Chemistry · 2013
JEE Main · 22 April 2013, Shift 1 · Q48
NaOH is a strong base. What will be pH of 5.0 × 10^-2 M NaOH solution? ( log 2=0.3)
NaOH is a strong base. What will be pH of $\displaystyle 5.0 \times 10^{-2} \mathrm{M} \mathrm{NaOH}$ solution ? $\displaystyle (\log 2=0.3)$
Official answer
(4)
$\displaystyle 12.70$
More from Ionic Equilibrium
- Assuming that the degree of hydrolysis is small, the pH of 0.1 M solution of sodium acetate ( K_a=1.0 × 10^-5 ) will be:2014
- Given below are two statements: Statement (I): Aqueous solution of ammonium carbonate is basic. Statement (II): Acidic/basic nature of salt solution…2024
- Which of the following are Lewis acids?2018
- The solubility of CdSO_4 in water is 8.0 × 10^-4 mol L^-1. Its solubility in 0.01 M H_2 SO_4 solution is \ \ \ \ × 10^-6 mol L^-1. (Round off to the…2021
- For a sparingly soluble salt AB_2, the equilibrium concentrations of A^2+ ions and B^- ions are 1.2 × 10^-4 M and 0.24 × 10^-3 M, respectively. The…2024
- Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R. Assertion A:Phenolphthalein is a pH dependent…2022
- In base vs. acid titration, at the end point methyl orange is present as2022
- For a concentrated solution of a weak electrolyte (K_eq=. equilibrium constant ) A_2 B_3 of concentration ' c ', the degree of dissociation ' α ' is2023
JEE Main 2013 Chemistry question, with the answer from NTA’s final answer key. Where our answers come from.