`100cm^3` of a solution of an acid (Molar mass `=98`) containing `29.4g` of the acid per litre were completely neutralized by `90.0 cm^3` of aq. `NaOH` containing `20g` of `NaOH` per `500cm^3`. The basicity of the acid is :

0.45 g of acid (mol. Wt. =90 ) was exactly neutralized by 20 ml of 0.5(M) NaOH . The basicity of the given acid is

0.45g of an acid of mol. Mass 90 was neutralised by 20mL of 0.5 N caustic potash (KOH) . The basicity of acid is :

1.25g of a solid dibasic acid is completely neutralised by 25mL of 0.25 molar Ba (OH)_2 solution. Molecular mass of the acid is :

Calculate the molarity of a solution containing 0.5 g of NaOH dissolved in 500 "cm"^(3) of the solution?

A given solution of NaOH contains 4.00 g of NaOH per litre of solution. Calculate the molarity of this solution .

4.0 g of NaOH are contained in one declitre of a solution. Calculate molarity of NaOH

An aqueous solution of 0.5 g of NaOH is dissolved in 500 cm^3 of the solution. The molarity of the solution will be :

A solution containing 500 g of a protein per liter is isotonic with a solution containing 3.42 g sucrose per liter. The molecular mass of protein in 5 x 10^(x) , hence x is.

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) If enthalpy of neutralization of CH_(3)COOH by NaOH is -49.86KJ // mol then enthalpy of ionization of CH_(3)COOH is:

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) ?