Equilibrium
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New answer posted
5 months agoContributor-Level 10
Equilibrium constant depends upon the way in which the reaction is written.
New question posted
5 months agoNew answer posted
5 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.
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5 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
5 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
5 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.
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5 months agoContributor-Level 10
(b) Both are correct statements but R is not the reason for A. The acid-base pair that differs only by one proton is called a conjugate acid-base pair. Therefore, OH– is called the conjugate base of an acid H2O and NH4+ is called conjugate acid of the base NH3. If Brönsted acid is a strong acid then its conjugate base is a weak base and vice-versa. It may be noted that conjugate acid has one extra proton and each conjugate base has one less proton.
New answer posted
5 months agoContributor-Level 10
For precipitation to take place, it is required that the calculated ionic product exceeds the Ksp value. So, following data on Ksp values should have been provided to answer the question.
KspforFeS=6.3*10−18,
MnS=2.5*10−13,
ZnS=1.6*10−24
CdS=8.0*10−27
Before mixing:
[S2−]=1.0*10−19M and [M2+]=0.04M
volume =10mL volume =5mL
After mixing:
[S2−]=? [M2+]=?
volume = (10+5)=15mL volume =15mL
[S2−]= (1.0*10−19*10)/ 15=6.67*10−20M
[M2+]= (0.04*5) / 15=1.33*10−2M
Ionic product = [M2+] [S2−]
= (1.33*10−2) (6.67*10−20)
=8.87*10−22
This ionic product exceeds the
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