Question

____is the range of pH of acidic solution
A.1-7
B.7-14
C.0-7
D.7-1

Answer 1

Hint: pH is defined as a negative logarithm of hydrogen ion concentration. Greater the concentration of hydrogen ion lower will be the pH of solution.

Complete step by step solution:
The solution containing acids are known as acidic solutions and solutions with bases are known as basic solutions. To know whether the given solution is acidic, basic or neutral we define the value of pH for the solution which can be used to know the nature of the given solution. In acidic solution; \[{{\text{H}}^ + }\] ions are more and in basic solution; \[{\text{O}}{{\text{H}}^ - }\] are more and at neutral pH concentrations of \[{{\text{H}}^ + }\] is equal to concentration of \[{\text{O}}{{\text{H}}^ - }\] ions. Sum of pH and pOH for a solution is equals to 14.
pH is defined as power or potential concentration of hydrogen ions. Range of pH is from 0-14, solutions with pH values less than 7 are acidic solutions, solutions with pH values greater than 7 are basic solutions and solutions with pH value 7 are neutral solutions.

Thus, the correct option is C.

Note:
 According to Arrhenius concept; acids are those which gives \[{{\text{H}}^ + }\] ion in aqueous solution and bases are those which given \[{\text{O}}{{\text{H}}^ - }\] ion in aqueous solution. However this concept could not explain the acidic behaviour of compounds like boron trichloride which do not give \[{{\text{H}}^ + }\] ion but still are acids. According to the Bronsted Lowry concept; acids are those which accept \[{{\text{H}}^ + }\] ion and bases are those which accept \[{{\text{H}}^ + }\] ion. However this too could not explain acidic behaviour of compounds like boron trichloride. According to Lewis concept; acids are those which can accept electron(s) and are electron deficient and bases are those which donate electrons or are electron rich, for example ammonia.