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explain why cp is always greater than cv????

Given : Kb($Cl{C}_{6}{H}_{4}N{H}_{2}$) = 4 x ${10}^{-13}$, log 19 = 1.3, log 2 = 0.3, $\sqrt{16.25}$=4.02

(A) 2.1

(B) 2.5

(C) 3.5

(D) 3.1

why oxygen is paramagnetic in nature by molecular orbital theory

what is the conjugate base of CN

^{- }what is physical equilibrium? Give two example

Equal volumes of two solutions pH=2 and pH=4 are mixed together.Calculate the pH of the resulting solution?

NO3- , NO2- NO2. and NO2+

plz answer me soon and explain

_{}2 NO(g) + Br_{2}(g) . If P_{Br2}_{}= P/9 at equilibrium and P is total pressure, the ratio of Kp/P is equal to(The ones marked in blue, those steps I couldn't understand , please explain it )the value of Kc = 4.24 at 800K for the reaction

CO(g) + H2O(g) CO2(g) + H2(g)

Calculate the equilibrium concentration of CO2 ,H2O ,CO , H2 at 800K ,if only CO and H2O are pesent initially at concentration of 0.10M each.

(1) NH

_{4}OH + NaOH(2) HCOOH + CH

_{3}COONa(3) 40 mL 0.1 M NaCN + 20 mL of 0.1 M HCl

(4) None of them

100 ml of 0.1 N NaOH is mixed with 100 ml of 0.1 N H

_{2}SO_{4}.The pH of the resultant solution is??_{b }of NH3 is 4.74In a closed system:A

_{(s)}⇌2B_{(g)+}3C_{(g)}if the partial pressure of C is doubled then partial pressure of B will be??Is SnCl_{4}a Lewis acid or a base???Arrange the following Bronsted Acids in increasing acidic strength,Give Reason for your choice :1)HCl,HBr ,HI,CH_{3}COOH,HCO_{3},H_{2}O2)HCOOH,C_{6}H_{5}COOH,CH_{3}COOH49) Which oxychloride has maximum pH?

a) NaClO b) NaClO

_{2}c) NaClO_{3}d) NaClO_{4}88) A infinite dilution the percentage ionisation for both the strong and weak electrolyes is:

a) 1% b)20% c)50% d) 100%

increase

decrease

unchanged

none

What is the pH of 10

^{-8}M HCl solution?how to solve x = antilog (-5.4)

At 90'C, pure water has [H30

^{+}]=10^{-6}mole/liter. the value of k_{W}at 90'C is:^{-6}^{-8}^{-12}^{-14}_{5}is 50% dissociated at an equilibrium pressure of 4 atm. At what pressure it would dissociate to the extent of 80% at the same temperature:-a) 0.05 atm

b) 0.60 atm

c) 0.75 atm

d) 2.50 atm

Kindly answer sir/mam.

Question -The pH of 0.1 M monobasic acid is 4.50. Calculate the concentration of H+, A- and HA. Also determine the values of ka and pka of mono basic acid._{4}(g) is attained by mixing equal moles of A and B in a one litre vessel. Then at equilibrium:- (Kindly explain the answer also)a) [A] = [B]

b) [A] > [B]

c) [A] < [B]

d) [AB

_{4}] > [A]Kindly answer sir/mam.

The pH of a solution obtained by mixing 100 ml of 0.2 M CH

_{3}COOH with 100 ml of 0.2 M NaOH will be??(given pK_{a}for CH_{3}COOH =4.74 and log 2=0.301)Is studying Chemical Kinetics necessary for understanding The chapters of Equlibrium? Namelsy, Ionic and Chemical?My seniors told me that it would be of help for me to go through the Chemical Kinetics chapter before I start with Ionic Equilibrium!Thanks in advance!

what is the formula and basicity of hydrated oxalic acid and anhydrous oxalic acid?

