通过调节pH值来提高酸盐的消毒能力
Timir Baran Sil1, Dmitry Malyshev1, Marina Aspholm2
1Department of Physics, Umeå University, Umeå, 90187, Sweden.
BMC microbiology
|February 28, 2025
概括
优化低化物 (HOCl) 消毒剂的pH值对于有效消毒子至关重要. 9.5的pH值平衡了强大的杀菌活性与Bacillus cereus,提高了溶液稳定性,优于高度性或酸性配方.
科学领域:
- 微生物学 微生物学
- 生物化学 生物化学
- 环境科学 环境科学
背景情况:
- 化物溶液是常见的消毒剂,但它们对细菌子的有效性各不相同.
- 中性或低pH的低化物溶液是由于低酸 (HOCl) 的形成而有效的杀菌剂.
- 为了平衡有效性,稳定性和腐蚀性,最佳的pH条件仍然不清楚.
研究的目的:
- 为了研究pH值对低酸盐对Bacillus cereus的杀菌效率的影响.
- 为了确定低化物消毒的最佳pH值,平衡疗效和保质期.
- 阐明在不同pH值下子去污染的生化机制.
主要方法:
- 在pH值7.0-12.0下测试了5000ppm的低化物对Bacillus cereus子进行检测.
- 评估了子生存能力的减少和溶液的保质期.
- 利用拉曼光谱和光成像来研究子核透性和CaDPA释放.
主要成果:
- 低化物在pH值11.0以上是无效的 (<1-log降低).
- 在pH值11.0和9.5.5之间观察到显著的虫杀菌活性 (4-log降低).
- 较低的pH值 (<8.5) 提高了疗效,但大幅减少了保质期;pH值9.5提供了一个平衡.
- 较低的pH值增加了子的透性和二林酸 (CaDPA) 的释放.
结论:
- 在pH,低酸盐的有效性和保质期之间存在复杂的关系.
- pH 9.5 提供了一个平衡,有效地使子无活化,并提高了溶液的稳定性.
- 标准的高性 (pH 11.9) 低化物溶液不足以消除B. cereus的子.
- 优化pH值对于提高低化物消毒方法至关重要.
相关概念视频
01:23Titration of a Strong Acid with a Strong Base
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During the titration of a strong acid with a strong base, pH calculations are primarily based on the concentration of residual hydronium or hydroxide ions. Initially, a strong acid like hydrochloric acid fully dissociates, creating hydronium and chloride ions, resulting in a low pH. The addition of a strong base like sodium hydroxide alters the concentration of hydronium ions by neutralizing them. As more base is added, the pH gradually increases. At the equivalence point, all hydronium ions...
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02:28Titration Calculations: Strong Acid - Strong Base
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Calculating pH for Titration Solutions: Strong Acid/Strong Base
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows:
(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then:
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows:
(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then:
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01:19Mixtures of Acids
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The pH of a solution containing an acid can be determined using its acid dissociation constant and initial concentration. If a solution contains two different acids, then its pH can be determined using one of several methods depending on the relative strength of the acids and their dissociation constants.
In a strong and weak acid mixture, the strong acid dissociates completely and becomes a source of almost all the hydronium ions present in the solution. In contrast, the weak acid shows...
In a strong and weak acid mixture, the strong acid dissociates completely and becomes a source of almost all the hydronium ions present in the solution. In contrast, the weak acid shows...
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03:22Strong Acid and Base Solutions
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A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial concentration of acid. For example, 0.20 M hydrobromic acid will dissociate completely in water and produces 0.20 M of hydronium ions and 0.20 M of bromide ions.
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04:01Factors Affecting Solubility
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Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
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02:45Calculating pH Changes in a Buffer Solution
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A buffer can prevent a sudden drop or increase in the pH of a solution after the addition of a strong acid or base up to its buffering capacity; however, such addition of a strong acid or base does result in the slight pH change of the solution. The small pH change can be calculated by determining the resulting change in the concentration of buffer components, i.e., a weak acid and its conjugate base or vice versa. The concentrations obtained using these stoichiometric calculations can be used...
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