Carbonate formation is the primary source of energy and carbon losses in lowtemperature carbon dioxide electrolysis. Realigning research priorities to address the carbonate problem is essential if this technology is to become a viable option for renewable chemical and fuel production. The plummeting cost and daily curtailment of renewable electricity have spurred growing interest in using CO 2 electrolysis to produce chemicals and fuels. High-temperature solid oxide cells that convert CO 2 to CO and O 2 have reached nascent commercialization. Low-temperature CO 2 electrolysis is an attractive alternative that offers more convenient and flexible operation and the ability to generate multicarbon products such as ethylene, ethanol, and propanol. Over the past 10 years, a dramatic expansion of research in this area has yielded substantial progress in fundamental understanding and prototype devices. Leveraging insights from fuel cells and membrane water electrolyzers, researchers have developed gas diffusion electrode (GDE) cells demonstrating synthetically relevant CO 2 electrolysis current densities (>100 mA cm −2) and promising stability. Despite these advances, the energy efficiency (power-to-product) and carbon efficiency (CO 2-toproduct) of low-temperature CO 2 electrolysis remain too low to support large-scale applications 1,2. While much current research is focused on CO 2 reduction catalyst design, the biggest obstacle to improving performance is an often overlooked basic chemistry problem: the rapid and thermodynamically favorable reaction of CO 2 with hydroxide (OH-) to form carbonate (CO 3 2-) imposes steady state electrolysis conditions that result in large voltage and CO 2 losses. Although recent work has brought attention to some aspects of the CO 3 2problem 2-4 , it is far more pernicious than what is widely appreciated. Here we explain how CO 3 2formation compromises efficiency to highlight the need for new research directions that address this problem. Hydroxide consumption makes alkaline CO 2 electrolyzers fuel-wasting devices The state-of-the-art for low-temperature CO 2 electrolysis has been obscured by studies that utilize a reservoir of flowing alkaline electrolyte to maintain a high pH in the cell 5-8. High pH minimizes the cell voltage, which makes these systems appear to have high energy efficiency, but consumption of OHin the reservoir by CO 3 2formation results in a net negative energy balance. Understanding why the cell voltage is minimized at high pH helps to clarify the CO 3 2problem (Fig. 1a). For most known catalyst materials, including Au and Cu, the CO 2 reduction rate depends on the electron transfer driving force but not explicitly on pH 9-13. As a result, synthetically relevant current densities require rather negative potentials versus an absolute reference such as the standard hydrogen electrode (SHE). Even with high surface area electrodes, CO 2 reduction at a geometric current density of >200 mA cm-2 has generally required potentials