A solution of copper sulphate cannot be stored in zinc vessel because:

For strong electrolytes, \(\Lambda_m\) increases with dilution and is represented by the equation \(\Lambda_m=\Lambda_m^0-A c^{1 / 2}\). Here, the
(A) Nature of solvent.
(B) Temperature.
(C) Charges on cation and anions produced.
(D) Type of electrolyte.
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Proteins are the polymers of about twenty different a-amino acids which are linked by peptide bonds. Proteins perform various structural and dynamic functions in the organisms. Proteins which contain only a-amino acids are called simple proteins. The secondary or tertiary structure of proteins get disturbed on change of pH or temperature and they are not able to perform their functions. This is called denaturation of proteins. Enzymes are biocatalysts which speed up the reactions in biosystems. Vitamins are accessory food factors required in the diet. They are classified as fat soluble (A, D, E and K) and water soluble (B group and C). Deficiency of vitamins leads to many diseases. Nucleic acids are the polymers of nucleotides which in turn consist of a base, a pentose sugar and phosphate moiety. Nucleic acids are responsible for the transfer of characters from parents to offsprings. There are two types of nucleic acids DNA and RNA. DNA contains a five carbon sugar molecule called 2-deoxyribose whereas RNA contains ribose.
RNA and DNA differ due to presence/absence of oxygen at which carbon of sugar moiety?

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One of the notable features of the transition element is the great variety of oxidation states it may show in its compounds. The elements which give the greatest number of oxidation states occur in or near the middle of the series. Manganese, for example exhibits all the oxidation states from +2 to +7. The lesser number of oxidation states at the extreme ends is either due to losing or sharing of few electrons (Sc, Ti) or too many d electrons of higher valence. Early in the first series scandium (II) is virtually unknown and titanium (IV) which is more stable than Ti (III) or Ti (II). On the other end, the only oxidation state of zinc is \(+ 2\).
Fe shows extra stability as \(Fe ^{3+}\) due to:

The correct mathematical representation of the rate of a reaction is

The negatively charged sol among the following is:

Match List-l with List-ll

List-l (Terms related to RNA)	List-II (Features)
(A). Capping	(I). Transcribes rRNAs
(B). Polyadenylation	(II). Removal of introns
(C). RNA polymerase I	(III). 5' end-methyl guanosine triphosphate addition
(D). Splicing	(IV). Addition of 200-300 adenylate residues

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The probabilities of occurrence of two events \(E\) and \(F\) are 0.25 and 0.50 respectively. The probability of their simultaneous occurrence is 0.14 . The probability that neither \(E\) nor \(F\) occurs is

If \(A=\left[\begin{array}{ll}1 & 0 \\ 0 & 0\end{array}\right], B=\left[\begin{array}{ll}0 & 0 \\ 3 & 0\end{array}\right]\) then

The function \(f(x)=x^x\) has a critical point at :

Match List-I with List-II

List-I (Contraceptive methods)	List-II (Examples)
(A) Non-medicated IUD	(I) LNG-20
(B) Hormone releasing IUD	(II) Multiload 375
(C) Copper releasing IUD	(III) Vaults
(D) Barrier method	(IV) Lippes loop

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Carboxylic acids are weaker than mineral acids, but they are stronger acids than alcohols and many simple phenols (\(\text{pKa}\) is ~ 16 for ethanol and 10 for phenol). The higher acidity of carboxylic acids as compared to phenols can be understood similarly. The conjugate base of carboxylic acid, a carboxylate ion, is stabilised by two equivalent resonance structures in which the negative charge is at the more electronegative oxygen atom. The conjugate base of phenol, a phenoxide ion, has non-equivalent resonance structures in which the negative charge is at the less electronegative carbon atom. Further, the negative charge is delocalised over two electronegative oxygen atoms in carboxylate ion whereas it is less effectively delocalised over one oxygen atom and less electronegative carbon atoms in phenoxide ion. Thus, the carboxylate ion is more estabilised than phenoxide ion, so carboxylic acids are more acidic than phenols.
Effect of substituents on the acidity of carboxylic acids: substituents may affect the stabliity of the conjugate base and thus, also affect the acidity of the carboxylic acids. Electron withdrawing group increase the acidity of carboxylic acids by stabilising the conjugate base through delocalisation of the negative charge by inductive and/or resonance effects. Conversely, electron donating groups decrease the acidity by destabilising the conjugate base.
The weakest among the following acid is :"