It’s definitely possible to calculate a negative pH value. In practice, any acid that yields a concentration of hydrogen ions with a molarity greater than 1 will be calculated to have a negative pH. For example, the pH of 12M HCl (hydrochloric acid) is calculated to be -log(12) = -1.08.

pH is one of the most common water quality tests performed. pH indicates the sample’s acidity but is actually a measurement of the potential activity of hydrogen ions (H+) in the sample. pH measurements run on a scale from 0 to 14, with 7.0 considered neutral. Solutions with a pH below 7.0 are considered acids.

Pure water has a pH of 7 and is considered “neutral” because it has neither acidic nor basic qualities.

6.5 to 8.5

The pH of most drinking-water lies within the range 6.5–8.5. Natural waters can be of lower pH, as a result of, for example, acid rain or higher pH in limestone areas.

pH is dependent on the concentration of H+ only, which varies with temperature as the extent of dissociation of water is temperature dependent. pH of pure water is 7 at 250C.

Detailed Description. pH is a measure of how acidic/basic water is. The range goes from 0 – 14, with 7 being neutral. pHs of less than 7 indicate acidity, whereas a pH of greater than 7 indicates a base.

The other two possibilities for a salt are strong acid and weak base or weak acid and strong base. As we can see, it is a salt of strong acid and strong base and has complete dissociation in water, it is the salt with highest pH. It’s pH will be equal to 7. Hence, the correct option is A.

Probably the highest pH ever measured in the deep sea, and possibly in any natural setting, is that of pore water ascending through the serpentinite mud volcanoes in the Mariana forearc (Figure 1).

From all the above options vinegar has the lowest pH-value that means it is the most acidic from the above and the washing soda is most basic.

Lemon juice in its natural state is acidic with a pH of about 2, but once metabolized it actually becomes alkaline with a pH well above 7.

pH is a measure of the concentration of hydrogen ions in a solution. Strong acids like hydrochloric acid at the sort of concentrations you normally use in the lab have a pH around 0 to 1.

The value of pH for a weak acid is less than 7 and not neutral (7). Its pH value is less than that of strong acids. Nonetheless, there can be some exceptions as Hydrofluoric acid’s pH is 3.27, which is also low as strong acid hydrochloric acid with pH value 3.01.

Strong Acids Generally, a strong acid has a pH of about zero to 3. The stronger the acid, the better it dissociates in an aqueous solution, releasing more cationic hydrogen (H+) ions. Examples of strong acids include hydrochloric acid (HCl), hydrobromic acid (HBr), perchloric acid (HClO4), and sulfuric acid (H2SO4).

Hydrofluoric acid is the only weak acid produced by a reaction between hydrogen and halogen (HF).

Nitric Acid

List of Strong Bases (8):

• LiOH (lithium hydroxide)
• NaOH (sodium hydroxide)
• KOH (potassium hydroxide)
• Ca(OH)2 (calcium hydroxide)
• RbOH (rubidium hydroxide)
• Sr(OH)2 (strontium hydroxide)
• CsOH (cesium hydroxide)
• Ba(OH)2 (barium hydroxide)

When going down a row in the Periodic Table (see figure below), the atoms get larger so the strength of the bonds get weaker, which means the acids get stronger. For the halogen-containing acids above, HF has the strongest bond and is the weakest acid.