Add the two reactions together and determine the overall net reaction. If the K, for reaction (1) is 1.44 x 10-4 and for reaction (2) the K is 1.90 x 10-2, then what would the K, for the overall net reaction be? Explain. Increasing CO, (g) would have...
What is the pH of a sample of river water in which (HCO3-) = 2.0 x...
What is the pH of a sample of river water in which (HCO3-) = 2.0 x 10-4 M and the concentration of dissolved CO2 in equilibrium with atmospheric CO2 is 1.0 x 10-5 M? Chemical Equation: H2CO3(aq) + H2O(l) = HCO3-(aq) + H3O+(aq) pka = 6.37 Henderson Hasselbach equation: pH=pka+log [base]/[acid] A/
1a.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50...
1a.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1b.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1c.) Calculate Ksp = _____ A2BO3 ->2A++ BO32- Molar concentration of A+ = Molar...
calculate the molar solubility of Cr(OH)3 in a solution with a pH of 11.5 knowing that...
calculate the molar solubility of Cr(OH)3 in a
solution with a pH of 11.5 knowing that Ksp(Cr(OH)3) = 6.7 x
10^(-31)
1. Calculate the molar solubility of Cr(OH), in a solution with a pH of 11.5 knowing that Kop(Cr(OH)2) = 6.7 x 10" 2. What is the pH of a 0.895M sodium fluoride (NaF) solution knowing that the hydrofluoric acid is 7.11 x 10 of 3. Calculate the molar solubility of antimony sulfide (Sb2S) in water knowing K =1.6 x...
calculate equilibrium dissiociation constant of water help! We know that Kw = 1.0 x 10-14 at...
calculate equilibrium dissiociation constant of water
help!
We know that Kw = 1.0 x 10-14 at 25°C. At 37°C, the [H3O+] in pure water is 1.6 x 10"| M. Calculate the equilibrium dissociation constant of water, Kw, at this temperature. A. 2.6 x 10-14 | CNH-TT H+7: 10 x 10-14 DH = -log(11 B. 1.0 x 10-7 C. 1.0 x 10-14 [1-6x10-?][6.16 *10-8] PH= 6.79 D. 1.6 x 10-7 POH=7. 21
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2...
Carbon dioxide dissolves in water to form carbonic acid, which
is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium
equation The acid dissociation constants listed in most standard
reference texts for carbonic acid actually apply to dissolved CO2.
For a CO2 partial pressure of 1.8×10–4 bar in the atmosphere, what
is the pH of water in equilibrium with the atmosphere? (For
carbonic acid Ka1 = 4.46× 10–7 and Ka2 = 4.69× 10–11).
Carbon dioxide dissolves in water to form carbonic...
Calculate the solubility of carbon dioxide in water at an
atmospheric pressure of 0.420 atm (a typical value at high
altitude).
Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.420 atm (a typical value at high altitude). Atmospheric Gas Mole Fraction N2 7.81 x 10-1 ky mol/(L*atm) 6.70 x 10-4 1.30 x 10-3 02 2.10 x 10-1 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 x 10-4 3.50 x 10-2 CH4 2.00 x 10-6...
2. What is the PCO2 and CO3 (aq) concentration of a 5 °C ground water sample with pH= 6.5, and 50 mg L HCO; (aq)? 3. In 1960 the average concentration of CO2(g) is 316.91 ppm. What was the pH of acid rain then. 4. Henry's constant for CO2(g) decreases with temperature, and therefore the solubility of CO2(g) also decreases with temperature. Use enthalpy data at 25 °C and Le Chatelier's principle to explain why and how equilibrium shifts with...
iSee Periodic Table See Hint Calculate the solubility of nitrogen in water at an atmospheric pressure of 0.370 atm (a typical value at high altitude) Atmospheric GasMole FractionKH mol/(L'atm) 02 Ar CO2 CH4 7.81x 10-1 2.10x 101 9.34 x 10% 3.33x 10-4 2.00 x 106 5.00x 10-7 6.70x 10-4 1.30 x 10-3 1.40 x 10-3 3.50x 102 1.40 x 103 7.80 x 104
Atmospheric CO2 (g) is in equilibrium with dissolved CO, (aq), CO2(g) CO2 (aq) CO: (aq) then can react with water to become H_CO. CO2 (aq) + H:0 (1) ~ HCO, (aq) (2) Add the two reactions together and determine the overall net reaction. If the K, for reaction (1) is 1.44 x 10-4 and for reaction (2) the K is 1.90 x 10-2, then what would the K, for the overall net reaction be? Explain. Increasing CO, (g) would have...
