{'fraction_non_alphanumeric': 0.03221384509938314, 'fraction_numerical': 0.00411240575736806, 'mean_word_length': 5.7592592592592595, 'pattern_counts': {'":': 0, '<': 0, '<?xml version=': 0, '>': 0, 'https://': 0, 'lorem ipsum': 0, 'www.': 0, 'xml': 0}, 'pii_count': 0, 'substrings_counts': 0, 'word_list_counts': {'cursed_substrings.json': 0, 'profanity_word_list.json': 0, 'sexual_word_list.json': 0, 'zh_pornsignals.json': 0}}
Stability of Activated Persulfate in the Presence of Aquifer Solids

Bench-scale experiments were performed to investigate the persistence of activated persulfate using citric acid (CA) chelated ferrous (Fe(II)), peroxide (H2O2), or hydroxide (OH−) activation in the presence of well-characterized aquifer solids. Chelation by citric acid was ineffective in controlling the interaction between persulfate and Fe(II), and oxidation of Fe(II) was observed, causing a rapid initial decrease in persulfate concentration. Subsequent to this loss, first-order persulfate degradation rate coefficients (kobs) were estimated, which were up to four times higher than the unactivated case due to the interaction with Fe(III), Fe(II), or CA. Total oxidation strength (TOS) was measured for peroxide activation experiments and was observed to decrease rapidly early due to peroxide degradation. This was followed by slow degradation kinetics similar to that of unactivated persulfate, implying that the initial TOS degradation was peroxide-dominated and the long-term kinetics were dominated by persulfate degradation. The kobs later used to capture TOS degradation were ∼1 to 100 times higher than kobs for unactivated persulfate. For alkaline activation, kobs were only one to four times higher than unactivated persulfate, and therefore alkaline conditions demonstrated the least overall impact on persulfate stability among the various activation strategies explored.