# Is it possible for a liquid chemical to have a pH value lower than its aqueous solution?

During the QC check of one of the products that we make as a company, the product had a $\mathrm{pH}$ of $10.44$ on one $\mathrm{pH}$ meter and $10.20$ on the other. (The product is a liquid, so it's straightforward to immerse $\mathrm{pH}$ probes to take the measurements.)

For QC of the product, it is required to make a $1\%$ solution using demineralised water and to take a $\mathrm{pH}$ reading.

The first $\mathrm{pH}$ meter read $11.72$ for this $1\%$ solution, and the second meter read $11.41$.

How is it possible for the raw product's $\mathrm{pH}$ to be lower than the $1\%$ solution's $\mathrm{pH}$? The product is supposed to be basic and not acidic at all.

• pH is a property of solutions. Bronsted-Lowry bases work by removing H+ from the solvent. If there is no H+ to take, the base cannot act like a base. Is your chemical a liquid when pure? – gsurfer04 Mar 11 '16 at 12:20
• Yes it is a liquid. It is used as a high pH boiler water treatment chemical. The previous batches of this product have always had a pH value greater than 12 as a raw product. This is the first time in 11 years of making this product that this has happened. – Dylan Le Sar Mar 11 '16 at 12:26