The following reactions are known to occur in the body

CO

_{2}+H_{2}O⇌H_{2}CO3⇌H^{+}+HCO3What will happen if CO

_{2}escapes from the system??_{p}) are related as ${\mathrm{K}}_{\mathrm{p}}=\frac{4{\mathrm{\alpha}}^{2}\mathrm{P}}{\left(1-{\mathrm{\alpha}}^{2}\right)}$?(1) ${\mathrm{N}}_{2}{\mathrm{O}}_{4}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_{2}\left(\mathrm{g}\right)$

(2) ${\mathrm{H}}_{2}\left(\mathrm{g}\right)+{\mathrm{I}}_{2}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)$

(3) ${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$

(4) ${\mathrm{PCl}}_{3}\left(\mathrm{g}\right)+{\mathrm{Cl}}_{2}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_{5}\left(\mathrm{g}\right)$

K

_{sp}of Mg(OH)_{2 }is 4.0×10^{-12}.The number of moles of Mg^{2+}ions in one litre of its saturated solution in 0.1 M NaOH is??2SO2 + O2 ------> 2SO3

has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the reaction at the same temperature

SO3 -----> SO2+ ½O2

what is the pH of solution when 0.2 mole of NaOH is added to one litre of a solution containing one mole each of NH3 and NH4Cl?

Kb for NH3 is 1.8 * 10 ^-5. assume the total volume remains one litre

Q] One mole of N

_{2}O_{4}(g) at 300K is kept in a closed container under one atmosphere. It is heated to 600K when 20% by mass of N_{2}O_{4}(g) decomposes to NO_{2}(g). The resultant pressure is??_{v.m}= a + bT, where a = 25.0 J/(mol. K) and b = 0.03 J (mol. K^{2}). Let 2 mole of the gas go from 300 K and 2.0 litre volume to 600 K and 4.0 litre. ΔS_{gas}is(1) 32.08 J/K (2) –12.08 J/K (3) 64.17 J/K (4) None of these

If the value of Kc is 3, the percentage by mass of iso-butanein the equilibriummixture would be:-

a) 75%

b) 90%

c) 30%

d) 60%

Kindly answer sir/mam.

The solubility of salts of weak acids increases at lower pH. Can you explain the derivation in textbook?

Calculate the degree of ionization of 0.01M solution of HCN.Ka = 4.8 X 10-10.Also calculate H

^{+ }ion concentration of the solution^{}^{}Q25. In a 7.0 l, evacuated chamber, 0.50 mol H

_{2}and 0.50 mol l_{2}react at 427$\xb0$C.H

_{2}(g) + l_{2}(g) $\underset{}{\overset{}{\rightleftharpoons}}$ 2HI (g). At the given temperature, K_{c}= 49 for the reaction.(i) What is the total pressure (atm) in the chamber?

(A) 83.14 (B) 831.4 (C) 8.21 (D) None

(ii) What is the value of K

_{p}?(A) 7 (B) 49 (C) 24.5 (D) None

(iii) How many moles of the iodine remain unreacted at equilibrium ?

(A) 0.388 (B) 0.112 (C) 0.25 (D) 0.125

(iv) What is the partial pressure (atm ) of Hl in the equilibrium mixture ?

(A) 6.385 (B) 12.77 (C) 40.768 (D) 646.58

the dissociation of H

_{2}S is suppresed by the presence of HCl explain whycalculate simultaneous solubility of AgCNS and AgBr in a solution of water.Ksp AgCNS=1.2*10

^{-12},Ksp AgBr=5*10^{-13}the value of delta G for the phosphorylation of glucose in glycolysis is 13.8 kj/mol. Find the value of Kc at 298K?

The solubility product constant of Ag

_{2}CrO_{4}and AgBr are 1.1 × 10^{–12}and 5.0 × 10^{–13}respectively. Calculate the ratio of the molarities of their saturated solutions.whats the basic difference between concentration and composition?

ARE ALL SALTS STRONG ELECTROLYTES OR THERE ARE SOME WEAK ELECTROLYTES WHICH ARE SALTS?

