At a total atmospheric pressure of 1.00 atm, the partial pressure of CO₂ in air is approximately 4.0 x 10-4 atm Part A If at 20 °C and a partial pressure of 760 mmHg, the solubility of CO₂ in water is 0.169 g/100 mL, what is the solubility of CO₂ in an open bottle of seltzer water at 20°C? Express your answer using two significant figures. [5] ΑΣΦ X₂ Submit → + √x √x x Î IXI X.10 8.89.10-10 You have already submitted this answer. Enter a new answer. No credit lost. Try again. Previous Answers Request Answer A g/100 mL

At a total atmospheric pressure of 1.00 atm, the partial pressure of CO₂ in air is approximately 4.0 x 10-4 atm Part A If at 20 °C and a partial pressure of 760 mmHg, the solubility of CO₂ in water is 0.169 g/100 mL, what is the solubility of CO₂ in an open bottle of seltzer water at 20°C? Express your answer using two significant figures. [5] ΑΣΦ X₂ Submit → + √x √x x Î IXI X.10 8.89.10-10 You have already submitted this answer. Enter a new answer. No credit lost. Try again. Previous Answers Request Answer A g/100 mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Part A At 20 ∘C and a partial pressure of 76 mmHg, the solubility of CO2 in water is 0.169 g/100mL. What is the solubility of CO2 at 3.8×104 mmHg ? Express your answer using two significant figures. Part B Rank the following liquids in order of decreasing vapor pressure at 20.0 ∘C CH3CH2CH2CH2OH CH3CH2OCH2CH3 HOCH2CH2CH2OH
What volume of water, in mL, is needed to dissolve 2.3×101 mg of carbon monoxide gas (28.0101 g/mol) when the partial pressure of carbon monoxide above the water is 3.0 atm at 25 °C? The Henry's constant for carbon monoxide gas in water at 25 °C is 9.5×10-4 M/atm. Provide your answer rounded to three significant figures.
Calculate the osmotic pressure of a 10 m/v% aqueous hemoglobin solution at 20 °C, if its molar mass is 68000 g/mol. What is the m/v% concentration of that calcium chloride solution which is isotonic with the above hemoglobin solution? (3,584 kPa; 5.44 · 10-3 %)
What mass of silver bromide will disolve in 1.70 L of a 0.10 M NaBr (aq) solution at 25 °C? The Ksp of silver bromide is 5.35×10-13 and its molar mass is 187.8 g/mol.
If the solubility of copper (i) sulphide is 7.4 x 10-17 mol/L, what is its Ksp? Please format your answer like the following example: 1.2x10^-15
Find the freezing point of a solution obtained by dissolving 4.71 g of the aminoacid alanine (a molecular compound with molecular formula C3H7NO2 and molar mass = 89.09 g/mol) in 174 g of benzene. The melting point of pure benzene is 5.5 °C and the freezing point depression constant of benzene is 5.12 °C/m. Give the answer with 2 or more significant figures.
Question 30 of 30 Submit A solution is made by dissolving 2.5 mg sodium fluoride (NaF) in 2.5 L of water at 20.0°C. What is the fluoride ion concentration in ppm of the resulting solution, given that NaF is 45.0% fluoride ion by mass, and the density of water of 1.00 kg/L? | ppm 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00
As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.69 atm and a temperature of 25.0 °C, what is the solubility of N2 in a diver's blood? [Use the value of the Henry's law constant k calculated in Part A, 6.26 x 10-4 mol/(L· atm).JAssume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood. Express your answer with the appropriate units.
6. @ (b) (c) Write the equation for the dissolution of sulphur dioxide in water. For this problem, assume that no other reaction other than dissolution takes place. Write the expression for the Henry's Law constant (KH) for this reaction. The average atmospheric sulphur dioxide concentration in Delhi, India is 13.4 µg/m³, which is equivalent to 5.11×10-9 atm. Calculate the concentration of sulphur dioxide dissolved in water in equilibrium with dry Delhi air at 25°C. Hint - you will need to look up the value of KH for sulphur dioxide.
g The solubility in water of ionic compound X is measured and found to be 0.372 at 20. °C. Calculate the volume of a saturated solution of X in water that mL would contain 130. mg of X at this temperature. Be sure your answer has the correct unit symbol and number of significant digits.
With air with a volumetric composition of 20% O2, 79% N2 and 1% Ar, water is saturated at 25 ° C and 1 atm. Henry constants for O2, N2, and Ar are 4.3x10 ^ 4atm, respectively; It is given as 8,8x10 ^ 4atm and 3,6x10 ^ 4atm. Find the solubility of gases in water, in molescales.
At room temperature and an oxygen pressure of 1 atm, the solubility of oxygen in water is 1.35 x 10-3 mol/L. Calculate the concentration of dissolved oxygen in water under atmospheric conditions if the partial pressure of oxygen is 0.25 atm.