The Acids, Bases and Salts – Numerical Applications section emphasizes quantitative problem-solving based on the principles of acid-base chemistry and salts. This module is designed for Class 11–12 students, undergraduate learners, and competitive exam aspirants, helping students apply formulas, equilibria, and titration concepts to solve numerical questions confidently.
In this section, you will practice:
pH and pOH calculations – strong acids/bases, weak acids/bases, and polyprotic acids
Titration-related problems – volume of titrant, equivalence point, and indicator selection
Solubility product (Ksp) calculations – precipitation predictions, common ion effect, and ionic equilibria
Hydrolysis of salts – calculating pH of acidic, basic, and neutral salts
Stepwise and multi-concept problems combining titration, Ksp, and hydrolysis
Competitive exam-style MCQs and previous-year numerical questions
Graph- and data-based problem solving – interpreting titration curves and ionic concentration plots
The content is structured to strengthen numerical confidence, improve speed and accuracy, and prepare students for school exams, UG assessments, and high-stakes competitive exams.
Master numerical applications in Acids, Bases and Salts to develop strong analytical skills and exam readiness.
Q. How many grams of sodium chloride are needed to prepare 0.5 L of a 0.2 M solution?
A.
5.84 g
B.
11.68 g
C.
2.92 g
D.
0.58 g
Solution
Molar mass of NaCl = 58.44 g/mol. Moles needed = 0.2 M * 0.5 L = 0.1 moles. Mass = moles * molar mass = 0.1 * 58.44 g = 5.844 g.
Q. What is the equivalent weight of sulfuric acid (H2SO4) for the purpose of neutralization?
A.
49 g
B.
98 g
C.
24.5 g
D.
196 g
Solution
Equivalent weight = molar mass / n, where n = number of H+ ions. Molar mass of H2SO4 = 98 g/mol, n = 2. Therefore, equivalent weight = 98 g / 2 = 49 g.
