An unopened can of soda has an aqueous CO2 concentration of 0.21 M at 25.0
K = C/P , 3.4 x 10^-2 = 0.21 /P
P = 6.17 atm = 6.2 atm = 6.2 x 760 torr = 4.7 x 10^3 torr
hence A is answer
An unopened can of soda has an aqueous CO2 concentration of 0.21 M at 25.0
6.) The solubility of CO2 (g) in water is 3.2 x 102 M at 25.0 °C and 1.0 atm pressure. a.) What is the Henry's Law constant for CO2 (g)? Cg = k P, ; Cg = concentration in M; k = Henry's Law constant in mol L atm*'; P. = pressure in atm. 3.2 x 10-2 M=k (1.0 atm) (3.2 x 10-2 M)/(1.0 atm) = k = 3.2 x 10-2 M/atm = 3.2 x 10-2 mol L atm" b.)...
Wtrich of the following aqueous solutions are good buffer systems? 0.21 M perchloric acid + 0.21 M sodium perchlorate 20.29 M ammonium nitrate + 0.31 M ammonia 0.19 M calcium hydroxide + 0.21 M calcium bromide 0.40 M acetic acid + 0.22 M potassium acetate 0.10 M nitrous acid + 0.13 M potassium nitrite
A soda pop has a pH = 3.80 at 25oC. Calculate the pressure of CO2 inside a closed-bottle of this soda pop at 25oC. Assume only water and CO2 are present and all dissolved CO2 is present as H2CO3. Ka1 (H2CO3) = 4.3 x 10^-7 and delta Gf naught (H2CO3 (aq)) = - 623.08 kJ/m
20. An aqueous solution at 25.0°C has an H* concentration of 4.0 x 102 molar. What is the OH- concentration in the same solution, in moles per liter? (A) 4.0 x 10-2 (B) 4.0 x 10-9 (C) 4.0 x 10-12 (D) 2.5 x 10-13
A soda pop has a pH = 3.80 at 25oC. Calculate the pressure of CO2 inside a closed-bottle of this soda pop at 25oC. Assume only water and CO2 are present and all dissolved CO2 is present as H2CO3. Ka,1(H2CO3) = 4.3 x 10-7 and ΔGfo(H2CO3,aq) = - 623.08 kJ/m Please include all math steps. The answer is Pco2=1.7atm
The beverage "soda pop” is made by compressing 85% carbon dioxide mixture, under a total pressure of 64.5 psi, into an aqueous syrup. The Henry's constant for carbon dioxide is 2.3 x 10-2 mole/ (liter * atm). The concentration of CO2 in soda pop is: (a) 0.072 M (b) 0.086 M (c) 0.092 M (d) 0.057 M
An aqueous solution at 25°C has a OH concentration of 3.7x10 M. Calculate the H,0 concentration. Be sure your answer has 2 significant digits. x 5 ?
Calculate the hydronium ion concentration in a solution that contains 0.21 M acetic acid and 0.17 M sodium acetate. For acetic acid, ka = 1.8 x 10^-5
Which of the following aqueous solutions are good buffer systems? 0.21 M hydroiodic acid 0.23 M potassium iodide 0.13 M hypochlorous acid + 0.12 M sodium hypochlorite 0.37 M hydrofluoric acid 0.26 M sodium fluoride 0.33 M ammonium bromide 0.3s M ammonia 0.13 M sodium hydroxide 0.28M sodium bromide
Calculate the approximate pH of an aqueous solution of H2S , 0.05 M, and H3PO4, 0.21 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa H2S/HS- = 7.02, pKa HS-/S2- = 13.99 pKaH3PO4/ H2PO4- =2.15, pKaH2PO4-/HPO42-=7.15, pKa HPO42-/ PO43- =12.38