Question

What are common acids found in the home with the amount of pH valve it contains?

Answer 1

Hint : In the given question firstly we have to define what exactly are the pH and how can we determine it and give the proper definition and the characteristics of it. Although we can say that we know many acids from day to day life like cola and vinegar .

Complete Step By Step Answer:
The given question statement asks about the various kinds of the acids which are quite common and can be found in common households along with the pH value it shows.
Basically the value of the pH will depend on the concentration of ${H_3}{O^ + }$ ions, so we can say that the numbers given here are rough estimates of what the pH readings we might expect while we would be investigating the acids at home.
First one is soda, It specifically contains phosphoric acid which has a chemical formula of ${H_3}P{O_4}(aq)$ which is why Cola gives a low pH of roughly 2-3, because it is a weak acid.
Second one is the acetic acid which has the chemical formula of \[C{H_3}COOH(aq)\] , it is found in vinegar in the kitchen. It is also a weak acid with a similar pH range to that of phosphoric acid.
The third one is the Citric acid which has a chemical formula of \[{C_6}{H_8}{O_7}\]and it is found in lemons. It is also a weak acid and also is within the range of acetic acid and phosphoric acid
Fourth one is the sulfuric acid which has a chemical formula of \[{H_2}S{O_4}(aq)\] and is mainly found in the car batteries. It has a pH of 1 and it is a strong acid.
Fifth one is the Carbonic acid which can be made by carbonating water and have a chemical formula of ${H_2}C{O_3}(aq)$, which has a pH around 5.6, making it only slightly acidic.

Note :
The pH scale is logarithmic and inversely indicates the concentration of hydrogen ions in the solution. This is because the formula used to calculate pH approximates the negative of the base 10 logarithm of the molar concentration of hydrogen ions in the solution. More precisely, pH is the negative of the base 10 logarithm of the activity of the H+ ion.