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The enthalpy of neutralization of three ...

The enthalpy of neutralization of three weak bases
`BOH`, `B'OH` and `B"OH` are `-40.08`, `-36.62` and `-51.82kj//gram-`equilvalent with HCl.
The correct order of their basec srength is `:-`

A

`B'OHltBOHltB''OH`

B

`BOHltB'OHltB''OH`

C

`B'OHltB''OHltBOH`

D

`B''OHltBOHltB'OH`

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The correct Answer is:
A
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The enthalpy of neutraliztion of weak base A OH and a strong base BOH by HCl are -12250 cal/mol and -13000 cal/mol respectively . When one mole of HCl is added to a solution containting 1 mole of A OH and 1 mole of BOH , the enthalpy change was -12500 cal/mol . In what ratio is the acid distribution between A OH and BOH?

Enthalpy of neutralization of HCl by NaOH is -55.84 kJ/mol and by NH_(4)OH is -51.34 kJ/mol. The enthalpy of ionization of NH_(4)OH is :

Assertion(A) : The value of enthalpy of neutralization of a weak acid by strong base is numerically less than 57.1 kJ . Reason(R ) : All OH^(-) ions of strong base are not completely neutralized by H^(+) ions obtained from acid.

Enthalpy of neutralzation is defined as the enthalpy change when 1 mole of acid /base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) What is DeltaH^(@) for complate neutralization of strong diacidic base A(OH)_(2)by HNO_(3) ?

Enthalpy of neutralization is defined as the enthalpy change when 1 mole of acid / / base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) If enthalpy of neutralization of CH_(3)COOH by NaOH is -49.86KJ // mol then enthalpy of ionization of CH_(3)COOH is: (a)5.98 kJ/mol (b) -5.98 kJ/mol (c)105.7 kJ/mol (d)None of these

Enthalpy of neutralzation is defined as the enthalpy change when 1 mole of acid // base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) under same conditions ,how many mL of 0.1 m NaOH and 0.05 M H_(2)A (strong diprotic acid ) solution should be mixed for a total volume of 100mL to producce the hight rise in temperature ?

Enthalpy of neutralization of HCl by NaOH is -57.1 J//mol and by NH_(4)OH is -51.1 KJ//mol . Calculate the enthalpy of dissociation of NH_(4)OH .

All the boron trihalides except BI_(3) may be prepared by direction between the elements. Boron trihalides consist of trigonal-planar BX_(3) molecules. Unlike the halides of the other elements in the group they are monomeric in the gas, liquid and solid states, BF_(3) and BCl_(3) are gases, BBr_(3) is a volatile liquid and BI_(3) is a solid. Boron trihalides are Lewis acids because they form simple Lewis complexes with suitable bases, as in the reaction: BF_(3)(g)+NH_(3)(g)toF_(3)B-NH_(3)(s) However, boron chlorides, bromides and iodides are susceptible (sensitive) to protolysis by mild proton sources such as water, alcohols and even amines, for example BCl_(3) undergoes rapid hydrolysis: BCl_(3)(g)+3H_(2)O(l)toB(OH)_(3)(aq)+3HCl (aq) It is supposed that the first step in the above reaction is the formation of the complex Cl_(3)B larr OH_(2) which then eliminates HCl and reacts with water. Which of the follwoing is the best order of Lewis acid strength of BF_(3),BCl_(3) and BBr_(3) ?

When a salt reacts with water to form acidic or basic solution , the process is called hydrolysis . The pH of salt solution can be calculated using the following relations : pH = 1/2 [pK_(w) +pK_(a) + logc] (for salt of weak acid and strong base .) pH = 1/2 [pK_(w) - pK_(b) - logc] (for salt of weak base and strong acid ) . pH = 1/2 [ pK_(w)+pK_(a)-pK_(b)] (for weak acid and weak base ). where 'c' represents the concentration of salt . When a weak acid or a weak base not completely neutralized by strong base or strong acid respectively , then formation of buffer takes place . The pH of buffer solution can be calculated using the following relation : pH = pK_(a) + log . (["Salt"])/(["Acid"]) , pOH = pK_(b) + log . (["Salt"])/([ "Base"]) Answer the following questions using the following data : pK_(a) = 4.7447 , pK_(b) = 4.7447 ,pK_(w) = 14 When 100 mL of 0.1 M NH_(4)OH is added to 50 mL of 0.1M HCl solution , the pH is

Salt hydrolysis is an acid - base reaction of cation or anion or both ions of salt with water . The resultant solution after hydrolysis may be acidic , basic or neutral . The anion X^(-) which is weaker base than OH^(-) and which has its conjugate acid HX stronger than water but weaker than H_(3)O^(+) shows the phenomenon of hydrolysis , e.g CH_(3)COO^(-) , NO_(2)^(-) , CN^(-) etc. The cation M^(+) which is weaker acid than H_(3)O^(+) and which has its conjugate base MOH stronger than water but weaker than OH^(-) shows the phenomenon of hydrolysis , e.g N_(2)H_(5)^(+), C_(6)H_(5)NH^(+),NH_(4)^(+) etc . The degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 0.1 .If the molarity of the solution is 0.05 M , the percentage hydrolysis of salt should be :

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