sulfate should be a constant factor, provided the sample volume and the pH during measurement are kept constant. A brief study of the solubility of barium sulfate in solutions of varying acidity was made to determine its solubility in the 0.005IV hydrochloric acid used in this analysis. The results are given in Table V. The solubility was found to be about 600 µg barium sulfate in 100 ml of 0.005N hydrochloric acid. In the sulfation plate analysis, the 20-ml aliquot may contain up to 120 µg dissolved barium sulfate (50 µg sulfate). Thus, in every analysis, 50 µg sulfate may be lost due to barium sulfate dissolving in the solution. If the standards are run at the same pH as the samples, the dissolved barium sulfate will be compensated for and the observed results will be correct. This contrasts with the standard method (3) where there may be a discrepancy of up to 30 µg sulfate between samples and standards, since only 20 µg sulfate are soluble in 20 ml deionized water at pH 6(6).Any changes in the results of the analysis of a specific sample due to standing for a period of time were studied using a standard solution of sodium sulfate (25 µg/ml) in 0.005ÍV hydrochloric acid. Twenty-ml samples of the stock solution were read at 15-minute intervals for 3 hours. The results indicated a loss of 5-7% of measurable sulfate. Samples should, therefore, be analyzed on the same day as acidification is made.(6) "Handbook of Chemistry and Physics," Chemical Rubber PublishingCo., New York, N.Y., 1970, p B-91.