While divided cells can allow good control over reaction pathways, their design may negatively impact user-friendliness, result in challenging process scale-ups and low overall energyefficiency due to the increased resistance that the physical barrier in the cell induces. Provided that the organic products from the parallel paired electrolysis are easy to separate from each other, a more straight-forward undivided electrolytic cell setup may be used. This strategy has, for example, been successfully implemented in an industrial setting, producing p-tert-butylbenzaldehyde dimethyl acetal and phthalide on multi-ton scale. Following the same logic, cathodic hydrogen evolution (HER) via proton reduction is attractive to couple with anodic oxidation of organic compounds to generate H 2 for fuel purposes at a lower cell potential compared to water electrolysis, along with the formation of valorized organic products. Overall, cathodic proton reduction represents the benchmark counter reaction for net oxidative electroorganic transformations (Figure ). For net reductive transformations, however, the choices of anodic counter reactions are more diverse. In a laboratory setting, the use of sacrificial anodes made from readily oxidized metals such as zinc, magnesium or aluminum is commonly employed. This approach results in continuous release of metal ions from the dissolving anode (Figure ), thereby typically promoting high selectivity and yields as parasitic oxidative transformations of starting materials, intermediates and/or products are suppressed. Nevertheless, the stoichiometric use of metal is not ideal from a sustainability perspective and can result in undesired side-reactions, such as Grignard reagent formation with aryl halides. Furthermore, the anode erosion inevitably results in a continuous change in inter-electrode distance and the formation of passivating layers of inorganic salts on electrode is common, with negative consequences for electrolysis outcome, not the least for large scale setups and flow processes. As alternative strategy, oxidation of chemical species such as solvent or stoichiometric reagents can be used to balance a net cathodic transformation (Figure ). For example, direct oxidation of amines, carboxylic acids, phosphines, thioureas, , bromide ions, and the use of H 2 as anodic fuel by means of quinone mediation in a divided cell have been successfully employed. While each system has its own merits, the lack of a unified approach to replace sacrificial metal anodes as counter reaction for electroreductive transformations can result in excessive screening of reaction conditions. Borohydride reagents remains severely underdeveloped in electrosynthetic transformations, despite their use as terminal reductant in fuel cell applications. We recently demonstrated that borohydride oxidation can serve as an efficient anodic counter reaction in electroreductive synthesis, effectively serving as the inverse of cathodic proton reduction that commonly balance electrooxidative transformations. Here, we demonstrate that this anodic borohydride oxidation has potential to serve as a user-friendly, effective and general counter reaction to electroreductive transformations with applicability on par with sacrificial metal anodes (Figure ).