Prefered Brands of HCL and Phosphoric Acid

You might find the following conversion of 5% HCl to a pH value (according to Grok... AI):

### Conversion of 5% HCl to pH

To convert a 5% (w/w) HCl solution to its pH value, follow these steps. Note that HCl is a strong acid, so it fully dissociates, and pH is calculated as -log₁₀[H⁺], where [H⁺] equals the molarity of the solution.

1. **Identify the concentration and properties**:  
   5% HCl means 5 grams of HCl per 100 grams of solution. The molar mass of HCl is 36.46 g/mol. The density of a 5% aqueous HCl solution is approximately 1.0228 g/cm³ (at ~20°C).

2. **Calculate the molarity (M)**:  
   Use the formula for molarity from weight percent:  
   M = (weight percent × density × 10) / molar mass  
   M = (5 × 1.0228 × 10) / 36.46  
   = 51.14 / 36.46  
   ≈ 1.403 M  
   This means [H⁺] = 1.403 mol/L.

3. **Calculate the pH**:  
   pH = -log₁₀(1.403)  
   First, compute log₁₀(1.403):  
   log₁₀(1.4) ≈ 0.1461  
   Adjust for 1.403: log₁₀(1.403) ≈ 0.1461 + (0.003 / 1.4) × 0.4343 ≈ 0.1461 + 0.00093 ≈ 0.147  
   Thus, pH ≈ -0.147  

   (Note: pH values can be negative for concentrated strong acid solutions, as [H⁺] > 1 M.)

### Table of HCl Concentrations from 1% to 10% (w/w) and Corresponding pH Values

The table below uses the same calculation method for each percentage, with densities sourced from a density-concentration table for aqueous HCl solutions. Densities (in g/cm³ at ~20°C) are: 1.0031 (1%), 1.0081 (2%), 1.0130 (3%), 1.0179 (4%), 1.0228 (5%), 1.0278 (6%), 1.0327 (7%), 1.0377 (8%), 1.0426 (9%), 1.0476 (10%). Molarities are calculated as above, and pH = -log₁₀(M), rounded to three decimal places.

| % HCl (w/w) | pH     |
|

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|
| 1%          | 0.560  |
| 2%          | 0.257  |
| 3%          | 0.079  |
| 4%          | -0.048 |
| 5%          | -0.147 |
| 6%          | -0.228 |
| 7%          | -0.297 |
| 8%          | -0.357 |
| 9%          | -0.411 |
| 10%         | -0.458 |

The following is from AI bot Leo on Brave Search:

HCl to pH Conversion

"The pH of a 5% hydrochloric acid (HCl) solution cannot be directly calculated from the percentage concentration without knowing the specific density of the solution to convert it to molarity. However, the pH of a 5 M HCl solution, which is a common reference point for concentrated HCl, is approximately -0.69 when calculated using the standard formula \mathrm{pH} = -\log[\ce{H3O+}], assuming complete dissociation of the strong acid. This calculation assumes the concentration of hydronium ions [\ce{H3O+}] is equal to the molar concentration of HCl.

It is important to note that for such a high concentration, the actual pH is influenced by the activity of the ions rather than just their concentration, and the true pH is likely lower than -0.69 due to non-ideal behavior. For a 5 M HCl solution, the pH is estimated to be around -1.1 when activity coefficients are considered. The 5% concentration by weight is less concentrated than 5 M HCl, so its pH would be higher (less negative) than -1.1, but a precise value requires the density of the 5% HCl solution to determine its molarity.".

AI-generated answer. Please verify critical facts.