Ncert Solutions Chemistry Class 11th
Get insights from 2k questions on Ncert Solutions Chemistry Class 11th, answered by students, alumni, and experts. You may also ask and answer any question you like about Ncert Solutions Chemistry Class 11th
Follow Ask QuestionQuestions
Discussions
Active Users
Followers
New answer posted
10 months agoContributor-Level 10
A catalyst does not affect the equilibrium composition of a reaction mixture. Catalysts influence the rate of both forward and backward reactions equally.
New answer posted
10 months agoContributor-Level 10
Equilibrium constant depends upon the way in which the reaction is written.
New question posted
10 months agoNew answer posted
10 months agoContributor-Level 10
5.10. We know,
PV=nRT
n = PV/RT
n= (0.1 x34.05 x 10-3)/ (0.083 x 819)
&n
New answer posted
10 months agoContributor-Level 10
(a) In case of a non-polar (covalent) solvent, solvation enthalpy is small and hence, not sufficient to overcome lattice enthalpy of the salt. Consequently, the salt does not dissolve in non-polar solvent. As a general rule, for a salt to be able to dissolve in a particular solvent its solvation enthalpy must be greater than its lattice enthalpy so that the latter may be overcome by former. Each salt has its characteristic solubility which depends on temperature.
New answer posted
10 months agoContributor-Level 10
(d) Higher order ionization constants (Ka2, Ka3) are smaller than the lower order ionization constant (Ka1) of a polyprotic acid. The reason for this is that it is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces. This can be seen in the case of removing a proton from the uncharged H2CO3 as compared from a negatively charged HCO3–.Similarly, it is more difficult to remove a proton from a doubly charged HPO42– anion as compared to H2PO4–.
New answer posted
10 months agoContributor-Level 10
(c) Ammonium hydroxide is a weak base (Kb = 1.77 * 10–5) and not a weak acid. Therefore, it remains almost unionised in solution. This results in increased of H+ ion concentration in solution making the solution acidic. Thus, the pH ofNH4Cl solution in water is less than 7.
New answer posted
10 months agoContributor-Level 10
(a) The cations (e.g., Na+, K+, Ca2+, Ba2+, etc.) of strong bases and anions (e.g., Cl–, Br–, NO3–, ClO4– etc.) of strong acids simply get hydrated but do not hydrolyse, and therefore the solutions of salts formed from strong acids and bases are neutral i.e., their pH is 7. However, the other category of salts does undergo hydrolysis.
Taking an Exam? Selecting a College?
Get authentic answers from experts, students and alumni that you won't find anywhere else
Sign Up on ShikshaOn Shiksha, get access to
- 66k Colleges
- 1.2k Exams
- 687k Reviews
- 1800k Answers