In salts of polyatomic anion, as polaris...

In salts of polyatomic anion, as polarising power of cation increase, thermal stability of the salt decrease and decomposed species may further undergo redox reaction
Q. Water soluble salt(x) was heated into three products A, B and C and B and C are two different paramagnetic gases. A is red in hot condition, then salt(x) is :

`Hg(NO_(3))_(2)`

`FeC_(2)O_(4)`

`ZnSO_(4)`

`Pb(NO_(3))_(2)`

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To solve the problem step by step, we need to analyze the information given about the water-soluble salt (X) and the products formed upon heating it. ### Step 1: Identify the nature of the products formed upon heating We know that when salt (X) is heated, it decomposes into three products: A, B, and C. Among these: - A is red in hot condition. - B and C are two different paramagnetic gases. ### Step 2: Understand the characteristics of the products - The fact that A is red in hot condition suggests that it could be a metal oxide, as many metal oxides exhibit color changes when heated. - The paramagnetic gases (B and C) indicate that they have unpaired electrons, which is a characteristic of certain nitrogen oxides or oxygen species. ### Step 3: Analyze possible salts We need to consider the common water-soluble salts that can decompose into a red-colored product and two paramagnetic gases upon heating. 1. **Hg(NO3)2**: Decomposes to Hg (liquid) and NO2 (gas). Not red. 2. **FeC2O4**: Decomposes to FeO (black) and CO, CO2 (not gases we want). 3. **ZnSO4**: Decomposes to ZnO (white) and SO2, O2 (not gases we want). 4. **Pb(NO3)2**: Decomposes to PbO (red) and NO2, O2 (paramagnetic gases). ### Step 4: Confirm the correct salt From the analysis: - **Pb(NO3)2** fits all criteria: - A (PbO) is red when hot. - B (NO2) and C (O2) are both paramagnetic gases. ### Conclusion Thus, the water-soluble salt (X) that meets all the criteria given in the question is **Pb(NO3)2**. ### Final Answer The salt (X) is **Pb(NO3)2** (Lead(II) nitrate). ---

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Water soluble salt (x) when heated decomposes into three products A, B and C. Here B and C are two different paramagnetic gases while A is yellow in hot condition Here the salt (x) is

In salts of polyatomic anion, as polarising power of cation increase, thermal stability of the salt decrease and decomposed species may further undergo redox reaction Q. Which of the followinng species undergoes non-redox thermal decomposition reaction on heating?

Salts M, N, O, P and Q undergo reactiom (i) to (v) respectively. Identify the cation present in these salts on the basis of these reaction. Tabulate your answer in the format given below. 1. When sodium hydroxide solution is added to the salt M, and heated strongly a colourless gas with a pungent smell is evolved which turm red litmus paper blue and gives dense white fumes with a moist glass rod with hydrochloric acid. 2. Addition of dilute hydrochloric acid to a solution of N gives a thick white precipitate which is soluble in hot water. 3. When ammonium hydroxide solution is added to the solution of 0 a light blue precipitate is obtained which is soluble in excess of ammonium hydroxide to form an inteme deep blue solution. 4. When ammonium hydroxide solution is added to the solution of P reddish brown (mustard colour) precipitate is obtained which ,is insoluble even in the excess of ammonium hydroxide solution. 5. When sodium hydroxide solution is added to the solution of Q a which coloured gelatinous precipitate is obtained which is soluble in excess of sodium hydroxide to form a clear solution

Salt (A) + lime water to white precipitate darr white precipitate + prolong passage of gas (B) to it forms soluble salt (C ), gas (B) has burning sulphur smell Identify the anion of salt (A) and (C ).

A solution which remains in equilibrium with undissolved solute , in contact , is said to be saturated . The concentration of a saturated solution at a given temperature is a called solubility . The product of concentration of ions in a saturated solution of an electrolyte at a given temperature is called solubility product (K_(sp)) . For the electrolyte A_(x),B_(y) with solubility S. The solubility product (K_(sp)) is given as K_(sp) = x^(x) xx y^(y) xx S^(x-y) . While calculating the solubility of a sparingly . soluable salt in the presence of some strong electrolyte containing a common ion , the common ion concentration is practically equal to that of strong electrolyte containing a common ion . the common ion soncentration is practically equal to that of strong electrolyte . If in a solution , the ionic product of an electroylte exceeds its K_(sp) value at a particular temperature , then precipitation occurs . If two or more electrolyte are presentt in the solution , then by the addition of some suitable reagent , precipitation generally occurs in increasing order of their k_(sp) values . Solubility of some sparingly soluable salts , is sometimes enhanced through complexation . While we are calculating the solubility of some sparingly or pH of an electrolyte , the nature of cation of anion should be checked carefully whether there ion (s) are capable of undergoing hydrolysis or not . If either or both of the ions are capable of undergoing hydrolysis , it should be taken into account in calculating the solubility . While calculating the pH of an amphiprotic species , it should be checked whether or not cation can undergo hydrolysis . Total a_(H^(-)) = sqrt(K_(a_(1)xxK_(a_(2)))) (if cation do not undergo hydrolysis ) a_(H^(+)) = sqrt(K_(a_(1))((K_(w))/(K_(b)) - K_(a_(2)))) (if cation also undergoes hydrolysis ) where symbols have usual meaning . Solubility of solids into liquids is a function of temperature alone but solubility of gases into liquids is a function of temperature as well as pressure . The effect of pressure on solubility of gases into liquids is governed by Henry's law . The solubility of PbSO_(4) in water is 0.0303 g/l at 25^(@)C , its solubility product at that temperature is

