When carbon dioxide gas dissolves in water, it reacts with the water to form carbonic acid. This is why soft drinks have a low pH, and soda water is often recommended as a mild cleaning agent. It is also why there is concern that rising levels of atmospheric carbon dioxide may cause the Earth's oceans to become more acidic. Here is the reaction between carbon dioxide gas and water: $H_2O(l) + CO_2(g) ightarrow H_2CO_3(aq)$ Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 164.5 g of water and 22.6 g of carbon dioxide gas each. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. vessel volume temperature initial rate of reaction A 4.0 L 33. $^circ$C ? B 2.0 L 34. $^circ$C ? C 2.0 L 35. $^circ$C ? D 4.0 L 34. $^circ$C ?
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Carbon dioxide dissolved in water effects the pH of rainwater and the pH of bodies of water such as the ocean, due to the formation of carbonic acid. Carbonic acid, which comes from the dissolution of carbon dioxide in water, is a diprotic weak acid. The two acid equilibriums reaction with acid equilibrium constants for aqueous carbonic acid are given here: H2CO3(aq) ⇄ H+(aq) + HCO3-(aq) Ka1 = 4.3 x 10-7 HCO3-(aq) ⇄ H+(aq) + CO32-(aq) Ka2 = 4.7 x 10-11 Answer the following questions based on an initial concentration of carbonic acid of 5.23 x 10-5 M. Part 1: What is the pH of the resulting solution? Part 2: What is the concentration of CO32- and HCO3- in the resulting solution at equilibrium? ____ M CO32- ____ M HCO3-
Dinesh S.
Carbon dioxide reacts with water in our blood to form carbonic acid. This reaction is critical in maintaining constant pH values. Water Hydrogen ion CO2 + H2O ⇌ H2CO3 ⇌ H+ + HCO3- Carbon dioxide Carbonic acid Bicarbonate ion When a person hyperventilates, their rate of breathing is elevated and comparatively more CO2 is lost from the body. What response will occur with the carbonate buffering system? The reaction moves to the right-hand side and the blood becomes more acidic. The reaction moves to the right-hand side and the blood becomes more alkaline. The reaction moves to the left-hand side and the blood becomes more acidic. The reaction moves to the left-hand side and the blood becomes more alkaline.
Josee P.
When carbon dioxide dissolves in water, it undergoes a multistep equilibrium process, with $K_{\text {overall }}=4.5 \times 10^{-7}$, which is simplified to the following: $$ \begin{aligned} \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) & \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \\ \mathrm{H}_{2} \mathrm{CO}_{3}(a q) &+\mathrm{H}_{2} \mathrm{O}(l) & \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \end{aligned} $$ (a) Classify each step as a Lewis or a Brónsted-Lowry reaction. (b) What is the $\mathrm{pH}$ of nonpolluted rainwater in equilibrium with clean air $\left(P_{\mathrm{CO},}\right.$ in clean air $=4 \times 10^{-4} \mathrm{~atm} ;$ Henry's law constant for $\mathrm{CO}_{2}$ at $25^{\circ} \mathrm{C}$ is $\left.0.033 \mathrm{~mol} / \mathrm{L} \cdot \mathrm{atm}\right) ?$ (c) What is $\left[\mathrm{CO}_{3}^{2-}\right]$ in rainwater $\left(K_{\mathrm{a}}\right.$ of $\left.\mathrm{HCO}_{3}^{-}=4.7 \times 10^{-11}\right) ?$ (d) If the partial pressure of $\mathrm{CO}_{2}$ in clean air doubles in the next few decades, what will the pH of rainwater become?
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