Which of the equations below best represents how excess acid in the blood plasma can be removed in the lungs by breathing? O2(g) → H₂ CO. H, CO3(aq) OH+ +0 (aq) OH+ + H,CO → H₂O(g) + CO2(g) (aq) 3(aq) OH+ + O2(g) → H₂ CO (aq) OH + HCO (aq) OH+ + O2(g) (aq) → H₂O(g) + CO2(g) + CO2(g) 3(aq) → H₂ CO3(g) → H₂O(g) + CO2(g → H₂ CO3(aq) H, 3(aq) → HCO3(aq)
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- The normal concentration of Ca2+ in blood is 5.0 mEq>L. How many milligrams of Ca2+ are in 1.00 L of blood?Carbon dioxide is dissolved in blood (pH 7.4) to form a mixture of carbonic acid and bicarbonate. Neglecting free CO2, what fraction will be present as carbonic acid? Would you expect a significant amount of carbonate (CO32-)?Which of the following correctly explains why the vapor pressure of water has to be included in the calculations? Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. Overview of the experiment:
- The following equation shows the reaction of baking soda (NaHCO3) and hydrochloric acid (HCl). NaHCO3+HCl → CO2+H2O+NaCl If you have 3.0 grams of NaHCO3, how many moles of HCl are needed for a complete relation?Nitric acid can be produced by the reaction ofgaseous nitrogen dioxide with water.3 NO2(g) + H2O(ℓ) −→2 HNO3(ℓ) + NO(g)If 956 L of NO2 gas react with water, whatvolume of NO gas will be produced? Assume the gases are measured under the sameconditionsBicarbonate/carbonic acid buffer in blood is an example of an equilibrium reaction that is meant to be very insensitive to change. How does the bicarbonate/carbonic acid buffer re-establish equilibrium if acidity increases? How does the bicarbonate/carbonic acid buffer re-establish equilibrium if alkalinity increases?
- What volume in liters would 20.0 moles of sulfur dioxide occupy at 75.3 °C with a pressure of 2.40 atm?When the following equation of a redox reaction in acidic solution is properly balanced, what are the coefficients for Cr2O72–, Fe2+ H+, Cr3+, Fe3+, and H2O, respectively? __Cr2O72– + __Fe2+ + __H+ --> __Cr3+ + __Fe3+ + __H2O (A) 1, 3, 14, 2, 3, 7; (B) 1, 6, 14, 2, 6, 7; (C) 2, 10, 14, 2, 10, 7; (D) 2, 12, 28, 4, 12, 14Consider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate its pH. b. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. c. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.
- For an acid HA, the concentrations of HA and A are 0.075 and 0.025, respectively, at pH 6.0. What is the p K a value for HA?At 39.9ºC, a solution of ethanol (XetOH = 0.9006, P * etOH = 130.4 Torr) and isooctane (P * iso = 43.9 Torr) forms a vapor phase with YetOH = 0.6667. The total pressure is 185.9 a. Calculate the activity and the activity coefficient of each component.b. Calculate the total pressure the solution would have if it were ideal.c. Comparing the ideal pressure to the actual pressure, what does this indicate about the molecular interactions?Write balanced ionic equations and net ionic equations forthe following reactions: (a) Aqueous sulfuric acid is neutralized by aqueous potassiumhydroxide.(b) Aqueous magnesium hydroxide is neutralized by aqueoushydrochloric acid.