A solution which remains in equilibrium with undissolved solute , in contact , is said to be saturated . The concentration of a saturated solution at a given temperature is a called solubility . The product of concentration of ions in a saturated solution of an electrolyte at a given temperature is called solubility product (K_(sp)) . For the electrolyte A_(x),B_(y) with solubility S. The solubility product (K_(sp)) is given as K_(sp) = x^(x) xx y^(y) xx S^(x-y) . While calculating the solubility of a sparingly . soluable salt in the presence of some strong electrolyte containing a common ion , the common ion concentration is practically equal to that of strong electrolyte containing a common ion . the common ion soncentration is practically equal to that of strong electrolyte . If in a solution , the ionic product of an electroylte exceeds its K_(sp) value at a particular temperature , then precipitation occurs . If two or more electrolyte are presentt in the solution , then by the addition of some suitable reagent , precipitation generally occurs in increasing order of their k_(sp) values . Solubility of some sparingly soluable salts , is sometimes enhanced through complexation . While we are calculating the solubility of some sparingly or pH of an electrolyte , the nature of cation of anion should be checked carefully whether there ion (s) are capable of undergoing hydrolysis or not . If either or both of the ions are capable of undergoing hydrolysis , it should be taken into account in calculating the solubility . While calculating the pH of an amphiprotic species , it should be checked whether or not cation can undergo hydrolysis . Total a_(H^(-)) = sqrt(K_(a_(1)xxK_(a_(2)))) (if cation do not undergo hydrolysis ) a_(H^(+)) = sqrt(K_(a_(1))((K_(w))/(K_(b)) - K_(a_(2)))) (if cation also undergoes hydrolysis ) where symbols have usual meaning . Solubility of solids into liquids is a function of temperature alone but solubility of gases into liquids is a function of temperature as well as pressure . The effect of pressure on solubility of gases into liquids is governed by Henry's law . The solubility of BaSO_(4) in 0.1 M BaCl_(2) solution is (K_(sp) " of " BaSO_(4) = 1.5 xx 10^(-9))

The reaction 2AX(g)+2B_(2)(g)rarr A_(2)(g)+2B_(2)X(g) has been studied kinetically and on the baiss of the rate law following mechanism has been proposed. I. 2A X hArr A_(2)X_(2) " " ("fast and reverse") II. A_(2)X_(2)+B_(2)rarrA_(2)X+B_(2)X III. A_(2)X+B_(2)rarrA_(2)+B_(2)X where all the reaction intermediates are gases under ordinary condition. form the above mechanism in which the steps (elementary) differ conisderably in their rates, the rate law is derived uisng the principle that the slowest step is the rate-determining step (RDS) and the rate of any step varies as the Product of the molar concentrations of each reacting speacting species raised to the power equal to their respective stoichiometric coefficients (law of mass action). If a reacting species is solid or pure liquid, its active mass, i.e., molar concentration is taken to be unity, the standard state. In qrder to find out the final rate law of the reaction, the concentration of any intermediate appearing in the rate law of the RDS is substituted in terms of the concentration of the reactant(s) by means of the law of mass action applied on equilibrium step. How many times the rate of formation of A_(2) will increase if concentrations of AX is doubled and that of B_(2) is increased theee fold?

The reaction 2AX(g)+2B_(2)(g)rarr A_(2)(g)+2B_(2)X(g) has been studied kinetically and on the baiss of the rate law following mechanism has been proposed. I. 2A X hArr A_(2)X_(2) " " ("fast and reverse") II. A_(2)X_(2)+B_(2)rarrA_(2)X+B_(2)X III. A_(2)X+B_(2)rarrA_(2)+B_(2)X where all the reaction intermediates are gases under ordinary condition. form the above mechanism in which the steps (elementary) differ conisderably in their rates, the rate law is derived uisng the principle that the slowest step is the rate-determining step (RDS) and the rate of any step varies as the Product of the molar concentrations of each reacting speacting species raised to the power equal to their respective stoichiometric coefficients (law of mass action). If a reacting species is solid or pure liquid, its active mass, i.e., molar concentration is taken to be unity, the standard state. In qrder to find out the final rate law of the reaction, the concentration of any intermediate appearing in the rate law of the RDS is substituted in terms of the concentration of the reactant(s) by means of the law of mass action applied on equilibrium step. Let the equilibrium constant of Step I be 2xx10^(-3) mol^(-1) L and the rate constants for the formation of A_(2)X and A_(2) in Step II and III are 3.0xx10^(-2) mol^(-1) L min^(-1) and 1xx10^(3) mol^(-1) L min^(-1) (all data at 25^(@)C) , then what is the overall rate constant (mol^(-2) L^(2) min^(-1)) of the consumption of B_(2) ?

Consider three P, Q, R, salts among them P and Q salts have different cations annd also have different coloured polyatomic anion due to charge transfer phenomenon while P and R salts have same cation but have different anions. Salts R decomposes into an acidic gas an a basic gas. Q. Salt P decomposes on heating into a coloured solid, neutral gas a neutral vapour, then which of the following can not be the product of salt P after decomposition?

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