H2(g)+I2(g)2HI(g)

at 720K is 48. What is the value of the equilibrium constant for the reaction

1/2H2(g)+1/2I2(g)HI(g)

At temperature T, a compound AB

_{2}(g) diassociates according to the reaction :2AB

_{2}(g) [reverisble sign ] 2AB(g) + B_{2}.with degree of dissociation, x, which is small compared to unity. Deduce the expression for x in terms of equillibrium constant K

_{p}and the total pressure.The equilibrium constants K

_{P1}and K_{P2}for the reactions X↔2Y and Z↔P +Q, respectively are in the ratio of 1 : 9. If the degree of dissociation of X and Z be equal then the ratio of total pressure at these equilibria isWhat is an evacuated vessel? [From Comprehensive Chemistry Pg.-370]

18. The correct- order of acidic strength is

$\left(1\right){\mathrm{CH}}_{3}\mathrm{COOH}\mathrm{HCN}{\mathrm{H}}_{2}\mathrm{O}{\mathrm{C}}_{2}{\mathrm{H}}_{5}\mathrm{OH}\phantom{\rule{0ex}{0ex}}\left(2\right){\mathrm{CH}}_{3}\mathrm{COOH}\mathrm{HCN}{\mathrm{H}}_{2}\mathrm{O}{\mathrm{C}}_{2}{\mathrm{H}}_{5}\mathrm{OH}\phantom{\rule{0ex}{0ex}}\left(3\right)\mathrm{HCN}{\mathrm{CH}}_{3}\mathrm{COOH}{\mathrm{H}}_{2}\mathrm{O}{\mathrm{C}}_{2}{\mathrm{H}}_{5}\mathrm{OH}\phantom{\rule{0ex}{0ex}}\left(4\right){\mathrm{CH}}_{3}\mathrm{COOH}\mathrm{HCN}{\mathrm{C}}_{2}{\mathrm{H}}_{5}\mathrm{OH}{\mathrm{H}}_{2}\mathrm{O}$

When 0.1 mole of ammonia is dissolved in sufficient water to make 1 litre of solution.The solution is found to have a hydroxide ion concentration of 1.34×10

^{-3}.The dissociaton constant of ammonia is??Ksp(BaSO4)= 1.5*10-9. find solubility in a)pure water b)0.1 M BaCl2 solution

^{+3}+ SCN^{-}-----> [Fe(SCN)]^{+2}?(ii) what happens to the intensity of blood red colour if Hg is added to the above reaction ?

reached, concentration of C was thrice the equilibrium concentration of B. Calculate KC.

1)- What is the pH of10

^{-8}(N) HCl?46) A sample of Na2CO3.H2O weighing 0.62g is added to 100ml of 0.1N H2SO4 solution. What will be the resulting solution

a) Acidic b) NEUTRAL c) BASIC

CO (g) + 1/2 O2 equlibrium equal is Co2 (g) is

How CH3COONa is a strong electrolyte?

an excess of agno3 is added to 100 ml of a 0.01 M solution of [cr(h2o)4cl2]cl.the number of agcl precipated would be:

is this question based on common ion effect

The dissociation constant of a weak acid HA and weak base BOH are 2×10

^{-5}and 5×10^{-6 }respectively.The equilibrium constant for the neutralization reaction of the two is ( ignore hydrolysis of resulting salt)N${H}_{4}$HS(s) $\rightleftharpoons $N${H}_{3}$(g) + ${H}_{2}$S(g) ; $\u25b3$H = +ve

${S}_{1}$ : On increase in temperature, equilibrium pressure of ammonia increases.

${S}_{2}$ : On increase in volume of container at constant temperature, equilibrium pressure of ammonia

increases.

${S}_{3}$ : On increase in mass of N${H}_{4}$HS(s) in the container at constant temperature, equilibrium pressure of

ammonia increases.

the equilibrium constant kp= 2.9*10^ -5 atm^3. the total pressure of gases at equilibrium when 1.0 mole of reactant was heated will be

calculate the PH of a 0.1 M ammonia solution. Calculate the pH after 50 ml of this solution is treated with 25ml of 0.1 HCl. the dissociation constant of ammonia K

_{b}= 1.77 x 10^{-5 }.plz explain me ostwald dilution law

^{-}calculate the pH of 1.0 X 10^ -8 M solution of HCL ?