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Mik0
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Can anyone tell me what a 1% (mass or volume) sulfuric acid solution is in moles? I want to find out the pH of a 1% (mass or volume) sulfuric acid solution?
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SUMMARY
A 1% sulfuric acid solution has a molar concentration of approximately 0.1 moles per liter, assuming a density of 1 g/mL. Given that sulfuric acid (H2SO4) is a strong acid, it dissociates completely in its first step, contributing to the hydrogen ion concentration. The pH can be calculated using the formula pH = -log([H+]), where [H+] is derived from the total dissociation of H2SO4. However, due to the second dissociation being weaker, about 76% of the acid exists in the HSO4- form, which slightly affects the final pH value.
PREREQUISITES- Understanding of molarity and molar concentration
- Knowledge of acid dissociation and strong vs. weak acids
- Familiarity with pH calculations and logarithmic functions
- Basic chemistry concepts, particularly regarding sulfuric acid
- Research the properties of sulfuric acid, including its dissociation constants
- Learn about calculating pH for weak acids and their equilibria
- Explore the impact of concentration on pH in strong acids
- Investigate the use of density tables for solution concentration conversions
Chemistry students, laboratory technicians, and anyone involved in acid-base chemistry or solution preparation will benefit from this discussion.
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