What is the pH of a sample of river water in which (HCO3-) = 2.0 x 10-4 M and the concentration of dissolved CO2 in equilibrium with atmospheric CO2 is 1.0 x 10-5 M? Chemical Equation: H2CO3(aq) + H2O(l) = HCO3-(aq) + H3O+(aq) pka = 6.37 Henderson Hasselbach equation: pH=pka+log [base]/[acid] A/
calculate the molar solubility of Cr(OH)3 in a
solution with a pH of 11.5 knowing that Ksp(Cr(OH)3) = 6.7 x
10^(-31)
1. Calculate the molar solubility of Cr(OH), in a solution with a pH of 11.5 knowing that Kop(Cr(OH)2) = 6.7 x 10" 2. What is the pH of a 0.895M sodium fluoride (NaF) solution knowing that the hydrofluoric acid is 7.11 x 10 of 3. Calculate the molar solubility of antimony sulfide (Sb2S) in water knowing K =1.6 x...
calculate equilibrium dissiociation constant of water
help!
We know that Kw = 1.0 x 10-14 at 25°C. At 37°C, the [H3O+] in pure water is 1.6 x 10"| M. Calculate the equilibrium dissociation constant of water, Kw, at this temperature. A. 2.6 x 10-14 | CNH-TT H+7: 10 x 10-14 DH = -log(11 B. 1.0 x 10-7 C. 1.0 x 10-14 [1-6x10-?][6.16 *10-8] PH= 6.79 D. 1.6 x 10-7 POH=7. 21
Carbon dioxide dissolves in water to form carbonic acid, which
is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium
equation The acid dissociation constants listed in most standard
reference texts for carbonic acid actually apply to dissolved CO2.
For a CO2 partial pressure of 1.8×10–4 bar in the atmosphere, what
is the pH of water in equilibrium with the atmosphere? (For
carbonic acid Ka1 = 4.46× 10–7 and Ka2 = 4.69× 10–11).
Carbon dioxide dissolves in water to form carbonic...
Most questions answered within 3 hours.
-
Calculate the pH of each of the following solutions.
0.50 M HBr
3.1×10−4 M KOH
4.2×10−5...
asked 1 hour ago -
For the year ended December 31, Depot Max’s cost of merchandise
sold was $85,600. Inventory at the...
asked 1 hour ago -
Week 10 - Professional Memo Assignment
Professional Memo Assignment
Your mission for this week, should you...
asked 1 hour ago -
Write a Python program that stores the data for each
player on the team, and it...
asked 1 hour ago -
In
the last 3 months, mike never knows when he is going to get his
allowance...
asked 1 hour ago -
Is Ca(OH)2 a Bronsted base, Lewis base, or both? Why?
asked 1 hour ago -
1A- Why don’t voters complain about U.S. tariffs on imported
sugar?
Because sugar is only a...
asked 1 hour ago -
Cash Payback Period
Primera Banco is evaluating two capital investment proposals for
a drive-up ATM kiosk,...
asked 1 hour ago -
Create a button in Swift (Xcode) that will create a charge,
create a charge using Stripe's...
asked 1 hour ago -
The reaction rate of CO and NO2 in the reaction
CO(g) + NO2(g) → CO2(g) +...
asked 1 hour ago -
Imagine that a chemist puts 6.40 mol each of
C3H8 and O2 in a 1.00-L container...
asked 1 hour ago -
How much money should be invested today in order to have $8340
at the end of...
asked 2 hours ago