Exams › JEE Advanced › Chemistry

100 mL of 0.3 M HCl is mixed with 200 mL of 0.3 M H2SO4. Calculate the molarity of H+ in the resulting solution.

1. 0.9 M
2. 0.6 M
3. 0.4 M
4. 0.5 M

Correct answer: 0.5 M

Solution

Total H+ moles = 0.03 (HCl) + 0.12 (H2SO4) = 0.15 mol in 300 mL, giving 0.5 M.

Related JEE Advanced Chemistry questions

• Which of the following contains the highest number of molecules?
• An organic compound with identical empirical and molecular formulas consists of 20% carbon, 6.7% hydrogen, 46.7% nitrogen, and the remainder as oxygen. When heated, it releases ammonia and leaves behind a solid residue. This residue produces a violet color when treated with an alkaline copper sulfate solution. Identify the compound.
• Which of the following statements accurately describe a hydrogen peroxide solution with a concentration of 17 g/L?
• The total energy needed to break all three P−H bonds in PH3(g) is 954 kJ mol⁻¹. What is the energy required to break a single P−H bond?
• Which of the following represents the balanced equation for the Calvin cycle in photosynthesis, showing the conversion of carbon dioxide into glucose?
• A substance H₂X with a molecular mass of 80 g is mixed into a liquid with a density of 0.4 g/ml. If the volume remains constant during dissolution, what is the molality of a solution with 3.2 molarity?

⚔️ Practice JEE Advanced Chemistry free + battle 1v1 →